# R = J/mol K R = L atm/mol K

Save this PDF as:

Size: px
Start display at page:

Download "R = J/mol K R = L atm/mol K"

## Transcription

1 version: master Exam 1 - VDB/LaB/Spk This MC portion of the exam should have 19 questions. The point values are given with each question. Bubble in your answer choices on the bubblehseet provided. Your score is based on what you bubble on the bubblesheet and not what is circled on the exam. Below are some constants you might want to use. Water Data T fp = 0 C T bp = 100 C 1 C ice = 2.09 J g 1 K 1 C water = J g 1 K 1 C steam = 2.03 J g 1 K H vap = 2260 J g 1 H fus = 334 J g 1 K b = C/m K f = 1.86 C/m R = J/mol K R = L atm/mol K Figure pressure (torr) temperature (K) 166 Phase Diagram for Xenon 1 What are the signs for the change in enthalpy and change in entropy when a system undergoes the phase transition of freezing? (4 pts) A. H < 0, S < 0 B. H < 0, S > 0 C. H > 0, S < 0 D. H > 0, S > 0 Explanation: Freezing is a transition from a liquid to a solid. This is both exothermic (solids are lower in enthalpy than liquids) and it lowers the entropy (solids are lower in entropy than liquids). 2 In which solvent do you expect hexane (C 6 H 14 ) to be miscible? (4 pts) A. C 5 H 12 B. CH 3 OH C. H 2 O D. CH 3 CN E. CH 3 COOH Explanation: miscible liquids should have similar intermolecular forces (like dissolves like). Hexane is non-polar and only has dispersion interactions. The same is true for pentane C 5 H Calculate the number of grams of nitrogen gas that will dissolve in 125 L of water if the partial pressure of the nitrogen gas is 0.79 atm. Henry s law constant for nitrogen gas is M/atm. (4 pts) A. 1.7 g B g C g D g

2 version: master Exam 1 - VDB/LaB/Spk page 2 Explanation: Henry s law constant times the partial pressure of the gas above the solution is equal to the concentration of the dissolved gas in the solution: C gas = k H P gas C gas = (0.79) = M You then convert concentration to moles by multiplying by volume: ( )(125) = moles. Mass is obtained by multiplying the moles of nitrogen by its molar mass: ( mol)(28 g/mol) = 1.7 g. 4 What mass of potassium can be produced by the reaction of g of Na with g of KCl? Na + KCl NaCl + K (4 pts) A g B g C g D g Explanation: This is a limiting reagent question. To decide the amount of K formed, you must first decide which is the limiting reactant. The Na to KCl molar ratio is one to one. So whichever reactant has the fewer number of moles at the start is the limiting reactant. Since the mass of each is the same and KCl has a greater molar mass than Na, the KCl will be the limiting reactant. To determine the amount of grams K produced start with what is given and convert to grams K. ( g KCl 1 ) ( ) ( ) ( ) 1 mol KCl 1 mol K 39.1 g K = g K g KCl 1 mol KCl 1 mol K 5 You have a sample containing 15 grams of solid ethanol together with 15 g of liquid ethanol. The sample is at the freezing temperature of ethanol, -114 C. What happens when you initially place this mixture in a deep freezer which is held at -180 C and energy flows out of the sample in the form of heat? (4 pts) A. The temperature of the sample increases while the liquid ethanol freezes. B. The temperature of the sample decreases while the liquid ethanol freezes. C. The temperature of the sample remains constant while the liquid ethanol freezes. D. The temperature of the sample remains constant while the solid ethanol melts. E. The temperature of the sample remains constant and the relative amount of liquid and solid ethanol remains constant. Explanation: none 6 You have a sample of Xe at 164 K and 760 torr. You reduce the pressure to 250 torr. According to figure 1, what happens? (4 pts) A. Nothing. No phase change occurs. B. It vaporizes. C. It solidifies. D. It melts. E. It condenses. Explanation: The substance is a liquid at the given starting temperature and pressure. As we reduce the pressure to the new 250 torr value, we cross the vapor pressure line into the gas region.

