# (a) graph Y versus X (b) graph Y versus 1/X

Save this PDF as:

Size: px
Start display at page:

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

## Transcription

1 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 is determined with a monometer that is filled with silicone oil (density = 1.30 g/ml). Assume an atmospheric pressure of 756 mm Hg, and determine the pressure of each gas in (1) mm Hg, (2) torr, (3) atmospheres and (4) pascals. (a) (b) (c) (d) 2. Given the following data: X Y (a) graph Y versus X (b) graph Y versus 1/X (c) graph log Y versus log X (d) graph XY versus X

2 HOMEWORK 5B Charles s Law; Absolute Zero; Avogadro s Law; Standard Temperature and Pressure (STP) 1. Calculate the moles of gas contained in a 986 ml flask at 29.2ºC with a pressure of 688 torr. 2. Calculate the density of ammonia gas at 27 C and 635 torr. 3. A compound is found to be 24.8% carbon, 2.1% hydrogen, and 73.1% chlorine by mass. When the compound was vaporized, a 256 ml flask at 373 K and 751 torr contained g of the gaseous compound. For the compound, determine its (a) empirical formula (b) molar mass (c) molecular formula 4. Draw a qualitative graph to show how the first property varies with the second in each of the following. In each case, assume the moles of gas are constant. (a) p versus T with constant V (c) p versus 1/V with constant T (e) pv versus V with constant T (b) p versus V with constant T (d) log p versus log V with constant T HOMEWORK 5C Dalton s Law of Partial Pressures; Partial Pressure; Mole Fraction 1. Calculate the volume of oxygen gas that can be produced at 30. C and 725 torr from the complete decomposition of 4.10 g mercury (II) oxide. 2. Urea, H 2 NCONH 2, is used as a nitrogen source in fertilizers, and can be produced commercially from the reaction of ammonia with carbon dioxide: 2NH 3 (g) + CO 2 (g) H 2 NCONH 2 (s) + H 2 O (g) Calculate the mass of urea that can be produced if 500. L of ammonia at 223 C and 90. atm are reacted with 600. L of carbon dioxide at 223 C and 45 atm. 3. When a flask is charged with g of ammonia gas and g of nitrogen gas, the pressure was measured to be 4.43 atm. (a) Draw Lewis structures and bond-orbital models for molecules for each gas. (b) Find the partial pressures of each gas.

3 HOMEWORK 5D Kinetic Molecular Theory; Joule; Diffusion; Effusion 1. Determine the pressure of dry hydrogen gas collected in each of the following eudiometers. Assume an atmospheric pressure of torr and a temperature of 22.0 C. Water vapor pressure at 22.0 C is 19.8 torr. 2. Acetylene gas, C 2 H 2, and calcium hydroxide are produced when solid calcium carbide, CaC 2, reacts with water. From a sample containing calcium carbide, 2.18 L of acetylene are collected over water in a eudiometer. The water level inside the eudiometer is 87.5 mm higher than the outside, the water temperature is 21.5 C, the atmospheric pressure is torr, and the water vapor pressure at 21.5 C is 19.2 torr. (a) Calculate the mass of the calcium carbide that reacted. (b) If the sample was known to be 90.0% calcium carbide by mass, calculate the mass of the sample that reacted. 3. Calculate the root-mean-square-velocity of nitrogen molecules (a) at 273 K (b) at 546 K 4. Graph the relative number of nitrogen molecules versus their velocities (a) at 273 K (b) at 546 K

4 HOMEWORK 5E Air Pollution; Acid Rain; Homogeneous Catalyst; Freon; Greenhouse Effect 1. A 3.50 g sample of a compound containing only carbon, hydrogen, and nitrogen was burned, producing 3.35 g of carbon dioxide and 4.11 g of water. The effusion rate of the compound was measured and found to be 24.6 ml/min. Under the same conditions, the effusion rate of argon gas was found to be 26.4 ml/min. (a) Determine the empirical formula of the compound (b) Determine the molar mass of the compound (c) Determine the molecular formula of the compound 2. Table 5.3 in the text book does not give the van der Waals constants a and b for gaseous Br 2. Predict their numerical values and explain your reasoning. 3. Calculate the pressure of moles of nitrogen gas in a L container at 25.0 C using: (a) the ideal gas law equation 4. Have access to Handout 7 from the Class Web Site (b) the van der Waals equation HOMEWORK 5F Exothermic; Endothermic; Bond Energy; Enthalpy; Calorimeter; Heat Capacity; Specific Heat Capacity; Molar Heat Capacity 1. Using the bond energies from Table 8.4 in the text book, estimate the energy change for the reaction: CH 4 (g) + 2O 2 (g) CO 2 (g) + 2H 2 O (g) 2. In a coffee-cup calorimeter, 50.0 ml of 1.00 M sulfuric acid is mixed with ml of 1.00 M sodium hydroxide, both at 24.6 C. After the reaction, the solution reaches a maximum temperature of 31.2 C, and the solution s mass is measured to be g. If the specific heat capacity of the solution is J/gC, calculate the heat of the reaction, in kj per mole of sodium sulfate.

