Enthalpy of Reaction and Calorimetry worksheet

Size: px
Start display at page:

Download "Enthalpy of Reaction and Calorimetry worksheet"

Transcription

1 Enthalpy of Reaction and Calorimetry worksheet 1. Calcium carbonate decomposes at high temperature to form carbon dioxide and calcium oxide, calculate the enthalpy of reaction. CaCO 3 CO 2 + CaO 2. Carbon tetrachloride can be formed by reacting chlorine with methane, calculate the enthalpy of reaction. CH Cl 2 CCl H 2 3. When potassium chloride reacts with oxygen under the right conditions, potassium chlorate is formed: 2 KCl + 3 O 2 2KClO 3 Given that the enthalpy of formation of potassium chloride is kj/mol and the enthalpy of formation of potassium chlorate is kj/mol, determine the enthalpy of reaction. Calorimetry Practice 4. Compound A is burned in a bomb calorimeter that contains 2.50 liters of water. If the combustion of moles of this compound causes the temperature of the water to rise C, what is the molar heat of combustion of compound A? 5. Compound B is burned in a bomb calorimeter that contains 1.50 liters of water. When I burned 50.0 grams of compound B in the calorimeter, the temperature rise of the water in the calorimeter was C. If the heat of combustion of compound B is 2,150 kj/mol, what is the molar mass of compound B? 6. The molar heat of combustion of compound C is 1,250 kj/mol. If I were to burn moles of this compound in a bomb calorimeter with a reservoir that holds 2.50 L of water, what would the expected temperature increase be?

2 INV MOLAR ENTHALPY of SOLUTION - MEDICAL COLD PACKS Part 2 1. Describe the difference between heat and temperature. 2. For the compounds used in this experiment ( Nelson Chemistry 12 p. 347): (a) Calculate the number of moles present in a g sample. (b) Calculate the molar enthalpy (c) Write the thermochemical chemical equation for your compound's dissociation in water. 3. (a) When a substance dissolves its heat content, or enthalpy, will either increase or decrease. This change in enthalpy is observed as a change in temperature of the water in the calorimeter. Sketch a graph showing the change in enthalpy for the dissolving of an ionic compound which is: (b) For your compound, state whether the dissolving was an endothermic or exothermic process. (c) Will the sign for _H in your case be positive or negative? 4. Describe two factors that affect the strength of an ionic bond in a compound. 5. (a) Define crystal lattice energy and hydration energy. (b) Which of the properties in part (a) reduces the solubility of an ionic compound? (c) Which property, when increased, increases the solubility? 6. For an ionic solid to melt, external energy must be applied to overcome the attractive forces holding its ions together. For example, sodium hydroxide must be heated to temperatures exceeding 318 C for it to melt. Despite such a high melting point, sodium hydroxide readily and exothermally dissolves and dissociates into its ions in water at room temperature. (a) What is the source of the energy required to separate the ions from the solid sodium hydroxide? (b) Why does the resulting sodium hydroxide solution feel hot? 7. Ammonium chloride is also soluble despite having a melting point of 320 C. Why does an ammonium chloride solution feel cold to the touch? 8. Magnesium oxide, MgO, and magnesium chloride, MgCl 2, are very similar, white, ionic solids with the following properties: Compound Melting Point Solubility MgO 2800 C insoluble MgCl C very soluble (a) Give the formula of the ions of each compound. (b) Account for the drastic difference in physical properties. 9. Consider the following data from the Group 1 chlorides. These compounds are similar in structure, each being formed from a + cation and the -1 chloride ion. However, they are quite different with respect to lattice energy, hydration energy, and enthalpy of solution. Explain these differences. Substance Lattice Energy (kj/mol) Hydration Energy (kj/mol) Enthalpy of Solution (kj/mol) LiCl NaCl KCI

3 Heats of Reaction Using the Standard values of Η f, calculate the heats of reaction, ΔΗ rxn, or heats of formation, ΔΗ f All answers must include the intermediate steps with the formation reaction from the elements and their manipulation to form the overall reaction. For #1-6, the equation: ΔHo rxn = ΣnΔHo products ΣnΔHo reactants eg. SO 2(g) + H 2 O (l) H 2 SO 4(aq) H kj (1) 1/8 S 8 + O 2 _ SO (2) H 2 + 1/2 O 2 _ H 2 O (3) H 2 + 1/2 O 2 + 1/8 S 8 _ H 2 SO Then multiply or reverse, whatever is needed so that they add to the original reaction. 1. C 6 H 6 (l) + 15/2 O 2 (g) 6 CO 2 (g) + 3 H 2 O (g) CANNOT BE USED HNO 3 (aq) + NO (g) 3 NO 2 (g) + H 2 O (l) 3. C 2 H 2 (g) + C 2 H 6 (g) 2 C 2 H 4 (g) 4. PbO 2 (s) + CO (g) PbO (s) + CO 2 (g) 5. Al 2 (SO 4 ) 3 (s) + 3 H 2 O (l) Al 2 O 3 (s) + 3 H 2 SO 4 (aq) 6. 3 SO 2 (s) + 2 HNO 3 (aq) + 2 H 2 O (l) 3 H 2 SO 4 (aq) + 2 NO (g) 7. Given that H rxn = kj for the following, calculate the H f for ClF 3 (g). 2 ClF 3 (g) + 2 NH 3 (g) N 2 (g) + 6 HF (g) + Cl 2 (g) 8. Given that H rxn = kj for the following, calculate the H f for HNO 2 (g). HNO 2 (g) + 1/2 O 2 (g) HNO 3 (aq) 9. Given that H rxn = kj for the following, calculate the H f for Fe(CO) 5 (g). Fe 2 O 3 (s) + 13 CO (g) 2 Fe(CO) 5 (g) + 3 CO 2 (g) 10. Given that H rxn = kj for the following, calculate the H f for Fe 3 O 4 (s). 2 Fe 3 O 4 (s) + CO 2 (g) 3 Fe 2 O 3 (s) + CO (g)

4 Practice Thermochemistry Questions 1. a) Urea (from urine) hydrolyzes slowly in the presence of water to produce ammonia and carbon dioxide. What is the standard H, S and G for this reaction when 1 mole of urea reacts with water? b) What is the spontaneity of this reaction? 2. What is G for the combustion of liquid ethyl alcohol (C 2 H 5 OH) to give CO 2(g) and H 2 O (g)? Is the reaction spontaneous? 3. Calculate H and S for the following reaction and decide in which direction each of these factors will drive the reaction. N 2(g) + 3 H 2(g) 2 NH 3(g) Use the data given below to answer your questions: Compound H (kj/mol) S (J/(mol K)) G (kj/(mol K)) CO(NH 2 ) 2(aq) H 2 O (l) CO 2(g) NH 3(g) C 2 H 5 OH (l) H 2 O (g) N 2 (g) H 2 (g)