3 version: master Exam 1 - VDB/LaB/Spk page 3 7 You have a 100 g sample of water at standard pressure and 70 C. How much energy is required to heat this sample to steam at 120 C? (4 pts) A. 243 kj B. 21 kj C. 239 kj D. 247 kj E. 185 kj F. 17 kj Explanation: You have three steps: The heat required to heat the water to the boiling point, the heat required to boil the water, and the heat required to heat the steam to 120 C. 8 Which aqueous solution would you expect to have the highest boiling point? (4 pts) A. 0.2 M sugar B. 0.2 M KCl C. 0.2 M Na 2 SO 4 D. All of these solutions would have the same boiling point. Explanation: The sodium sulfate will have the highest effective molality: the highest concentration of solute particles in solution, since each sodium sulfate will ionize into two sodium ions and one sulfate ion. 9 According to figure 1, what is the normal boiling point of Xe? (4 pts) A. 166 K B. 152 K C. 161 K D. < 152 K E. > 166 K Explanation: Then normal boiling point is the temperature at which the vapor pressure equals 760 torr. 10 An aqueous solution at 25 C contains 35 grams of a non-ionizing solute with MW = 83.1 g/mol. The total mass of the solution is 215 grams. The vapor pressure of pure water at 25 C is torr. What is the vapor pressure of the solution? (4 pts) A torr B torr C torr D torr E torr Explanation: none 11 What is the boiling point of an aqueous solution of 1.2 m CaCl 2? (4 pts) A C B C C C D C E C Explanation: The solution has three ions, so the net concentration is 3.6 m. The change in boiling point is (3.6 m)(0.512 C m 1 ) = 1.8 C. So the new boiling point is = C.

4 version: master Exam 1 - VDB/LaB/Spk page 4 12 You have a solution that contains 25 g of an unknown non-ionizing polymer in a 250 ml solution of chloroform (CHCl 3 ). The osmotic pressure of this solution at 25 C is found to be atm. What is the molecular weight of the unknown solid? (4 pts) A. 43,500 g mol 1 B. 3,650 g mol 1 C. 10,870 g mol 1 D. 41,000 g mol 1 E. 1,740 g mol 1 Explanation: The osmotic pressure is given by Π = MRT. Using R = L-atm K 1 mol 1 and T = K the concentration of the solution is M = (0.056 atm) ( L atm K 1 mol 1 )(298.15K) = Since volume of the solution is 250 ml, this means you have a total of moles of solute. Given the mass of 25g this gives a molecular weight of MW = = 43, 500 g/mol 25 g moles 13 The solubility of PbBr 2 is 8.44 g/l at 20 C. What is K sp for this compound? (4 pts) A B C D E Explanation: (8.44g/L / 367g/mol) =.023 M. [Pb 2+ ] = M, [Br ] = M. K sp = [Pb 2+ ][Br ] 2 = (0.023)(0.046) 2 = Which of the following compounds has the lowest solubility in water? (4 pts) A. PbBr 2, K sp = B. AgI, K sp = C. Sr 3 (PO 4 ) 2, K sp = D. Ag(CH 3 COO), K sp = Explanation: You can approximate the molar solubility as the n th root of the K sp. For AgI this is about 10 8 M. That is the smallest value. Sr 3 (PO 4 ) 2 ) has the smallest K sp, but it makes 5 ions. So the solubility is approximately the 5th root of the K sp or You have an aqueous solution that contains a wide array of different ions along with a solid chunk of Ag 3 PO 4 (K sp = ) in it. The concentration of PO 3 4 in the solution is M. What is the concentration of the silver ion? (4 pts) A M B M C M D M E M Explanation: K sp = [Ag + ] 3 [PO 3 4 ] = [Ag + ] 3 ( ). [Ag + ] = M 16 You have two closed containers with ether. Each container has a total volume of 1L. One container is filled with 750 ml of liquid ether. The other container has 500 ml of liquid ether. How does the partial pressure of the ether in the gas phase above the liquid compare in the two containers? (4 pts) A. It is the same in both containers. B. It is higher in the container with 750 ml. C. It is higher in the container with 500 ml. Explanation: The vapor pressure is independent of the amount of liquid or the volume the gas can occupy.