5 HOMEWORK 5G 1. A g sample of magnesium metal is added to 20 ml of a 1.0 M hydrochloric acid solution in a calorimeter, and the temperature of the solution increases from 21.4ºC to 48.9ºC. If the mass of the solution is g and the specific heat capacity of the solution is J/gC, calculate the heat of the reaction, in kj per mole of magnesium. 2. Using your answer from question 1, calculate the amount of heat relaeased or absorbed when the given amounts of magnesium metal react with excess hydrochloric acid. (a) moles of Mg (b) 4.75 grams of Mg 3. The reaction between hydrochloric acid and barium hydroxide has a heat of neutralization of 118 kj per mole of barium chloride. In a coffee-cup calorimeter, ml of M hydrochloric acid is mixed with ml of M barium hydroxide, both at 25.0 C. After the reaction, the final mixture has a mass of g and has a specific heat capacity of J/gC. Calculate the final temperature of the mixture. 4. A g sample of quinone (C 6 H 4 O 2 ) is burned in a bomb calorimeter that has a heat capacity of 1.56 kj/c, and the temperature of the calorimeter rises from 21.0 C to 24.2 C. Calculate the heat of combustion of quinone in kj per gram of quinone. 5. Using your answer from question 4, calculate the amount of heat relaeased or absorbed when the given amounts of quinone are burned. (a) 3.65 grams of quinone (b) 75.0 ml of quinone (density = g/ml) 6. A bomb calorimeter with a heat capacity of 10.8 kj/c has an initial temperature of C. A g sample of benzoic acid is combusted in the calorimeter. If the benzoic acid has a heat of combustion of kj/g benzoic acid, calculate the final temperature of the bomb calorimeter.

6 HOMEWORK 5H Hess s Law; Lattice Energy; Standard Enthalpy of Formation 1. Given the heat of combustions for the following reactions: C 2 H 2 (g) + 5 /2O 2 (g) 2CO 2 (g) + H 2 O(g) H = 1257 kj C(s) + O 2 (g) CO 2 (g) H = 394 kj H 2 (g) + ½O 2 (g) H 2 O(g) H = 242 kj calculate the H for the reaction: 2C(s) + H 2 (g) C 2 H 2 (g) 2. Using the heat of combustions for C 4 H 4 ( 2341 kj/mol), C 4 H 8 ( 2755 kj/mol), and H 2 ( 242 kj/mol), calculate the H for the reaction: C 4 H 4 + 2H 2 C 4 H 8 3. Have access to Handout 8 from the Class Web Site. HOMEWORK 5I State Function; Petroleum; Natural Gas; Coal 1. Using the standard heat of formations in Appendix 4 (pages A21-A23) of your text book., calculate H for the combustion of octane, in kj/gram of octane, and H for the combustion of ethanol, in kj/gram of ethanol. Determine which fuel provides the most energy per gram. (The standard heat of formation for octane is found only in Table 6.2) (a) 2C 8 H 18 (l) + 25O 2 (g) 16CO 2 (g) + 18H 2 O(g) (b) C 2 H 5 OH(l) + 3O 2 (g) 2CO 2 (g) + 3H 2 O(g) 2. The standard heat of combustion of butane gas, C 4 H 10, is kj/gram of butane. Using the standard heat of formations in Appendix 4 (pages A21-A23) of your text book, calculate the standard heat of formation of butane gas.

7 HOMEWORK 5J Internal Energy; Heat; Work; First Law of Thermodynamics 1. Calculate the change in internal energy for each of the following: (a) a gas absorbs 45 kj of heat and expands, doing 29 kj of work on the surroundings. (b) a gas releases 125 kj of heat and is compressed, having 104 kj of work done on it. 2. A gas expands from 62 ml to 287 ml against a constant pressure of atm. Calculate the work done by the gas in each of the following units: (a) Latm (b) J 3. A balloon containing 313 g helium has a volume of L at 28 C. The temperature of the helium decreases to 13 C and the volume of the balloon shrinks to 1814 L against a constant pressure of 1.00 atm. The molar heat capacity of helium is 20.8 J/molC. For the helium, calculate (a) q (b) w (c) E (d) H HOMEWORK 4R 1. Give the missing information for each gas: p V n T (a) 5.00 atm 2.00 mol 155 C (b) 228 torr 2.00 L 155 K (c) atm 775 ml mol (d) 2.25 L 10.5 mol 75 C 2. Calculate the density of gaseous trichlorsilane (SiHCl 3 ) at 85 C and 758 torr. 3. Calculate the molar mass of a gaseous substance if a L sample of the gas at 99.5 C and torr has a mass of g. 4. If the gas in question 3 was found to be 36.4% carbon, 6.1% hydrogen, and 57.5% fluorine by mass, determine its empirical and molecular formulas. 5. When g of methane gas, 1.02 g of nitrogen gas, and 1.35 g of argon gas are placed in a flask, they produce a pressure of 587 torr. Find the partial pressures of each gas. (continued on next page)