5 SUPPLEMENTARY ENTHALPY PROBLEMS 1. Construct an enthalpy diagram showing the enthalpy changes for a one step conversion of germanium, Ge(s), into GeO2 (s) and a two step conversion - first to the monoxide, GeO(s) followed by the oxidation to GeO2 (s). The relevant thermochemical equations are as follows; Ge(s) + 1/2 O2 (g) GeO(s) H = -255 kj Ge(s) + O2(g) GeO2 (s) H = kj Using this diagram, determine the value of H for the reaction GeO(s) + 1/2 O2 (g) GeO2 (s) 2. Nitrogen monoxide oxidizes to the toxic red brown gas nitrogen dioxide in air. Construct an accurate enthalpy diagram for this reaction. Use the diagram to explain which of the oxides of nitrogen has stronger covalent bonds. 2 NO(g) + O2 (g) 2 NO2 (g) 3. One of the building blocks for proteins such as those in muscles and in sinews, is an amino acid called glycine, C2H5NO2. The equation for its combustion is 4 C2H5NO2 (s) + 9 O2 (g) 8 CO2 (g) + 10 H2O(l) + 2 N2 (g) The value of its H comb is kj/mol. Calculate H f for glycine. 4. On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near Denver, Colorado. The spill was neutralized with sodium carbonate. The reaction is 2 HNO3 (aq) + Na2CO3 (s) 2 NaNO3 (aq) + H2O(l) + CO2 (g) (a)calculate H for this reaction. H f for NaNO3 (aq) is -467 kj/mol, H f for HNO3 (aq) is kj/mol, H f for Na2CO3 (aq) is kj/mol] (b) Approximately 9.1 x 10 4 L of nitric acid was spilled. Assuming a molar concentration of 15.4M, how much sodium carbonate was required for complete neutralization and how much heat was evolved. (c) According to the Denver Post for April 4, 1983, authorities feared a volatile reaction might occur during the neutralization. Considering the magnitude of H, what was their major concern? The large amount of heat energy released in this neutralization reaction could cause the decomposition of the nitrate compounds into toxic oxides of nitrogen.

6 Supplementary Thermochemistry Problems 1. a) Calculate the enthalpy change, ΔH rxn, for the following reaction using equations 1, 2 and 3. Given: FeO + CO Fe + CO 2 ΔH rxn (kj) 1) Fe 2 O CO 2 Fe + 3 CO ) 3 Fe 2 O 3 + CO 2 Fe 3 O 4 + CO ) Fe 3 O 4 + CO 3 FeO + CO Calculate the enthalpy change, ΔH rxn, for the following reaction using equations 1, 2 and 3. Given: 3 N 2 H ClF 3 3 N HF + 2 Cl 2 ΔH rxn (kj) 1) 2 ClF NH 3 N HF + Cl ) N 2 H 4 + O 2 N H 2 O ) 4 NH O 2 2 N H 2 O Calculate the enthalpy change, ΔH rxn, for the following reaction using equations 1, 2 and 3. Given: 2 H 3 BO 3 B 2 O H 2 O ΔH rxn (kj) 1) H 3 BO 3 HBO 2 + H 2 O ) 2 B 2 O 3 + H 2 O H 2 B 4 O ) H 2 B 4 O 7 + H 2 O 4 HBO Using the average bond energies, N N (941 kj/mol), N=N (418 kj/mol), N-N (160 kj/mol), N-H (391 kj/mol) and H-H (432 kj/mol) estimate the ΔH f for hydrazine, N 2 H The ΔH rxn of the gaseous reaction: XeF 2 + H 2 2 HF + Xe is found to be 430 kj. Use this value and average bond energies [H-F (565 kj/mol)] to determine the average bond energy of the Xe-F bond.

7 1. For the following reaction, KINETICS Rate Mechanisms and the RDS NO (g) + O 3 (g) NO 2 (g) + O 2 (g) Given: E a(forward) = 10.0 kj/mol and ΔH (forward) = kj/mol a) Draw the energy level diagram for this reversible reaction. b) Calculate the E a(reverse) and the ΔH (reverse). For the reaction the following data was obtained: Trial [O 3 ] i (mol / L) [NO] i (mol / L) Initial Rate of Formation of NO 2 (mol / L s) x x x c) What is the rate law for the reaction? d) The proposed mechanism is 3-step. The 1 st is the RDS producing O and NO 3, which are both rxn intermediates. Derive the other 2 elementary steps for the mechanism. 2. Propose a mechanism for the chain reaction: H 2 (g) + I 2 (g) 2 HI (g) Where, I, is a catalyst. Label each step as either chain initiation, propagation or termination. 3. For the reaction: 2 NO (g) + Br 2 (g) 2 NOBr (g) the following data was obtained: Trial [NO] i (mol / L) [Br 2 ] i (mol / L) Initial Rate of Formation of NOBr (mol / L s) x x x 10-4 a) Write the rate law equation that is consistent with the data. b) Calculate the value of the specific rate constant, k, and specify units. c) The following mechanism was proposed for the reaction: Br 2 (g) + NO (g) NOBr 2 (g) slow NOBr 2 (g) + NO (g) 2 NOBr (g) fast Is this mechanism consistent with the given experimental observations? Justify your answer. 4. Propose a mechanism for the chain reaction: H 2 (g) + I 2 (g) 2 HI (g) Where, I, is a reaction intermediate. Label each step as either chain initiation, propagation or termination.

8 5. The reaction: NO 2 (g) + CO (g) NO (g) + CO 2 (g) is believed to occur by the following reaction mechanism: NO 2 (g) + NO 2 (g) NO 3 (g) + NO (g) ( slow ) NO 3 (g) + CO (g) NO 2 (g) + CO 2 (g) ( fast ) a) What is the rate law according to this mechanism? b) What would be the rate law if the reaction occurred directly in a single step? 6. Draw an energy level diagram for: X + Y Z using the following information: a) The reaction is reversible b) The reaction consists of three elementary steps c) The rate determining step is the second step d) The forward reaction is endothermic e) The E a is twice the H for the forward reaction.