5 version: master Exam 1 - VDB/LaB/Spk page 5 17 Which of the following would have the lowest vapor pressure? (4 pts) A. NH 3 B. CH 3 NH 2 C. C 4 H 9 NH 2 D. C 8 H 17 NH 2 Explanation: All will have hydrogen bonding, but C 8 H 17 NH 2 will have significantly more dispersion forces. The stronger IMFs will lead to a lower vapor pressure. 18 The vapor pressure of liquids increases as the temperature increases because (4 pts) A. at a higher temperatures the kinetic energy distribution of molecules shifts to higher values. B. intermolecular forces have a strength that is inversely proportional to temperature. C. vapor pressure does not increase with temperature, it decreases. D. as temperature increases the volume increases. E. the enthalpy decreases with increasing temperature. Explanation: As the temperature increases the kinetic energy of the molecules increase. Therefore compared to the intermolecular forces holding them in the liquid state, more of them have a sufficient energy to enter the gas phase. 19 K sp = for Ba(NO 3 ) 2. What is the concentration of the nitrate ion in a saturated Ba(NO 3 ) 2 solution? (4 pts) A M B M C M D M E M F M Explanation: K sp = [Ba 2+ ][NO 3 ]2. [Ba 2+ ] = x. [NO 3 ] = 2x. Therefore K sp = 4x 3 = 4.64 x x = M. [NO 3 ] = 2x = M. Make sure you complete the front and back of the free response portion. Remember to bubble in ALL your answers BEFORE time is called. Sign your exam, bubblesheet, AND free response page. Turn in ALL parts: exam copy, bubblesheet, and free response.

### 48 Practice Problems for Ch. 17 - Chem 1C - Joseph

48 Practice Problems for Ch. 17 - Chem 1C - Joseph 1. Which of the following concentration measures will change in value as the temperature of a solution changes? A) mass percent B) mole fraction C) molality

### Chem. 1A Final Exam Review Problems From ch. 11, 12 & 13

Chem. A Final Exam Review Problems From ch., 2 & 3 f Multiple Choice Identify the choice that best completes the statement or answers the question.. Place the following cations in order from lowest 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

### Sample Test 1 SAMPLE TEST 1. CHAPTER 12

13 Sample Test 1 SAMPLE TEST 1. CHAPTER 12 1. The molality of a solution is defined as a. moles of solute per liter of solution. b. grams of solute per liter of solution. c. moles of solute per kilogram

### 1. How many of the following compounds will exhibit hydrogen bonding?

Spring 2002 Test 1 1. ow many of the following compounds will exhibit hydrogen bonding? N A. 1 B. 2 C. 3 D. 4 E. 5 N C 3 Cl N N C O OC 2 C 2 O 2. Which of the following is indicative of the existence of

### Unit 13 Practice Test

Name: Class: Date: Unit 13 Practice Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1) The dissolution of water in octane (C 8 H 18 ) is prevented by.

### CHEMISTRY The Molecular Nature of Matter and Change

CHEMISTRY The Molecular Nature of Matter and Change Third Edition Chapter 13 The Properties of Mixtures: Solutions and Colloids Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction

### 1. solid, vapor, critical point correct. 2. solid, liquid, critical point. 3. liquid, vapor, critical point. 4. solid, liquid, triple point

mcdonald (pam78654) HW 7B: Equilibria laude (89560) 1 This print-out should have 18 questions. Multiple-choice questions may continue on the next column or page find all choices before answering. 001 10.0

### Sample Exercise 13.1 Predicting Solubility Patterns

Sample Exercise 13.1 Predicting Solubility Patterns Predict whether each of the following substances is more likely to dissolve in the nonpolar solvent carbon tetrachloride (CCl 4 ) or in water: C 7 H

### Name: Thermochemistry. Practice Test B. General Chemistry Honors Chemistry

Name: Thermochemistry B Practice Test B General Chemistry Honors Chemistry 1 Objective 1: Use the relationship between mass, specific heat, and temperature change to calculate the heat flow during a chemical

### Name Date Class. SECTION 16.1 PROPERTIES OF SOLUTIONS (pages 471 477)

16 SOLUTIONS SECTION 16.1 PROPERTIES OF SOLUTIONS (pages 471 477) This section identifies the factors that affect the solubility of a substance and determine the rate at which a solute dissolves. Solution