8 6. Give the pressure of dry oxygen gas is each of the following gas collecting devices. Assume atmospheric pressure is 758 torr and the temperature is 21 C. Water vapor pressure at 21 C is 19 torr. 7. A 370. ml sample of oxygen gas is produced in the laboratory from the decomposition of potassium chlorate. The oxygen is collected by water displacement in an Erlenmeyer flask, the level of water inside the flask the same as the level of water outside the flask. The water temperature is 27.0 C and atmospheric pressure is torr. Water vapor pressure at 27.0 C is 26.7 torr. Calculate the mass of potassium chlorate that was decomposed. 8. Calculate the root-mean-square velocity of methane molecules at 273 K. 9. Consider three identical flasks filled with different gases: Flask A: CO at 760 torr and 0 C Flask B: N 2 at 250 torr and 0 C Flask C: H 2 at 100 torr and 0 C (a) In which flask will the molecules have the greatest average kinetic energy? (b) In which flask will the molecules have the greatest average velocity? 10. The diffusion rate of an unknown gas is measured and found to be ml/min. Under identical conditions, the diffusion rate of oxygen gas is found to be ml/min. Identify the unknown gas if it is known to be either ammonia, carbon monoxide, nitrogen monoxide, carbon dioxide, or nitrogen dioxide. 11. For the following gases: CO 2 HF He (a) arrange them from smallest to largest according to the van der Waal s constant a. (b) arrange them from smallest to largest according to the van der Waal s constant b. (continued on next page)

9 12. The heat change of a substance can be given by the following relationship: q = Cm T Graph each of the following relationships: (a) q vs. T (at constant m) (b) m vs. T (at constant q) (c) m vs. 1/ T (at constant q) (d) m T vs. m (at constant q) (e) log m vs. log T (at constant q) 13. A balloon filled with 156 grams of helium gas has a volume of 876 L at STP. While the pressure remains constant, the temperature of the balloon is increased to 38.0 C, and it expands to a volume of 998 L. Calculate q, w, E and H for the helium in the balloon. The heat capacity for helium gas is 5.20 J/gC. 14. For the incomplete combustion of silicon: 2Si(s) + O 2 (g) 2SiO(g) H = kj calculate the amount of heat released for each of the following: (a) 5.00 mol of Si is reacted (b) 5.00 g of Si is reacted 15. In coffee-cup calorimeter 20.0 ml of M silver nitrate, initially at C, are mixed with 30.0 ml of M hydrochloric acid, also at C. After the solutions mix, and a precipitate is formed, the temperature of the mixture reaches a maximum of C. The mass of the solution was g. Assuming the heat capacity of the solution is J/gC, find the heat of the reaction, in kilojoules per mole of silver chloride. 16. The reaction between sulfuric acid and sodium hydroxide has a heat of neutralization of 112 kj per mole of sodium sulfate. In a coffee-cup calorimeter, ml of M sulfuric acid is mixed with ml of M sodium hydroxide, both at C. After the reaction, the final mixture has a mass of g and has a specific heat capacity of J/gC. Calculate the final temperature of the mixture. 17. A g sample of wax is burned in a bomb calorimeter that has a heat capacity of 1.75 kj/c, and the temperature of the calorimeter rises from C to C. Calculate the heat of combustion of wax in kj per gram of wax. 18. Camphor (C 10 H 16 O) has a heat of combustion of 5904 kj/mol. When a sample of camphor with a mass of g is burned in a bomb calorimeter, the temperature increases from C to C. Calculate the heat capacity of the calorimeter. 19. Given the following data: H 2 (g) + ½O 2 (g) H 2 O(l) N 2 O 5 (g) + H 2 O(l) 2HNO 3 (l) ½N 2 (g) + 1½O 2 (g) + ½H 2 (g) HNO 3 (l) calculate the H for the reaction: 2N 2 (g) + 5O 2 (g) 2N 2 O 5 (g) H = kj H = 76.6 kj H = kj (continued on next page)