9 KINETICS - REVIEW 1. At high temperatures, the following reaction occurs: 4 NH 3 (g) + 5 O 2 (g) 4 NO (g) + 6 H 2 O (g) One experiment showed a concentration of ammonia of mol/l at 10 s and of mol/l at 55 s. Calculate the average rate, over this time interval, for each of the following: a) the rate of decomposition of NH 3. b) the rate of production of water. c) the rate of production of NO. d) the rate of consumption of oxygen. 2. For the following reactions, For the following reaction and its reverse activation energies were determined as follows: C2H4(g) + H2 (g) C2H6(g) Ea = 180 kj/mol C2H6(g) C2H4(g) + H2(g) Ea = 317 kj/mol Calculate H for the reaction of C2H4 with hydrogen 3. For the reaction: 2 A + 2 B C + D The following data about the reaction above were obtained from three experiments: Experiment [A] mol/l [B] mol/l Rate of Formation of C (mol/l min) x x x10-4 a) What is the rate equation for the reaction? b) What is the numerical value of the rate constant k? What are its dimensions? c) Propose a reaction mechanism for this reaction.

10 A + A + B A 2 B A 2 B + B A 2 + B 2 Then 2 A + 2 B A 2 (or C) + B 2 (or D) 4. The following results were obtained when the reaction represented below was studied at 25 C ClO 2(g) + F 2(g) 2 ClO 2 F (g) Experiment [ClO 2 ] i (mol/l) [F 2 ] i (mol/l) Rate of Increase of [ClO 2 F] i (mol/l s) x x x10-3 a) Write the rate law expression for the reaction above. b) Calculate the numerical value of the rate constant and specify the units. c) In experiment 2, what is the initial rate of decrease of [F 2 ]? d) Which of the following reaction mechanisms is consistent with the rate law developed in (a). Justify your choice. I. ClO 2 + F 2 ClO 2 F 2 (fast) ClO 2 F 2 ClO 2 F + F (slow) ClO 2 + F ClO 2 F (fast) II. F 2 2 F (slow) 2 (ClO 2 + F ClO 2 F) (fast) 5. Freon gases, e.g. CCl 2 F 2 (g), from leaking air conditioners and refrigeration units also make their way into the upper atmosphere.. These gases catalyze the destruction of ozone. CCl 2 F 2 (g) + O 3 (g) CClF 2 (g) + ClO (g) + O 2 (g) Where, Cl, is a reaction intermediate. Propose a mechanism for this reaction.

11 6. Draw a potential energy diagram for the reaction X + Y Z showing the following information. (a) The mechanism consists of two elementary steps. (b) The second elementary step is the rate-determining step. (c) The overall reaction is exothermic. (d) What would happen to the shape of the graph if a catalyst were added?

87 16 70 20 58 24 44 32 35 40 29 48 (a) graph Y versus X (b) graph Y versus 1/X

87 16 70 20 58 24 44 32 35 40 29 48 (a) graph Y versus X (b) graph Y versus 1/X HOMEWORK 5A Barometer; Boyle s Law 1. The pressure of the first two gases below is determined with a manometer that is filled with mercury (density = 13.6 g/ml). The pressure of the last two gases below

More information

SUGGESTION ANSWER SCHEME CHAPTER 8: THERMOCHEMISTRY. 1 (a) Use the data in the table below to answer the following questions:

SUGGESTION ANSWER SCHEME CHAPTER 8: THERMOCHEMISTRY. 1 (a) Use the data in the table below to answer the following questions: SUGGESTION ANSWER SCHEME CHAPTER 8: THERMOCHEMISTRY ANSWER SCHEME UPS 2004/2005 SK027 1 (a) Use the data in the table below to answer the following questions: Enthalpy change ΔH (kj/mol) Atomization energy

More information

www.chemsheets.co.uk 17-Jul-12 Chemsheets A2 033 1

www.chemsheets.co.uk 17-Jul-12 Chemsheets A2 033 1 www.chemsheets.co.uk 17-Jul-12 Chemsheets A2 033 1 AS THERMODYNAMICS REVISION What is enthalpy? It is a measure of the heat content of a substance Enthalpy change ( H) = Change in heat content at constant

More information

Problem Solving. Stoichiometry of Gases

Problem Solving. Stoichiometry of Gases Skills Worksheet Problem Solving Stoichiometry of Gases Now that you have worked with relationships among moles, mass, and volumes of gases, you can easily put these to work in stoichiometry calculations.

More information

Chapter 8: Chemical Equations and Reactions

Chapter 8: Chemical Equations and Reactions Chapter 8: Chemical Equations and Reactions I. Describing Chemical Reactions A. A chemical reaction is the process by which one or more substances are changed into one or more different substances. A chemical

More information

Unit 3 Notepack Chapter 7 Chemical Quantities Qualifier for Test

Unit 3 Notepack Chapter 7 Chemical Quantities Qualifier for Test Unit 3 Notepack Chapter 7 Chemical Quantities Qualifier for Test NAME Section 7.1 The Mole: A Measurement of Matter A. What is a mole? 1. Chemistry is a quantitative science. What does this term mean?

More information

Bomb Calorimetry. Example 4. Energy and Enthalpy

Bomb Calorimetry. Example 4. Energy and Enthalpy Bomb Calorimetry constant volume often used for combustion reactions heat released by reaction is absorbed by calorimeter contents need heat capacity of calorimeter q cal = q rxn = q bomb + q water Example

More information

Chemistry: Chemical Equations

Chemistry: Chemical Equations Chemistry: Chemical Equations Write a balanced chemical equation for each word equation. Include the phase of each substance in the equation. Classify the reaction as synthesis, decomposition, single replacement,

More information

Test Review # 9. Chemistry R: Form TR9.13A

Test Review # 9. Chemistry R: Form TR9.13A Chemistry R: Form TR9.13A TEST 9 REVIEW Name Date Period Test Review # 9 Collision theory. In order for a reaction to occur, particles of the reactant must collide. Not all collisions cause reactions.

More information

Mr. Bracken. Multiple Choice Review: Thermochemistry

Mr. Bracken. Multiple Choice Review: Thermochemistry Mr. Bracken AP Chemistry Name Period Multiple Choice Review: Thermochemistry 1. If this has a negative value for a process, then the process occurs spontaneously. 2. This is a measure of how the disorder

More information

In the box below, draw the Lewis electron-dot structure for the compound formed from magnesium and oxygen. [Include any charges or partial charges.

In the box below, draw the Lewis electron-dot structure for the compound formed from magnesium and oxygen. [Include any charges or partial charges. Name: 1) Which molecule is nonpolar and has a symmetrical shape? A) NH3 B) H2O C) HCl D) CH4 7222-1 - Page 1 2) When ammonium chloride crystals are dissolved in water, the temperature of the water decreases.