### Chapter 13. Properties of Solutions

Sample Exercise 13.1 (p. 534) By the process illustrated below, water vapor reacts with excess solid sodium sulfate to form the hydrated form of the salt. The chemical reaction is Na 2 SO 4(s) + 10 H 2

### Colligative Properties of Nonvolatile Solutes 01. Colligative Properties of Nonvolatile Solutes 02. Colligative Properties of Nonvolatile Solutes 04

Colligative Properties of Nonvolatile Solutes 01 Colligative Properties of Nonvolatile Solutes 02 Colligative Properties: Depend on the amount not on the identity There are four main colligative properties:

### From the book (10, 12, 16, 18, 22, 24 52, 54, 56, 58, 62, 64, 66, 68, 74, 76, 78, 80, 82, 86, 88, 90, 92, 106 and 116)

Chem 112 Solutions From the book (10, 12, 16, 18, 22, 24 52, 54, 56, 58, 62, 64, 66, 68, 74, 76, 78, 80, 82, 86, 88, 90, 92, 106 and 116) 1. Which of the following compounds are nonelectrolytes? A. NaF

### Chapter 14 Solutions

Chapter 14 Solutions 1 14.1 General properties of solutions solution a system in which one or more substances are homogeneously mixed or dissolved in another substance two components in a solution: solute

### Chapter 12: Solutions

Chapter 12: Solutions Problems: 3, 5, 8, 12, 14, 16, 22, 29, 32, 41-58, 61-68, 71-74 solution: homogeneous mixture of a solute dissolved in a solvent solute: solvent: component present in smaller amount

### Chapter 14. Mixtures

Chapter 14 Mixtures Warm Up What is the difference between a heterogeneous and homogeneous mixture? Give 1 example of a heterogeneous mixture and 1 example of a homogeneous mixture. Today s Agenda QOTD:

### CHEM 36 General Chemistry EXAM #1 February 13, 2002

CHEM 36 General Chemistry EXAM #1 February 13, 2002 Name: Serkey, Anne INSTRUCTIONS: Read through the entire exam before you begin. Answer all of the questions. For questions involving calculations, show

### CHAPTER 13: ANSWERS TO ASSIGNED PROBLEMS Hauser- General Chemistry I revised 8/03/08

CHAPTER 13: ANSWERS TO ASSIGNED PROBLEMS Hauser- General Chemistry I revised 8/03/08 13.21 The solubility of Cr(NO 3 ) 3 9 H 2 O in water is 208 g per 100 g of water at 15 C. A solution of Cr(NO 3 ) 3

### Solutions. Occur in all phases. Ways of Measuring. Ways of Measuring. Energy of Making Solutions. 1. Break apart Solvent. Page 1

s Occur in all phases The solvent does the dissolving. The solute is dissolved. There are examples of all types of solvents dissolving all types of solvent. We will focus on aqueous solutions. Ways of

### Types of Solutions. Chapter 17 Properties of Solutions. Types of Solutions. Types of Solutions. Types of Solutions. Types of Solutions

Big Idea: Liquids will mix together if both liquids are polar or both are nonpolar. The presence of a solute changes the physical properties of the system. For nonvolatile solutes the vapor pressure, boiling

### Chapter 13. Properties of Solutions

13.4 Ways of Expressing Concentration All methods involve quantifying the amount of solute per amount of solvent (or solution). Concentration may be expressed qualitatively or quantitatively. The terms

### Colligative Properties

Colligative Properties Vapor pressures have been defined as the pressure over a liquid in dynamic equilibrium between the liquid and gas phase in a closed system. The vapor pressure of a solution is different

### Colligative Properties. Vapour pressure Boiling point Freezing point Osmotic pressure

Colligative Properties Vapour pressure Boiling point Freezing point Osmotic pressure Learning objectives Describe meaning of colligative property Use Raoult s law to determine vapor pressure of solutions

### Element of same atomic number, but different atomic mass o Example: Hydrogen

Atomic mass: p + = protons; e - = electrons; n 0 = neutrons p + + n 0 = atomic mass o For carbon-12, 6p + + 6n 0 = atomic mass of 12.0 o For chlorine-35, 17p + + 18n 0 = atomic mass of 35.0 atomic mass

### Chemical Equations C5.6b Predict single replacement reactions.

Chemistry 2SEM Chemical Equations C5.6b Predict single replacement reactions. Common Assessment Review Predict the following single replacement reactions: a. Zn + Pb(C2H3O2)2 ----> Pb + Zn(C2H3O2)2_ b.