10 20. The heat of combustion of solid carbon to carbon dioxide is kj/mol, and the heat of combustion of carbon monoxide to form carbon dioxide is kj/mol. Use these data to calculate the H for the reaction 2C(s) + O 2 (g) 2CO(g) 21. Given the following data: Lattice Energy of NaCl First Ionization Energy of Na Second Ionization Energy of Na Electron Affinity of Cl Bond Energy of Cl 2 Sublimation Energy of Na estimate the standard heat of formation for solid sodium chloride. 786 kj/mol 495 kj/mol 4560 kj/mol 349 kj/mol 239 kj/mol 109 kj/mol 22. Calculate H for each of the following reactions using the standard heat of formations in Appendix 4 (pages A21-A23) of your text book: (a) 2NO(g) + O 2 (g) 2NO 2 (g) (b) 2NH 3 (g) + 3O 2 (g) + 2CH 4 (g) 2HCN(g) + 6H 2 O(g) 23. The reusable booster rockets of the space shuttle use a mixture of aluminum and ammonium perchlorate as fuel. A possible reaction is: 3Al(s) + 3NH 4 ClO 4 (s) Al 2 O 3 (s) + AlCl 3 (s) + 3NO(g) + 6H 2 O(g) Calculate H, in kj/gram Al, for this reaction using the standard heat of formations in Appendix 4 (pages A21-A25) of your text book: 24. Consider the reaction: 2ClF 3 (g) + 2NH 3 (g) N 2 (g) + 6HF(g) + Cl 2 (g) H = kj Using the standard heat of formations in Appendix 4 (pages A21-A23) of your text book, calculate the standard heat of formation of gaseous chlorine trifluoride. 25. Using the bond energies from Table 8.4 in the text book, estimate the heat of reaction for each of the following: (a) H 2 + Cl 2 2HCl (b) N 2 + 3H 2 2NH 3 HOMEWORK 4R ANSWERS 1. (a) 14.1 L (b) mol (c) 141 K (d) 133 atm g/l g/mol 4. CH 2 F, C 2 H 4 F torr CH 4, 196 torr N 2, 182 torr Ar (continued on next page)

11 6. (a) 354 mm Hg (b) 1112 mm Hg (c) 739 mm Hg (d) 728 mm Hg g KClO m/s 9. (a) all are equal (b) flask C 10. nitrogen monoxide 11. (a) He, CO 2, HF (b) He, HF, CO (a) (b) (c) (d) (e) 13. q = 30,800 J, w = -12,400 J, E = 18,400 J, H = 30,800 J 14. (a) -221 kj (b) kj kj/mol AgCl C kj/g wax kj/c kj kj kj 22. (a) -112 kj (b) kj kj/g kj/mol 25. (a) -183 kj (b) -109 kj

### Chapter 5. Name: Class: Date: Multiple Choice Identify the choice that best completes the statement or answers the question.

Class: Date: Chapter 5 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. What is the pressure of the sample of gas trapped in the open-tube mercury manometer

### Figure 10.3 A mercury manometer. This device is sometimes employed in the laboratory to measure gas pressures near atmospheric pressure.

Characteristics of Gases Practice Problems A. Section 10.2 Pressure Pressure Conversions: 1 ATM = 101.3 kpa = 760 mm Hg (torr) SAMPLE EXERCISE 10.1 Converting Units of Pressure (a) Convert 0.357 atm to

### MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

Chapter 10 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) A gas at a pressure of 10.0 Pa exerts a force of N on an area of 5.5 m2. A) 1.8 B) 0.55

### CHAPTER 12 GASES AND THEIR BEHAVIOR

Chapter 12 Gases and Their Behavior Page 1 CHAPTER 12 GASES AND THEIR BEHAVIOR 12-1. Which of the following represents the largest gas pressure? (a) 1.0 atm (b) 1.0 mm Hg (c) 1.0 Pa (d) 1.0 KPa 12-2. Nitrogen

### 4. Aluminum chloride is 20.2% aluminum by mass. Calculate the mass of aluminum in a 35.0 gram sample of aluminum chloride.

1. Calculate the molecular mass of table sugar sucrose (C 12 H 22 O 11 ). A. 342.30 amu C. 320.05 amu B. 160.03 amu D. 171.15 amu 2. How many oxygen atoms are in 34.5 g of NaNO 3? A. 2.34 10 23 atoms C.

### 3. Of energy, work, enthalpy, and heat, how many are state functions? a) 0 b) 1 c) 2 d) 3 e) 4 ANS: c) 2 PAGE: 6.1, 6.2

1. A gas absorbs 0.0 J of heat and then performs 15.2 J of work. The change in internal energy of the gas is a) 24.8 J b) 14.8 J c) 55.2 J d) 15.2 J ANS: d) 15.2 J PAGE: 6.1 2. Calculate the work for the

### Force. Pressure = ; Area. Force = Mass times Acceleration;

Force Pressure = ; Area Force = Mass times Acceleration; If mass = kg, and acceleration = m/s 2, Force = kg.m/s 2 = Newton (N) If Area = m 2, Pressure = (kg.m/s 2 )/m 2 = N/m 2 = Pascal; (1 Pa = 1 N/m

### 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

### CHM1045 Practice Test 3 v.1 - Answers Name Fall 2013 & 2011 (Ch. 5, 6, 7, & part 11) Revised April 10, 2014

CHM1045 Practice Test 3 v.1 - Answers Name Fall 013 & 011 (Ch. 5, 6, 7, & part 11) Revised April 10, 014 Given: Speed of light in a vacuum = 3.00 x 10 8 m/s Planck s constant = 6.66 x 10 34 J s E (-.18x10

### 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.

### Tutorial 6 GASES. PRESSURE: atmospheres or mm Hg; 1 atm = 760 mm Hg. STP: Standard Temperature and Pressure: 273 K and 1 atm (or 760 mm Hg)

T-41 Tutorial 6 GASES Before working with gases some definitions are needed: PRESSURE: atmospheres or mm Hg; 1 atm = 760 mm Hg TEMPERATURE: Kelvin, K, which is o C + 273 STP: Standard Temperature and Pressure:

### CHEM 1411, chapter 5 exercises

CHEM 1411, chapter 5 exercises 1. A gas-filled balloon with a volume of 12.5 L at 0.90 atm and 21 C is allowed to rise to the stratosphere where the temperature is 5 C and the pressure is 1.0 millibar.