More information

Chapter 8 - Chemical Equations and Reactions

Chapter 8 - Chemical Equations and Reactions Chapter 8 - Chemical Equations and Reactions 8-1 Describing Chemical Reactions I. Introduction A. Reactants 1. Original substances entering into a chemical rxn B. Products 1. The resulting substances from

More information

Writing and Balancing Chemical Equations

Writing and Balancing Chemical Equations Name Writing and Balancing Chemical Equations Period When a substance undergoes a chemical reaction, chemical bonds are broken and new bonds are formed. This results in one or more new substances, often

More information

IB Chemistry. DP Chemistry Review

IB Chemistry. DP Chemistry Review DP Chemistry Review Topic 1: Quantitative chemistry 1.1 The mole concept and Avogadro s constant Assessment statement Apply the mole concept to substances. Determine the number of particles and the amount

More information

Standard Free Energies of Formation at 298 K. Average Bond Dissociation Energies at 298 K

Standard Free Energies of Formation at 298 K. Average Bond Dissociation Energies at 298 K 1 Thermodynamics There always seems to be at least one free response question that involves thermodynamics. These types of question also show up in the multiple choice questions. G, S, and H. Know what

More information

Chemical Reactions in Water Ron Robertson

Chemical Reactions in Water Ron Robertson Chemical Reactions in Water Ron Robertson r2 f:\files\courses\1110-20\2010 possible slides for web\waterchemtrans.doc Properties of Compounds in Water Electrolytes and nonelectrolytes Water soluble compounds

More information

Stoichiometry. 1. The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 0.1; (4) 0.2.

Stoichiometry. 1. The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 0.1; (4) 0.2. Stoichiometry 1 The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 01; (4) 02 2 A 44 gram sample of a hydrate was heated until the water of hydration was driven

More information

Balancing Chemical Equations Worksheet

Balancing Chemical Equations Worksheet Balancing Chemical Equations Worksheet Student Instructions 1. Identify the reactants and products and write a word equation. 2. Write the correct chemical formula for each of the reactants and the products.

More information

SCH 4C1 Unit 2 Problem Set Questions taken from Frank Mustoe et all, "Chemistry 11", McGraw-Hill Ryerson, 2001

SCH 4C1 Unit 2 Problem Set Questions taken from Frank Mustoe et all, Chemistry 11, McGraw-Hill Ryerson, 2001 SCH 4C1 Unit 2 Problem Set Questions taken from Frank Mustoe et all, "Chemistry 11", McGraw-Hill Ryerson, 2001 1. A small pin contains 0.0178 mol of iron. How many atoms of iron are in the pin? 2. A sample

More information

stoichiometry = the numerical relationships between chemical amounts in a reaction.

stoichiometry = the numerical relationships between chemical amounts in a reaction. 1 REACTIONS AND YIELD ANSWERS stoichiometry = the numerical relationships between chemical amounts in a reaction. 2C 8 H 18 (l) + 25O 2 16CO 2 (g) + 18H 2 O(g) From the equation, 16 moles of CO 2 (a greenhouse

More information

Moles. Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Equations

Moles. Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Equations Moles Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Equations Micro World atoms & molecules Macro World grams Atomic mass is the mass of an

More information

Chapter 16: Tests for ions and gases

Chapter 16: Tests for ions and gases The position of hydrogen in the reactivity series Hydrogen, although not a metal, is included in the reactivity series because it, like metals, can be displaced from aqueous solution, only this time the

More information

Chemistry B11 Chapter 4 Chemical reactions

Chemistry B11 Chapter 4 Chemical reactions Chemistry B11 Chapter 4 Chemical reactions Chemical reactions are classified into five groups: A + B AB Synthesis reactions (Combination) H + O H O AB A + B Decomposition reactions (Analysis) NaCl Na +Cl

More information

Name Date Class STOICHIOMETRY. SECTION 12.1 THE ARITHMETIC OF EQUATIONS (pages 353 358)

Name Date Class STOICHIOMETRY. SECTION 12.1 THE ARITHMETIC OF EQUATIONS (pages 353 358) Name Date Class 1 STOICHIOMETRY SECTION 1.1 THE ARITHMETIC OF EQUATIONS (pages 353 358) This section explains how to calculate the amount of reactants required or product formed in a nonchemical process.

More information

Chapter 13 Chemical Kinetics

Chapter 13 Chemical Kinetics Chapter 13 Chemical Kinetics Student: 1. The units of "reaction rate" are A. L mol -1 s -1. B. L 2 mol -2 s -1. C. s -1. D. s -2. E. mol L -1 s -1. 2. For the reaction BrO 3 - + 5Br - + 6H + 3Br 2 + 3H

More information

Chapter 6: Writing and Balancing Chemical Equations. AB A + B. CaCO3 CaO + CO2 A + B C. AB + C AC + B (or AB + C CB + A)

Chapter 6: Writing and Balancing Chemical Equations. AB A + B. CaCO3 CaO + CO2 A + B C. AB + C AC + B (or AB + C CB + A) 78 Chapter 6: Writing and Balancing Chemical Equations. It is convenient to classify chemical reactions into one of several general types. Some of the more common, important, reactions are shown below.

More information

Chapter 3: Stoichiometry

Chapter 3: Stoichiometry Chapter 3: Stoichiometry Key Skills: Balance chemical equations Predict the products of simple combination, decomposition, and combustion reactions. Calculate formula weights Convert grams to moles and

More information

Thermochemical equations allow stoichiometric calculations.

Thermochemical equations allow stoichiometric calculations. CHEM 1105 THERMOCHEMISTRY 1. Change in Enthalpy ( H) Heat is evolved or absorbed in all chemical reactions. Exothermic reaction: heat evolved - heat flows from reaction mixture to surroundings; products

More information

Spring 2009. kj mol 125 0-229 -92. H f. H rxn = Σ H f (products) - Σ H f (reactants)

Spring 2009. kj mol 125 0-229 -92. H f. H rxn = Σ H f (products) - Σ H f (reactants) Spring 2009 2. The reaction of an elemental halogen with an alkane is a very common reaction. The reaction between chlorine and butane is provided below. (NOTE: Questions a d and f pertain to this reaction.)