### Solutions. Occur in all phases. Ways of Measuring. Ways of Measuring. Page 1

Solutions Occur in all phases The solvent does the dissolving. The solute is dissolved. There are examples of all types of solvents dissolving all types of solvent. We will focus on aqueous solutions.

### Two Ways to Form Solutions. Role of Disorder in Solutions 2/27/2012. Types of Reactions

Role of Disorder in Solutions Disorder (Entropy) is a factor Solutions mix to form maximum disorder Two Ways to Form Solutions 1. Physical Dissolving (Solvation) NaCl(s) Na + (aq) + Cl - (aq) C 12 H 22

### Unit 3: Solubility Equilibrium

Unit 3: Chem 11 Review Preparation for Chem 11 Review Preparation for It is expected that the student understands the concept of: 1. Strong electrolytes, 2. Weak electrolytes and 3. Nonelectrolytes. CHEM

### Exam 3 Chemistry 65 Summer Score:

Name: Exam 3 Chemistry 65 Summer 2015 Score: Instructions: Clearly circle the one best answer 1. The main interactions between molecules of iodine I2 are examples of A) ionic bonds. B) covalent bonds.

### 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.

### 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

### COLLIGATIVE PROPERTIES:

COLLIGATIVE PROPERTIES: A colligative property is a property that depends only on the number of solute particles present, not their identity. The properties we will look at are: lowering of vapor pressure;

### CHE 107 Exam 1 Spring 2016

CHE 107 Exam 1 Spring 2016 Your Name: Your ID: Question #: 1 Molecular View State Density Shape Volume Strength of Intermolecu lar Forces solid high definite definite 1 [strong, weak] liquid high indefinite

### 2. Why does the solubility of alcohols decrease with increased carbon chain length?

Colligative properties 1 1. What does the phrase like dissolves like mean. 2. Why does the solubility of alcohols decrease with increased carbon chain length? Alcohol in water (mol/100g water) Methanol

### 1) What is the overall order of the following reaction, given the rate law?

PRACTICE PROBLEMS FOR TEST 2 (March 11, 2009) 1) What is the overall order of the following reaction, given the rate law? A) 1st order B) 2nd order C) 3rd order D) 4th order E) 0th order 2NO(g) + H 2(g)

### Name Class Date. In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question.

Assessment Chapter Test A Chapter: States of Matter In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. 1. The kinetic-molecular

### Chapter 13 Properties of Solutions. Classification of Matter

Chapter 13 Properties of Solutions Learning goals and key skills: Describe how enthalpy and entropy changes affect solution formation Describe the relationship between intermolecular forces and solubility,

### Chemical Equations and Calculations

Chemical Equations and Calculations A chemical equation is a shorthand way of indicating what is going on in a chemical reaction. We could do it the long way Two molecules of Hydrogen gas react with one

### Name: Thermochemistry. Practice Test A. General Chemistry Honors Chemistry

Name: Thermochemistry Practice Test A General Chemistry Honors Chemistry 1 Objective 1: Use the relationship between mass, specific heat, and temperature change to calculate the heat flow during a chemical

### Colligative properties CH102 General Chemistry, Spring 2014, Boston University

Colligative properties CH102 General Chemistry, Spring 2014, Boston University here are four colligative properties. vapor-pressure lowering boiling-point elevation freezing-point depression osmotic pressure

### Chapter 14 The Chemistry of Solutes and Solutions. Solute-Solvent Interactions. Solute-Solvent Interactions. Solute-Solvent Interactions

John W. Moore Conrad L. Stanitski Peter C. Jurs Solubility & Intermolecular Forces Solution = homogeneous mixture of substances. It consists of: http://academic.cengage.com/chemistry/moore solvent - component

### Ch. 11: Liquids and Intermolecular Forces

Ch. 11: Liquids and Intermolecular Forces Learning goals and key skills: Identify the intermolecular attractive interactions (dispersion, dipole-dipole, hydrogen bonding, ion-dipole) that exist between

### 12.3 Colligative Properties

12.3 Colligative Properties Changes in solvent properties due to impurities Colloidal suspensions or dispersions scatter light, a phenomenon known as the Tyndall effect. (a) Dust in the air scatters the

### H 2 (g) + ½ O 2 (g) H 2 O(l) H o f [NO(g)] = 90.2 kj/mol; H o f [H 2 O(g)] = kj/mol H o f [NH 3 (g)] = kj/mol; H o f [O 2 (g)] =?