### Sample Exercise 10.1 Converting Pressure Units

Sample Exercise 10.1 Converting Pressure Units (a) Convert 0.357 atm to torr. (b) Convert 6.6 10 2 torr to atmospheres. (c) Convert 147.2 kpa to torr. Solution Analyze In each case we are given the pressure

### 21 st Century Chemistry Multiple Choice Question in Topic 3 Metals Unit 11

21 st Century Chemistry Multiple Choice Question in Topic 3 Metals Unit 11 1. Consider the equation: 2Ca(s) + O 2 (g) 2CaO(s) Which of the following statements are correct? (1) Calcium and oxygen are reactants.

### Chapter 5 Gases. August 2, 2009 [PROBLEM SET FROM R. CHANG TEST BANK] Student:

Chapter 5 Gases Student: 1. A pressure that will support a column of Hg to a height of 256 mm would support a column of water to what height? The density of mercury is 13.6 g/cm 3 ; the density of water

### Exam 4 Practice Problems false false

Exam 4 Practice Problems 1 1. Which of the following statements is false? a. Condensed states have much higher densities than gases. b. Molecules are very far apart in gases and closer together in liquids

### The Gas Laws. Our Atmosphere. Pressure = Units of Pressure. Barometer. Chapter 10

Our Atmosphere The Gas Laws 99% N 2 and O 2 78% N 2 80 70 Nitrogen Chapter 10 21% O 2 1% CO 2 and the Noble Gases 60 50 40 Oxygen 30 20 10 0 Gas Carbon dioxide and Noble Gases Pressure Pressure = Force

### 0.786 mol carbon dioxide to grams g lithium carbonate to mol

1 2 Convert: 2.54 x 10 22 atoms of Cr to mol 4.32 mol NaCl to grams 0.786 mol carbon dioxide to grams 2.67 g lithium carbonate to mol 1.000 atom of C 12 to grams 3 Convert: 2.54 x 10 22 atoms of Cr to

### 1. Balance the following equation. What is the sum of the coefficients of the reactants and products?

1. Balance the following equation. What is the sum of the coefficients of the reactants and products? 1 Fe 2 O 3 (s) + _3 C(s) 2 Fe(s) + _3 CO(g) a) 5 b) 6 c) 7 d) 8 e) 9 2. Which of the following equations

### 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

### Enthalpy of Reaction and Calorimetry worksheet

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

### Chapter 3. Stoichiometry: Ratios of Combination. Insert picture from First page of chapter. Copyright McGraw-Hill 2009 1

Chapter 3 Insert picture from First page of chapter Stoichiometry: Ratios of Combination Copyright McGraw-Hill 2009 1 3.1 Molecular and Formula Masses Molecular mass - (molecular weight) The mass in amu

### SCH3UI-02 Final Examination Review (Fall 2014)

SCH3UI-02 Final Examination Review (Fall 2014) 1. Chlorine has an atomic number of 17. Create a Bohr Rutherford diagram of a Cl-35 atom. To achieve a stable arrangement, is this atom most likely to gain

### 6.1 Some basic principles

Ch 6 Thermochemistry: Energy Flow and Chemical Change 6.1 Forms of Energy and Their Interconversion 6.2 Enthalpy: Heats of Reaction and Chemical Change 6.3 Calorimetry: Laboratory Measurement of Heats

### ESSAY. Write your answer in the space provided or on a separate sheet of paper.

Test 1 General Chemistry CH116 Summer, 2012 University of Massachusetts, Boston Name ESSAY. Write your answer in the space provided or on a separate sheet of paper. 1) Sodium hydride reacts with excess

### 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

### Exploring Gas Laws. Chapter 12. Solutions for Practice Problems. Student Textbook page 477

Chapter 12 Exploring Gas Laws Solutions for Practice Problems Student Textbook page 477 1. Problem At 19 C and 100 kpa, 0.021 mol of oxygen gas, O 2(g), occupy a volume of 0.50 L. What is the molar volume

### 4. Magnesium has three natural isotopes with the following masses and natural abundances:

Exercise #1 Atomic Masses 1. The average mass of pennies minted after 1982 is 2.50 g and the average mass of pennies minted before 1982 is 3.00 g. In a sample that contains 90.0% new and 10.0% old pennies,

### 7. 1.00 atm = 760 torr = 760 mm Hg = 101.325 kpa = 14.70 psi. = 0.446 atm. = 0.993 atm. = 107 kpa 760 torr 1 atm 760 mm Hg = 790.