More information

CHEM 105 HOUR EXAM III 28-OCT-99. = -163 kj/mole determine H f 0 for Ni(CO) 4 (g) = -260 kj/mole determine H f 0 for Cr(CO) 6 (g)

CHEM 105 HOUR EXAM III 28-OCT-99. = -163 kj/mole determine H f 0 for Ni(CO) 4 (g) = -260 kj/mole determine H f 0 for Cr(CO) 6 (g) CHEM 15 HOUR EXAM III 28-OCT-99 NAME (please print) 1. a. given: Ni (s) + 4 CO (g) = Ni(CO) 4 (g) H Rxn = -163 k/mole determine H f for Ni(CO) 4 (g) b. given: Cr (s) + 6 CO (g) = Cr(CO) 6 (g) H Rxn = -26

More information

DETERMINING THE ENTHALPY OF FORMATION OF CaCO 3

DETERMINING THE ENTHALPY OF FORMATION OF CaCO 3 DETERMINING THE ENTHALPY OF FORMATION OF CaCO 3 Standard Enthalpy Change Standard Enthalpy Change for a reaction, symbolized as H 0 298, is defined as The enthalpy change when the molar quantities of reactants

More information

Unit 10A Stoichiometry Notes

Unit 10A Stoichiometry Notes Unit 10A Stoichiometry Notes Stoichiometry is a big word for a process that chemist s use to calculate amounts in reactions. It makes use of the coefficient ratio set up by balanced reaction equations

More information

States of Matter CHAPTER 10 REVIEW SECTION 1. Name Date Class. Answer the following questions in the space provided.

States of Matter CHAPTER 10 REVIEW SECTION 1. Name Date Class. Answer the following questions in the space provided. CHAPTER 10 REVIEW States of Matter SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. Identify whether the descriptions below describe an ideal gas or a real gas. ideal gas

More information

Introductory Chemistry, 3 rd Edition Nivaldo Tro. Roy Kennedy Massachusetts Bay Community College Wellesley Hills, Maqqwertd ygoijpk[l

Introductory Chemistry, 3 rd Edition Nivaldo Tro. Roy Kennedy Massachusetts Bay Community College Wellesley Hills, Maqqwertd ygoijpk[l Introductory Chemistry, 3 rd Edition Nivaldo Tro Quantities in Car an octane and oxygen molecules and carbon dioxide and water Chemical Reactions Roy Kennedy Massachusetts Bay Community College Wellesley

More information

1. What is the molecular formula of a compound with the empirical formula PO and a gram-molecular mass of 284 grams?

1. What is the molecular formula of a compound with the empirical formula PO and a gram-molecular mass of 284 grams? Name: Tuesday, May 20, 2008 1. What is the molecular formula of a compound with the empirical formula PO and a gram-molecular mass of 284 grams? 2 5 1. P2O 5 3. P10O4 2. P5O 2 4. P4O10 2. Which substance

More information

Name Class Date. Section: Calculating Quantities in Reactions. Complete each statement below by writing the correct term or phrase.

Name Class Date. Section: Calculating Quantities in Reactions. Complete each statement below by writing the correct term or phrase. Skills Worksheet Concept Review Section: Calculating Quantities in Reactions Complete each statement below by writing the correct term or phrase. 1. All stoichiometric calculations involving equations

More information

4. Using the data from Handout 5, what is the standard enthalpy of formation of BaO (s)? What does this mean?

4. Using the data from Handout 5, what is the standard enthalpy of formation of BaO (s)? What does this mean? HOMEWORK 3A 1. In each of the following pairs, tell which has the higher entropy. (a) One mole of liquid water or one mole of water vapor (b) One mole of dry ice or one mole of carbon dioxide at 1 atm

More information

Chemistry 12 Worksheet 1-1 - Measuring Reaction Rates

Chemistry 12 Worksheet 1-1 - Measuring Reaction Rates Chemistry 12 Worksheet 1-1 - Measuring Reaction Rates 1. A chemist wishes to determine the rate of reaction of zinc with hydrochloric acid. The equation for the reaction is: Zn (s) + 2HCl (aq) oh 2(g)

More information

Stoichiometry. What is the atomic mass for carbon? For zinc?

Stoichiometry. What is the atomic mass for carbon? For zinc? Stoichiometry Atomic Mass (atomic weight) Atoms are so small, it is difficult to discuss how much they weigh in grams We use atomic mass units an atomic mass unit (AMU) is one twelfth the mass of the catbon-12

More information

Molarity of Ions in Solution

Molarity of Ions in Solution APPENDIX A Molarity of Ions in Solution ften it is necessary to calculate not only the concentration (in molarity) of a compound in aqueous solution but also the concentration of each ion in aqueous solution.

More information

Name: Class: Date: 2 4 (aq)

Name: Class: Date: 2 4 (aq) Name: Class: Date: Unit 4 Practice Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1) The balanced molecular equation for complete neutralization of

More information

Chemistry 51 Chapter 8 TYPES OF SOLUTIONS. A solution is a homogeneous mixture of two substances: a solute and a solvent.

Chemistry 51 Chapter 8 TYPES OF SOLUTIONS. A solution is a homogeneous mixture of two substances: a solute and a solvent. TYPES OF SOLUTIONS A solution is a homogeneous mixture of two substances: a solute and a solvent. Solute: substance being dissolved; present in lesser amount. Solvent: substance doing the dissolving; present

More information

Chemical Equations & Stoichiometry

Chemical Equations & Stoichiometry Chemical Equations & Stoichiometry Chapter Goals Balance equations for simple chemical reactions. Perform stoichiometry calculations using balanced chemical equations. Understand the meaning of the term

More information

Chemical Calculations: Formula Masses, Moles, and Chemical Equations

Chemical Calculations: Formula Masses, Moles, and Chemical Equations Chemical Calculations: Formula Masses, Moles, and Chemical Equations Atomic Mass & Formula Mass Recall from Chapter Three that the average mass of an atom of a given element can be found on the periodic

More information

NOTE: This practice exam contains more than questions than the real final.

NOTE: This practice exam contains more than questions than the real final. NOTE: This practice exam contains more than questions than the real final 1 The wavelength of light emitted from a green laser pointer is 532 10 2 nm What is the wavelength in meters? 532 10-7 m 2 What

More information

Topic 4 National Chemistry Summary Notes. Formulae, Equations, Balancing Equations and The Mole

Topic 4 National Chemistry Summary Notes. Formulae, Equations, Balancing Equations and The Mole Topic 4 National Chemistry Summary Notes Formulae, Equations, Balancing Equations and The Mole LI 1 The chemical formula of a covalent molecular compound tells us the number of atoms of each element present

More information

Chemistry Post-Enrolment Worksheet

Chemistry Post-Enrolment Worksheet Name: Chemistry Post-Enrolment Worksheet The purpose of this worksheet is to get you to recap some of the fundamental concepts that you studied at GCSE and introduce some of the concepts that will be part

More information

IB Chemistry 1 Mole. One atom of C-12 has a mass of 12 amu. One mole of C-12 has a mass of 12 g. Grams we can use more easily.