Chapter 16 Thermodynamics GCC CHM152 Thermodynamics You are responsible for Thermo concepts from CHM 151. You may want to review Chapter 8, specifically sections 2, 5, 6, 7, 9, and 10 (except work ). Thermodynamics:

### Example: orange juice from frozen concentrate.

Dilution: a process in which the concentration (molarity) of a solution is lowered. The amount of solute (atoms, moles, grams, etc.) remains the same, but the volume is increased by adding more solvent.

### Intermolecular Forces

Intermolecular Forces: Introduction Intermolecular Forces Forces between separate molecules and dissolved ions (not bonds) Van der Waals Forces 15% as strong as covalent or ionic bonds Chapter 11 Intermolecular

### The Solution Process CHEMISTRY. Properties of Solutions. The Central Science. Prof. Demi Levendis Room GH807 Gate House

CHEMISTRY The Central Science Properties of Solutions The Solution Process Solutions: Air; brass; body fluids; sea water When a solution forms some questions we can ask are: What happens on a molecular

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

A.P. Chemistry Practice Test: Ch. 11, Solutions Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Formation of solutions where the process is

### Chapter 16 Review Packet

Chapter 16 Review Packet AP Chemistry Chapter 16 Practice Multiple Choice Portion 1. For which process is ΔS negative? Note: ΔS = S final S initial therefore, if ΔS is positive, S final > S initial if

### 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

### a) Consider mixing two liquids where mixing is exothermic ( Hsoln < 0). Would you expect a solution to form (yes/maybe/no)? Justify your answer.

Problems - Chapter 13 (with solutions) 1) The following question concerns mixing of liquids. a) Consider mixing two liquids where mixing is exothermic (Hsoln < 0). Would you expect a solution to form (yes/maybe/no)?

### Chapter 12. Solutions. Lecture Presentation

12.1 Thirsty Solutions: Why You Shouldn t Drink Seawater 544 12.2 Types of Solutions and Solubility 546 12.3 Energetics of Solution Formation 551 12.4 Solution Equilibrium and Factors Affecting Solubility

### 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

### Intermolecular forces, acids, bases, electrolytes, net ionic equations, solubility, and molarity of Ions in solution:

Intermolecular forces, acids, bases, electrolytes, net ionic equations, solubility, and molarity of Ions in solution: 1. What are the different types of Intermolecular forces? Define the following terms:

### 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

### 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.

### 1/27/2014. Chapter 12. Solutions. Thirsty Seawater. Seawater. Seawater. Homogeneous Mixtures. Seawater. Lecture Presentation

Lecture Presentation Chapter 12 Solutions Sherril Soman, Grand Valley State University Thirsty Seawater Drinking seawater can cause dehydration. Seawater Is a homogeneous mixture of salts with water Contains

### 0.279 M Change g to mol: g/mol = mol Molarity = mol L = mol 0.325L = M

118 ChemQuest 39 Name: Date: Hour: Information: Molarity Concentration is a term that describes the amount of solute that is dissolved in a solution. Concentrated solutions contain a lot of dissolved solute,

### Chemistry Ch 15 (Solutions) Study Guide Introduction

Chemistry Ch 15 (Solutions) Study Guide Introduction Name: Note: a word marked (?) is a vocabulary word you should know the meaning of. A homogeneous (?) mixture, or, is a mixture in which the individual

### CHAPTER 14 Solutions

CHAPTER 14 Solutions The Dissolution Process 1. Effect of Temperature on Solubility 2. Molality and Mole Fraction Colligative Properties of Solutions 3. Lowering of Vapor Pressure and Raoult s Law 4. Fractional