CHATER 3. The atmosphere is a homogeneous mixture (a solution) of gases.. Solids and liquids have essentially fixed volumes and are not able to be compressed easily. have volumes that depend on their conditions,

### Chapter 3 Mass Relationships in Chemical Reactions

Chapter 3 Mass Relationships in Chemical Reactions Student: 1. An atom of bromine has a mass about four times greater than that of an atom of neon. Which choice makes the correct comparison of the relative

### CHAPTER 6 THERMOCHEMISTRY

Chapter 6 Thermochemistry Page 1 CHAPTER 6 THERMOCHEMISTRY 6-1. The standard state of an element or compound is determined at a pressure of and a temperature of. (a) 760 atm, 0 o C (b) 1 mmhg, 273 o C

### Chapter 4 The Properties of Gases

Chapter 4 The Properties of Gases Significant Figure Convention At least one extra significant figure is displayed in all intermediate calculations. The final answer is expressed with the correct number

### CHE141 Chapter 10. Chapter 10 Gases

Chapter 0 Gases. A sample of gas (4.g) initially at 4.00 atm was compressed from 8.00 L to.00 L at constant temperature. After the compression, the gas pressure was atm. (a). 4.00 (b)..00 (c)..00 (d).

### 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?

### Chemistry Guide

551534 - Chemistry Guide 1- Contents Question Item Objective Type Skill 1 0102 M03.02.04 Multiple-choice answer Mastery of Problem Solving 2 0099 M03.03.02 Multiple-choice answer Mastery of Concepts 3

### 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

### Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten. Chapter 10 Gases

Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 10 Gases A Gas Has neither a definite volume nor shape. Uniformly fills any container.

### 1.23 Gas Calculations

1.23 Gas Calculations Gas calculations at A-level are done in two different ways although both link the volumes of a gas to the amount in moles of the gas. The same amount in moles of any gas will have

### 1011_2nd Exam_

1011_2nd Exam_1011114 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Identify the reducing agent in the following reaction: 2 NO2(g) + 7 H2(g)

### STOICHIOMETRY STOICHIOMETRY. Measurements in Chemical Reactions. Mole-Mole Relationships. Mass-Mass Problem. Mole-Mole Relationships

STOICHIOMETRY STOICHIOMETRY The analysis of the quantities of substances in a chemical reaction. Stoichiometric calculations depend on the MOLE- MOLE relationships of substances. Measurements in Chemical

### 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

### Thermodynamics- Chapter 19 Schedule and Notes

Thermodynamics- Chapter 19 Schedule and Notes Date Topics Video cast DUE Assignment during class time One Review of thermodynamics 1_thermo_review AND Review of thermo Wksheet 2.1ch19_intro Optional: 1sc_thermo

### Stoichiometry Chapter 9 Assignment & Problem Set

Stoichiometry Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Stoichiometry 2 Study Guide: Things You Must Know Vocabulary (know the definition

### Overview of Physical Properties of Gases. Gas Pressure

Overview of Physical Properties of Gases! volume changes with pressure! volume changes with temperature! completely miscible! low density gases: < 2 g/l liquids and solids: 1000 g/l Gas Pressure force

### Gas particles move in straight line paths. As they collide, they create a force, pressure.

#28 notes Unit 4: Gases Ch. Gases I. Pressure and Manometers Gas particles move in straight line paths. As they collide, they create a force, pressure. Pressure = Force / Area Standard Atmospheric Pressure

### ENERGY. Thermochemistry. Heat. Temperature & Heat. Thermometers & Temperature. Temperature & Heat. Energy is the capacity to do work.

ENERGY Thermochemistry Energy is the capacity to do work. Chapter 6 Kinetic Energy thermal, mechanical, electrical, sound Potential Energy chemical, gravitational, electrostatic Heat Heat, or thermal energy,

### CHEMICAL QUANTITIES. Chapter 10

CHEMICAL QUANTITIES Chapter 10 What is a mole? A unit of measurement in chemistry 1 mole of a substance = 6.02 x 10 23 (Avagadro s number) representative particles of a substance Representative particle

### AT Chapter 3 Notes 15.notebook. September 29, Measuring Atomic Masses

Measuring Atomic Masses Mass Spectrometer used to isolate isotopes of an element and determine their mass. 1 An element sample is heated to vaporize it and the gaseous atoms are zapped with an electron

### Unit 9 Stoichiometry Notes (The Mole Continues)

Unit 9 Stoichiometry Notes (The Mole Continues) 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

### Chemistry Final Exam Review

Name: Date: Block: Chemistry Final Exam Review 2012-2013 Unit 1: Measurement, Numbers, Scientific Notation, Conversions, Dimensional Analysis 1. Write 0.000008732 in scientific notation 8.732x10-6 2. Write

### 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?

### Chemistry 110 Lecture Unit 5 Chapter 11-GASES

Chemistry 110 Lecture Unit 5 Chapter 11-GASES I. PROPERITIES OF GASES A. Gases have an indefinite shape. B. Gases have a low density C. Gases are very compressible D. Gases exert pressure equally in all

### Chemical Quantities: The Mole Chapter 7 Assignment & Problem Set

Chemical Quantities: The Mole Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Chemical Quantities: The Mole 2 Study Guide: Things You Must Know

### Thermodynamics. Energy can be used * to provide heat * for mechanical work * to produce electric work * to sustain life

Thermodynamics Energy can be used * to provide heat * for mechanical work * to produce electric work * to sustain life Thermodynamics is the study of the transformation of energy into heat and for doing

### Chapter 3 Stoichiometry: Calculations with Chemical Formulas and Equations

CHE11 Chapter Chapter Stoichiometry: Calculations with Chemical Formulas and Equations 1. When the following equation is balanced, the coefficients are. NH (g) + O (g) NO (g) + H O (g) (a). 1, 1, 1, 1

### Gas Laws. The kinetic theory of matter states that particles which make up all types of matter are in constant motion.