IB Chemistry 1 Mole. One atom of C-12 has a mass of 12 amu. One mole of C-12 has a mass of 12 g. Grams we can use more easily. The Mole Atomic mass units and atoms are not convenient units to work with. The concept of the mole was invented. This was the number of atoms of carbon-12 that were needed to make 12 g of carbon. 1 mole

More information

Problem Solving. Percentage Yield

Problem Solving. Percentage Yield Skills Worksheet Problem Solving Percentage Yield Although we can write perfectly balanced equations to represent perfect reactions, the reactions themselves are often not perfect. A reaction does not

More information

CP Chemistry Review for Stoichiometry Test

CP Chemistry Review for Stoichiometry Test CP Chemistry Review for Stoichiometry Test Stoichiometry Problems (one given reactant): 1. Make sure you have a balanced chemical equation 2. Convert to moles of the known substance. (Use the periodic

More information

Chapter 3. Chemical Reactions and Reaction Stoichiometry. Lecture Presentation. James F. Kirby Quinnipiac University Hamden, CT

Chapter 3. Chemical Reactions and Reaction Stoichiometry. Lecture Presentation. James F. Kirby Quinnipiac University Hamden, CT Lecture Presentation Chapter 3 Chemical Reactions and Reaction James F. Kirby Quinnipiac University Hamden, CT The study of the mass relationships in chemistry Based on the Law of Conservation of Mass

More information

Unit 5 Practice Test. Name: Class: Date: Multiple Choice Identify the choice that best completes the statement or answers the question.

Unit 5 Practice Test. Name: Class: Date: Multiple Choice Identify the choice that best completes the statement or answers the question. Name: Class: Date: Unit 5 Practice Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1) The internal energy of a system is always increased by. A) adding

More information

Summer Holidays Questions

Summer Holidays Questions Summer Holidays Questions Chapter 1 1) Barium hydroxide reacts with hydrochloric acid. The initial concentration of the 1 st solution its 0.1M and the volume is 100ml. The initial concentration of the

More information

UNIT 1 THERMOCHEMISTRY

UNIT 1 THERMOCHEMISTRY UNIT 1 THERMOCHEMISTRY THERMOCHEMISTRY LEARNING OUTCOMES Students will be expected to: THERMOCHEMISTRY STSE analyse why scientific and technological activities take place in a variety individual and group

More information

Chapter 5. Chemical Reactions and Equations. Introduction. Chapter 5 Topics. 5.1 What is a Chemical Reaction

Chapter 5. Chemical Reactions and Equations. Introduction. Chapter 5 Topics. 5.1 What is a Chemical Reaction Introduction Chapter 5 Chemical Reactions and Equations Chemical reactions occur all around us. How do we make sense of these changes? What patterns can we find? 1 2 Copyright The McGraw-Hill Companies,

More information

CHEMICAL REACTIONS AND REACTING MASSES AND VOLUMES

CHEMICAL REACTIONS AND REACTING MASSES AND VOLUMES CHEMICAL REACTIONS AND REACTING MASSES AND VOLUMES The meaning of stoichiometric coefficients: 2 H 2 (g) + O 2 (g) 2 H 2 O(l) number of reacting particles 2 molecules of hydrogen react with 1 molecule

More information

ATOMS. Multiple Choice Questions

ATOMS. Multiple Choice Questions Chapter 3 ATOMS AND MOLECULES Multiple Choice Questions 1. Which of the following correctly represents 360 g of water? (i) 2 moles of H 2 0 (ii) 20 moles of water (iii) 6.022 10 23 molecules of water (iv)

More information

Stoichiometry Review

Stoichiometry Review Stoichiometry Review There are 20 problems in this review set. Answers, including problem set-up, can be found in the second half of this document. 1. N 2 (g) + 3H 2 (g) --------> 2NH 3 (g) a. nitrogen

More information

Chapter 1: Moles and equations. Learning outcomes. you should be able to:

Chapter 1: Moles and equations. Learning outcomes. you should be able to: Chapter 1: Moles and equations 1 Learning outcomes you should be able to: define and use the terms: relative atomic mass, isotopic mass and formula mass based on the 12 C scale perform calculations, including

More information

1. The graph below represents the potential energy changes that occur in a chemical reaction. Which letter represents the activated complex?

1. The graph below represents the potential energy changes that occur in a chemical reaction. Which letter represents the activated complex? 1. The graph below represents the potential energy changes that occur in a chemical reaction. Which letter represents the activated complex? 4. According to the potential energy diagram shown above, the

More information

Question Bank Electrolysis

Question Bank Electrolysis Question Bank Electrolysis 1. (a) What do you understand by the terms (i) electrolytes (ii) non-electrolytes? (b) Arrange electrolytes and non-electrolytes from the following substances (i) sugar solution

More information

1. When the following equation is balanced, the coefficient of Al is. Al (s) + H 2 O (l)? Al(OH) 3 (s) + H 2 (g)

1. When the following equation is balanced, the coefficient of Al is. Al (s) + H 2 O (l)? Al(OH) 3 (s) + H 2 (g) 1. When the following equation is balanced, the coefficient of Al is. Al (s) + H 2 O (l)? Al(OH) (s) + H 2 (g) A) 1 B) 2 C) 4 D) 5 E) Al (s) + H 2 O (l)? Al(OH) (s) + H 2 (g) Al (s) + H 2 O (l)? Al(OH)

More information

Unit 4 Conservation of Mass and Stoichiometry

Unit 4 Conservation of Mass and Stoichiometry 9.1 Naming Ions I. Monatomic Ions A. Monatomic ions 1. Ions formed from a single atom Unit 4 Conservation of Mass and Stoichiometry B. Naming Monatomic Ions 1. Monatomic cations are a. Identified by the

More information

Name period Unit 9: acid/base equilibrium

Name period Unit 9: acid/base equilibrium Name period Unit 9: acid/base equilibrium 1. What is the difference between the Arrhenius and the BronstedLowry definition of an acid? Arrhenious acids give H + in water BronstedLowry acids are proton

More information

W1 WORKSHOP ON STOICHIOMETRY

W1 WORKSHOP ON STOICHIOMETRY INTRODUCTION W1 WORKSHOP ON STOICHIOMETRY These notes and exercises are designed to introduce you to the basic concepts required to understand a chemical formula or equation. Relative atomic masses of

More information

Chemical Equations and Chemical Reactions. Chapter 8.1

Chemical Equations and Chemical Reactions. Chapter 8.1 Chemical Equations and Chemical Reactions Chapter 8.1 Objectives List observations that suggest that a chemical reaction has taken place List the requirements for a correctly written chemical equation.