### Chapter 13: Physical Properties of Solutions

Chapter 13: Physical Properties of Solutions Key topics: Molecular Picture (interactions, enthalpy, entropy) Concentration Units Colligative Properties terminology: Solution: a homogeneous mixture Solute:

### 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( )

### C) 6 D) thermal energy B) Aluminum reacts with sulfuric acid. C) 1676 kj B) kilojoules C) Magnesium reacts with an acid. D) 100 C and 1 atm

1. What is the atomic number of the element whose atoms bond to each other in chains, rings, and networks? A) 10 B) 8 C) 6 D) 4 2. Which statement describes a chemical property of aluminum? A) Aluminum

### 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

### 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

### e) 2 CsOH + H 2 SO 4 Cs 2 SO H 2 O

1 1. Classify the following reaction? Mg(CN) 2 (s) + H 2 SO 4 (aq) MgSO 4 (aq) + 2 HCN(g) a) Single-Replacement Reaction b) Double-Replacement Reaction c) Redox Reaction d) Combination Reaction e) Neutralization

### Colligative Properties: Freezing Point Depression and Molecular Weight

Purpose: Colligative Properties: Freezing Point Depression and Molecular Weight The first purpose of this lab is to experimentally determine the van't Hoff (i) factor for two different substances, sucrose

### 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

### Chapter 13 - LIQUIDS AND SOLIDS

Chapter 13 - LIQUIDS AND SOLIDS Problems to try at end of chapter: Answers in Appendix I: 1,3,5,7b,9b,15,17,23,25,29,31,33,45,49,51,53,61 13.1 Properties of Liquids 1. Liquids take the shape of their container,

### Lab 9. Colligative Properties an Online Lab Activity

Prelab Assignment Before coming to lab: Lab 9. Colligative Properties an Online Lab Activity Chemistry 162 - K. Marr Revised Winter 2014 This lab exercise does not require a report in your lab notebook.

### 1. Define the term colligative property and list those physical properties of a solution that can be classified as colligative properties.

Solutions Colligative Properties DCI Name Section 1. Define the term colligative property and list those physical properties of a solution that can be classified as colligative properties. Colligative

### A) HCl C) 52 g KCl in 100 g water at 80ºC A) temperature of the solution increases B) supersaturated D) low temperature and high pressure D) KClO3

1. Which compound becomes less soluble in water as the temperature of the solution is increased? A) HCl B) 2. The solubility of O3(s) in water increases as the A) temperature of the solution increases

### Major chemistry laws. Mole and Avogadro s number. Calculating concentrations.

Major chemistry laws. Mole and Avogadro s number. Calculating concentrations. Major chemistry laws Avogadro's Law Equal volumes of gases under identical temperature and pressure conditions will contain

### Chapter 13 Properties of Solutions

Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 13 Properties of are homogeneous mixtures of two or more pure substances. In a solution,

### Chapter Thirteen. Physical Properties Of Solutions

Chapter Thirteen Physical Properties Of Solutions 1 Solvent: Solute: Solution: Solubility: Types of Solutions Larger portion of a solution Smaller portion of a solution A homogeneous mixture of 2 or more

### Chapter 7 Solutions 1

1 Chapter 7 Solutions Solutions: Solute and Solvent Solutions are homogeneous mixtures of two or more substances form when there is sufficient attraction between solute and solvent molecules have two components:

### Colligative Properties

Colligative Properties Say Thanks to the Authors Click http://www.ck12.org/saythanks (No sign in required) To access a customizable version of this book, as well as other interactive content, visit www.ck12.org

### Molecular Mass by Freezing Point Depression

Molecular Mass by Freezing Point Depression Kyle Miller November 28, 2006 1 Purpose The purpose of this experiment is to determine the molecular mass of organic compounds which are dissolved in a solvent

### Lecture 6: Lec4a Chemical Reactions in solutions

Lecture 6: Lec4a Chemical Reactions in solutions Zumdahl 6 th Ed, Chapter 4 Sections 1-6. 4.1 Water, the Common Solvent 4.2 The Nature of Aqueous Solutions: Strong and Weak Electrolytes 4.3 The Composition