Name Period Gas Laws Kinetic energy is the energy of motion of molecules. Gas state of matter made up of tiny particles (atoms or molecules). Each atom or molecule is very far from other atoms or molecules.

### 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,

### 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

### 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

### CHEMISTRY Practice exam #4 answer key October 16, 2007

CHEMISTRY 123-01 Practice exam #4 answer key October 16, 2007 1. An endothermic reaction causes the surroundings to a. warm up. b. become acidic. c. condense. 2. Which of the following is an example of

### 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

### 6/27/2014. Periodic Table of the ELEMENTS. Chemical REACTIONS you should know. Brief Review for 1311 Honors Exam 2

Brief Review for 3 Honors Exam 2 Chapter 2: Periodic Table I. Metals. Representative Metals Alkali Metals Group Alkaline Earth Metals. Group 2 2. Transition Metals II. Metalloids Chapter 3: All Chapter

### Chapter 5 Thermochemistry

Chapter 5 Thermochemistry I. Nature of Energy Energy units SI unit is joule, J From E = 1/2 mv 2, 1J = 1kg. m 2 /s 2 Traditionally, we use the calorie as a unit of energy. 1 cal = 4.184J (exactly) The

### Solution. Practice Exercise. Concept Exercise

Example Exercise 9.1 Atomic Mass and Avogadro s Number Refer to the atomic masses in the periodic table inside the front cover of this textbook. State the mass of Avogadro s number of atoms for each of

### Molecular Formula: Example

Molecular Formula: Example A compound is found to contain 85.63% C and 14.37% H by mass. In another experiment its molar mass is found to be 56.1 g/mol. What is its molecular formula? 1 CHAPTER 3 Chemical

### AP Chemistry Prep - Summer Assignment 2013

AP Chemistry Prep - Summer Assignment 2013 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Which value has only 4 significant digits? a. 6.930 c. 8450

### INTRODUCTORY CHEMISTRY Concepts and Critical Thinking

INTRODUCTORY CHEMISTRY Concepts and Critical Thinking Sixth Edition by Charles H. Corwin Chapter 9 The Mole Concept by Christopher Hamaker 2011 Pearson Education, Inc. Chapter 9 1 Avogadro s Number Avogadro

### How many moles are in a breath of air whose volume is 2.32L at body temperature (37 C) and a pressure of 745 torr?

Lecture 9 State of gas described by (n,p,v,t) n # moles P pressure V volume T (absolute) temperature (K) Sample Problem A balloon filled with helium has a volume of 1.60 L at 1.00 atm and 25oC. What will

### 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

### 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.

### AP Chemistry ( MCSEMENICK2015 ) My Courses Course Settings Chemistry: The Central Science, 12e Brown/LeMay/Bursten/Murphy/Woodward

Signed in as Daniel Semenick, Instructor Help Sign Out AP Chemistry ( MCSEMENICK2015 ) My Courses Course Settings Chemistry: The Central Science, 12e Brown/LeMay/Bursten/Murphy/Woodward Instructor Resources

### Review - After School Matter Name: Review - After School Matter Tuesday, April 29, 2008

Name: Review - After School Matter Tuesday, April 29, 2008 1. Figure 1 The graph represents the relationship between temperature and time as heat was added uniformly to a substance starting at a solid

### 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

### Practice questions for Chapter 8

Practice questions for Chapter 8 2) How many atoms of nickel equal a mass of 58.69 g? (Refer to the Periodic Table.) A) 1 B) 28 C) 58.69 D) 59 E) 6.02 x 1023 Answer: E Section: 8.1 Avogadro's Number 6)

### CHAPTER 12. Gases and the Kinetic-Molecular Theory

CHAPTER 12 Gases and the Kinetic-Molecular Theory 1 Gases vs. Liquids & Solids Gases Weak interactions between molecules Molecules move rapidly Fast diffusion rates Low densities Easy to compress Liquids

### 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

### 5. Which temperature is equal to +20 K? 1) 253ºC 2) 293ºC 3) 253 C 4) 293 C

1. The average kinetic energy of water molecules increases when 1) H 2 O(s) changes to H 2 O( ) at 0ºC 3) H 2 O( ) at 10ºC changes to H 2 O( ) at 20ºC 2) H 2 O( ) changes to H 2 O(s) at 0ºC 4) H 2 O( )