More information

Chapter 1 The Atomic Nature of Matter

Chapter 1 The Atomic Nature of Matter Chapter 1 The Atomic Nature of Matter 6. Substances that cannot be decomposed into two or more simpler substances by chemical means are called a. pure substances. b. compounds. c. molecules. d. elements.

More information

Chemistry Assessment Unit AS 1

Chemistry Assessment Unit AS 1 Centre Number 71 Candidate Number ADVANCED SUBSIDIARY (AS) General Certificate of Education January 2011 Chemistry Assessment Unit AS 1 assessing Basic Concepts in Physical and Inorganic Chemistry [AC111]

More information

WRITING CHEMICAL FORMULA

WRITING CHEMICAL FORMULA WRITING CHEMICAL FORMULA For ionic compounds, the chemical formula must be worked out. You will no longer have the list of ions in the exam (like at GCSE). Instead you must learn some and work out others.

More information

INTI COLLEGE MALAYSIA A? LEVEL PROGRAMME CHM 111: CHEMISTRY MOCK EXAMINATION: DECEMBER 2000 SESSION. 37 74 20 40 60 80 m/e

INTI COLLEGE MALAYSIA A? LEVEL PROGRAMME CHM 111: CHEMISTRY MOCK EXAMINATION: DECEMBER 2000 SESSION. 37 74 20 40 60 80 m/e CHM111(M)/Page 1 of 5 INTI COLLEGE MALAYSIA A? LEVEL PROGRAMME CHM 111: CHEMISTRY MOCK EXAMINATION: DECEMBER 2000 SESSION SECTION A Answer ALL EIGHT questions. (52 marks) 1. The following is the mass spectrum

More information

HOMEWORK 4A. Definitions. Oxidation-Reduction Reactions. Questions

HOMEWORK 4A. Definitions. Oxidation-Reduction Reactions. Questions HOMEWORK 4A Oxidation-Reduction Reactions 1. Indicate whether a reaction will occur or not in each of following. Wtiring a balcnced equation is not necessary. (a) Magnesium metal is added to hydrochloric

More information

1. Read P. 368-375, P. 382-387 & P. 429-436; P. 375 # 1-11 & P. 389 # 1,7,9,12,15; P. 436 #1, 7, 8, 11

1. Read P. 368-375, P. 382-387 & P. 429-436; P. 375 # 1-11 & P. 389 # 1,7,9,12,15; P. 436 #1, 7, 8, 11 SCH3U- R.H.KING ACADEMY SOLUTION & ACID/BASE WORKSHEET Name: The importance of water - MAKING CONNECTION READING 1. Read P. 368-375, P. 382-387 & P. 429-436; P. 375 # 1-11 & P. 389 # 1,7,9,12,15; P. 436

More information

Chemical Equations. Chemical Equations. Chemical reactions describe processes involving chemical change

Chemical Equations. Chemical Equations. Chemical reactions describe processes involving chemical change Chemical Reactions Chemical Equations Chemical reactions describe processes involving chemical change The chemical change involves rearranging matter Converting one or more pure substances into new pure

More information

1. Thermite reaction 2. Enthalpy of reaction, H 3. Heating/cooling curves and changes in state 4. More thermite thermodynamics

1. Thermite reaction 2. Enthalpy of reaction, H 3. Heating/cooling curves and changes in state 4. More thermite thermodynamics Chem 105 Fri 10-23-09 1. Thermite reaction 2. Enthalpy of reaction, H 3. Heating/cooling curves and changes in state 4. More thermite thermodynamics 10/23/2009 1 Please PICK UP your graded EXAM in front.

More information

4.5 Physical Properties: Solubility

4.5 Physical Properties: Solubility 4.5 Physical Properties: Solubility When a solid, liquid or gaseous solute is placed in a solvent and it seems to disappear, mix or become part of the solvent, we say that it dissolved. The solute is said

More information

Unit 19 Practice. Name: Class: Date: Multiple Choice Identify the choice that best completes the statement or answers the question.

Unit 19 Practice. Name: Class: Date: Multiple Choice Identify the choice that best completes the statement or answers the question. Name: Class: Date: Unit 19 Practice Multiple Choice Identify the choice that best completes the statement or answers the question. 1) The first law of thermodynamics can be given as. A) E = q + w B) =

More information

Solution a homogeneous mixture = A solvent + solute(s) Aqueous solution water is the solvent

Solution a homogeneous mixture = A solvent + solute(s) Aqueous solution water is the solvent Solution a homogeneous mixture = A solvent + solute(s) Aqueous solution water is the solvent Water a polar solvent: dissolves most ionic compounds as well as many molecular compounds Aqueous solution:

More information

H 2 + O 2 H 2 O. - Note there is not enough hydrogen to react with oxygen - It is necessary to balance equation.

H 2 + O 2 H 2 O. - Note there is not enough hydrogen to react with oxygen - It is necessary to balance equation. CEMICAL REACTIONS 1 ydrogen + Oxygen Water 2 + O 2 2 O reactants product(s) reactant substance before chemical change product substance after chemical change Conservation of Mass During a chemical reaction,

More information

Unit 6 The Mole Concept

Unit 6 The Mole Concept Chemistry Form 3 Page 62 Ms. R. Buttigieg Unit 6 The Mole Concept See Chemistry for You Chapter 28 pg. 352-363 See GCSE Chemistry Chapter 5 pg. 70-79 6.1 Relative atomic mass. The relative atomic mass

More information

Moles. Moles. Moles. Moles. Balancing Eqns. Balancing. Balancing Eqns. Symbols Yields or Produces. Like a recipe:

Moles. Moles. Moles. Moles. Balancing Eqns. Balancing. Balancing Eqns. Symbols Yields or Produces. Like a recipe: Like a recipe: Balancing Eqns Reactants Products 2H 2 (g) + O 2 (g) 2H 2 O(l) coefficients subscripts Balancing Eqns Balancing Symbols (s) (l) (aq) (g) or Yields or Produces solid liquid (pure liquid)

More information

Stoichiometry. 1. The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 0.1; (4) 0.2.