### Calculations involving concentrations, stoichiometry

Calculations involving concentrations, stoichiometry MUDr. Jan Pláteník, PhD Mole Unit of amount of substance the amount of substance containing as many particles (atoms, ions, molecules, etc.) as present

### 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

### Chemistry 102 Chapter 17 THERMODYNAMICS

THERMODYNAMICS Thermodynamics is concerned with the energy changes that accompany chemical and physical processes. Two conditions must be fulfilled in order to observe a chemical or physical change: The

### Chemistry 212 EXAM 2 February 17, 2004 KEY

1 Chemistry 212 EXAM 2 February 17, 2004 100_ (of 100) KEY Name Part 1: Multiple Choice. (1 point 4. The equilibrium constant for the each, circle only one answer, reaction 1. For the equilibrium that

### Chemistry 1 Final Exam Study Guide Spring 2009

Chemistry 1 Final Exam Study Guide Spring 2009 1. If a substance has a mass of 36.4 g and a volume of 8.500 ml, what is its density? 2. Which involves a chemical change? a. powdering sugar b. condensing

### 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

### Phase diagram of water. Note: for H 2 O melting point decreases with increasing pressure, for CO 2 melting point increases with increasing pressure.

Phase diagram of water Note: for H 2 O melting point decreases with increasing pressure, for CO 2 melting point increases with increasing pressure. WATER Covers ~ 70% of the earth s surface Life on earth

### Chem 112 Intermolecular Forces Chang From the book (10, 12, 14, 16, 18, 20,84,92,94,102,104, 108, 112, 114, 118 and 134)

Chem 112 Intermolecular Forces Chang From the book (10, 12, 14, 16, 18, 20,84,92,94,102,104, 108, 112, 114, 118 and 134) 1. Helium atoms do not combine to form He 2 molecules, What is the strongest attractive

### 13.3 Factors Affecting Solubility Solute-Solvent Interactions Pressure Effects Temperature Effects

Week 3 Sections 13.3-13.5 13.3 Factors Affecting Solubility Solute-Solvent Interactions Pressure Effects Temperature Effects 13.4 Ways of Expressing Concentration Mass Percentage, ppm, and ppb Mole Fraction,

### Name: Class: Date: 2) Which one of the following exhibits dipole-dipole attraction between molecules? A) XeF 4 B) AsH 3 C) CO 2 D) BCl 3 E) Cl 2

Name: Class: Date: IM Bonding 1) In liquids, the attractive intermolecular forces are. A) very weak compared with kinetic energies of the molecules B) strong enough to hold molecules relatively close together

### Name Matter Questions Date:

Name Matter Questions Date: 1. Which substance has a definite shape and a definite volume at STP? 1) NaCl(aq) 2) Cl2(g) 3) CCl4( ) 4) AlCl3(s) 2. Which two particle diagrams represent mixtures of diatornic

### Chemistry Summer School Pre-Test 2015

NAME: 1. A material consists of pure sodium. How many types of atomic structures are present in this substance? (C.1.1) A. No atomic structures are present as this is a pure substance. B. One type of atomic

### Chapter mol H2S 34.08g H2S L 1 mol H S. = mg O 2 / 100 ml. = 1.48 mg N 2 / 100 ml

Practice Exercises 1.1 C H S = k H P H S P H S = 1.0 atm C H S = 0.11 mol HS 4.08g HS L 1 mol H S =.7 g L 1.7 g L 1 H S = k H (1.0 atm H s S) k H =.7 g L 1 Hydrogen sulfide is more soluble in water than

### Colligative Properties Discussion Chem. 1A

Colligative Properties Discussion Chem. 1A The material covered today is found in sections Chapter 12.5 12.7 This material will not be covered in lecture, you will have homework assigned. Chem. 1A Colligative

### Unit 2: Quantities in Chemistry

Mass, Moles, & Molar Mass Relative quantities of isotopes in a natural occurring element (%) E.g. Carbon has 2 isotopes C-12 and C-13. Of Carbon s two isotopes, there is 98.9% C-12 and 11.1% C-13. Find

### CHM1 Review for Exam 9

Topics 1. Reaction Types a. Combustion b. Synthesis c. Decomposition d. Single replacement i. Metal activity series ii. Nonmetal activity series e. Double replacement i. Precipitates and solubility rules