### Boyles Law. At constant temperature the volume occupied by a fixed amount of gas is inversely proportional to the pressure on the gas 1 P = P

Boyles Law At constant temperature the volume occupied by a fixed amount of gas is inversely proportional to the pressure on the gas 1 or k 1 Boyles Law Example ressure olume Initial 2.00 atm 100 cm 3

### CHEMISTRY. Stoichiometry

Stoichiometry 1gram molecular mass 6.022 x 10 23 molecules Avagadro No of particles 6.022 x 10 23 particles MOLE 1 gram atomic mass 6.022 x 10 23 atoms Molar volume 22.4dm 3 at STP Equivalent mass of an

### Mole Notes.notebook. October 29, 2014

1 2 How do chemists count atoms/formula units/molecules? How do we go from the atomic scale to the scale of everyday measurements (macroscopic scale)? The gateway is the mole! But before we get to the

### Campbell Chemistry Chapter 13 (&12): Gas Laws Unit Packet

Campbell Chemistry Chapter 13 (&12): Gas Laws Unit Packet Name: Date In Class Homework 1/5 Tue 1/6 Wed 1/7 Thur 1/8 Fri 1/11 Mon. LSM Welcome (back), Semester Plan, Gas Law Activities Computers: set up

### STOICHIOMETRY. - the study of the quantitative aspects of chemical

STOICHIOMETRY - the study of the quantitative aspects of chemical GENERAL PLAN FOR STOICHIOMETRY Mass reactant Mass product Moles reactant Stoichiometric factor Moles product STOICHIOMETRY It rests on

### 2. If pressure is constant, the relationship between temperature and volume is a. direct b. Inverse

Name Unit 11 Review: Gas Laws and Intermolecular Forces Date Block 1. If temperature is constant, the relationship between pressure and volume is a. direct b. inverse 2. If pressure is constant, the relationship

### Subscripts and Coefficients Give Different Information

Chapter 3: Stoichiometry Goal is to understand and become proficient at working with: 1. Chemical equations (Balancing REVIEW) 2. Some simple patterns of reactivity 3. Formula weights (REVIEW) 4. Avogadro's

### CHEMISTRY GAS LAW S WORKSHEET

Boyle s Law Charles Law Guy-Lassac's Law Combined Gas Law For a given mass of gas at constant temperature, the volume of a gas varies inversely with pressure PV = k The volume of a fixed mass of gas is

### 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

### AP* Chemistry THERMOCHEMISTRY

AP* Chemistry THERMOCHEMISTRY Terms for you to learn that will make this unit understandable: Energy (E) the ability to do work or produce heat ; the sum of all potential and kinetic energy in a system

### Chemical Reactions Chapter 8 Assignment & Problem Set

Chemical Reactions Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Chemical Reactions 2 Study Guide: Things You Must Know Vocabulary (know the

### CHE 105 Summer 2016 EX2

CHE 105 Summer 2016 EX2 Your Name: Your ID: Question #: 1 How many grams of H2SO4 (molar mass = 98.08 g/mol) are in 0.23 moles of H2SO4? Do not include units in your answer. 1 grams 1. Question #: 2 When

### Example. c. Calculate the amount of heat (in kj) required to heat 1.00 kg (~1 L) of water at 25 C to its boiling point.

Example When consuming an ice-cold drink, one must raise the temperature of the beverage to 37.0 C (normal body temperature). Can one lose weight by drinking ice-cold beverages if the body uses up about

### Name Date Class THERMOCHEMISTRY. SECTION 17.1 THE FLOW OF ENERGY HEAT AND WORK (pages 505 510)

17 THERMOCHEMISTRY SECTION 17.1 THE FLOW OF ENERGY HEAT AND WORK (pages 505 510) This section explains the relationship between energy and heat, and distinguishes between heat capacity and specific heat.

### Potassium + Chlorine. K(s) + Cl 2 (g) 2 KCl(s)

Types of Reactions Consider for a moment the number of possible chemical reactions. Because there are millions of chemical compounds, it is logical to expect that there are millions of possible chemical

### 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

### THERMOCHEMISTRY & DEFINITIONS

THERMOCHEMISTRY & DEFINITIONS Thermochemistry is the study of the study of relationships between chemistry and energy. All chemical changes and many physical changes involve exchange of energy with the

### 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

### CHEMISTRY 3310 PROBLEM SHEET #4

CHEMISTRY 3310 PROBLEM SHEET #4 1. The specific heats of a number of materials are listed below. Calculate the molar heat capacity for each. (a) gold, (b) rust (Fe 2 O 3 ) (c) sodium chloride 2. Calculate

### Calorimeter: A device in which the heat associated with a specific process is measured.

1 CALORIMETRY p. 661-667 (simple), 673-675 (bomb) Calorimeter: A device in which the heat associated with a specific process is measured. There are two basic types of calorimeters: 1. Constant-pressure

Thermochemistry Reading: Chapter 5 (omit 5.8) As you read ask yourself What is meant by the terms system and surroundings? How are they related to each other? How does energy get transferred between them?