Stoichiometry. 1. The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 0.1; (4) 0.2. Stoichiometry 1 The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 01; (4) 02 2 A 44 gram sample of a hydrate was heated until the water of hydration was driven

More information

Chapter 17. How are acids different from bases? Acid Physical properties. Base. Explaining the difference in properties of acids and bases

Chapter 17. How are acids different from bases? Acid Physical properties. Base. Explaining the difference in properties of acids and bases Chapter 17 Acids and Bases How are acids different from bases? Acid Physical properties Base Physical properties Tastes sour Tastes bitter Feels slippery or slimy Chemical properties Chemical properties

More information

Transfer of heat energy often occurs during chemical reactions. A reaction

Transfer of heat energy often occurs during chemical reactions. A reaction Chemistry 111 Lab: Thermochemistry Page I-3 THERMOCHEMISTRY Heats of Reaction The Enthalpy of Formation of Magnesium Oxide Transfer of heat energy often occurs during chemical reactions. A reaction may

More information

Calculation of Molar Masses. Molar Mass. Solutions. Solutions

Calculation of Molar Masses. Molar Mass. Solutions. Solutions Molar Mass Molar mass = Mass in grams of one mole of any element, numerically equal to its atomic weight Molar mass of molecules can be determined from the chemical formula and molar masses of elements

More information

Chapter 8 Concepts of Chemical Bonding

Chapter 8 Concepts of Chemical Bonding Chapter 8 Concepts of Chemical Bonding Chemical Bonds Three types: Ionic Electrostatic attraction between ions Covalent Sharing of electrons Metallic Metal atoms bonded to several other atoms Ionic Bonding

More information

Chemistry Diagnostic Questions

Chemistry Diagnostic Questions Chemistry Diagnostic Questions Answer these 40 multiple choice questions and then check your answers, located at the end of this document. If you correctly answered less than 25 questions, you need to

More information

SUPPLEMENTARY TOPIC 3 ENERGY AND CHEMICAL REACTIONS

SUPPLEMENTARY TOPIC 3 ENERGY AND CHEMICAL REACTIONS SUPPLEMENTARY TOPIC 3 ENERGY AND CHEMICAL REACTIONS Rearranging atoms. In a chemical reaction, bonds between atoms in one or more molecules (reactants) break and new bonds are formed with other atoms to

More information

ENTHALPY CHANGES FOR A CHEMICAL REACTION scaling a rxn up or down (proportionality) quantity 1 from rxn heat 1 from Δ r H. = 32.

ENTHALPY CHANGES FOR A CHEMICAL REACTION scaling a rxn up or down (proportionality) quantity 1 from rxn heat 1 from Δ r H. = 32. CHEMISTRY 103 Help Sheet #10 Chapter 4 (Part II); Sections 4.6-4.10 Do the topics appropriate for your lecture Prepared by Dr. Tony Jacob http://www.chem.wisc.edu/areas/clc (Resource page) Nuggets: Enthalpy

More information

Chapter 6 Notes Science 10 Name:

Chapter 6 Notes Science 10 Name: 6.1 Types of Chemical Reactions a) Synthesis (A + B AB) Synthesis reactions are also known as reactions. When this occurs two or more reactants (usually elements) join to form a. A + B AB, where A and

More information

CHM1 Review for Exam 12

CHM1 Review for Exam 12 Topics Solutions 1. Arrhenius Acids and bases a. An acid increases the H + concentration in b. A base increases the OH - concentration in 2. Strong acids and bases completely dissociate 3. Weak acids and

More information

CHEMICAL REACTIONS. Chemistry 51 Chapter 6

CHEMICAL REACTIONS. Chemistry 51 Chapter 6 CHEMICAL REACTIONS A chemical reaction is a rearrangement of atoms in which some of the original bonds are broken and new bonds are formed to give different chemical structures. In a chemical reaction,

More information

General Chemistry II Chapter 20

General Chemistry II Chapter 20 1 General Chemistry II Chapter 0 Ionic Equilibria: Principle There are many compounds that appear to be insoluble in aqueous solution (nonelectrolytes). That is, when we add a certain compound to water

More information

2. DECOMPOSITION REACTION ( A couple have a heated argument and break up )

2. DECOMPOSITION REACTION ( A couple have a heated argument and break up ) TYPES OF CHEMICAL REACTIONS Most reactions can be classified into one of five categories by examining the types of reactants and products involved in the reaction. Knowing the types of reactions can help

More information

Chapter 7: Chemical Reactions

Chapter 7: Chemical Reactions Chapter 7 Page 1 Chapter 7: Chemical Reactions A chemical reaction: a process in which at least one new substance is formed as the result of a chemical change. A + B C + D Reactants Products Evidence that

More information

Chemistry 151 Final Exam

Chemistry 151 Final Exam Chemistry 151 Final Exam Name: SSN: Exam Rules & Guidelines Show your work. No credit will be given for an answer unless your work is shown. Indicate your answer with a box or a circle. All paperwork must

More information

Aqueous Solutions. Water is the dissolving medium, or solvent. Some Properties of Water. A Solute. Types of Chemical Reactions.

Aqueous Solutions. Water is the dissolving medium, or solvent. Some Properties of Water. A Solute. Types of Chemical Reactions. Aqueous Solutions and Solution Stoichiometry Water is the dissolving medium, or solvent. Some Properties of Water Water is bent or V-shaped. The O-H bonds are covalent. Water is a polar molecule. Hydration

More information

Other Stoich Calculations A. mole mass (mass mole) calculations. GIVEN mol A x CE mol B. PT g A CE mol A MOLE MASS :

Other Stoich Calculations A. mole mass (mass mole) calculations. GIVEN mol A x CE mol B. PT g A CE mol A MOLE MASS : Chem. I Notes Ch. 12, part 2 Using Moles NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. 1 MOLE = 6.02 x 10 23 representative particles (representative particles

More information

neutrons are present?

neutrons are present? AP Chem Summer Assignment Worksheet #1 Atomic Structure 1. a) For the ion 39 K +, state how many electrons, how many protons, and how many 19 neutrons are present? b) Which of these particles has the smallest

More information

Writing, Balancing and Predicting Products of Chemical Reactions.

Writing, Balancing and Predicting Products of Chemical Reactions. Writing, Balancing and Predicting Products of Chemical Reactions. A chemical equation is a concise shorthand expression which represents the relative amount of reactants and products involved in a chemical

More information

Chem 1A Exam 2 Review Problems

Chem 1A Exam 2 Review Problems Chem 1A Exam 2 Review Problems 1. At 0.967 atm, the height of mercury in a barometer is 0.735 m. If the mercury were replaced with water, what height of water (in meters) would be supported at this pressure?

More information