Test Prep Series for AP Chemistry for Chemistry: The Central Science 14th ed AP

14th Edition

ISBN: 9780134661483

Author: Edward L Waterman

Publisher: PEARSON

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Textbook Question

Chapter 5.5, Problem 5.7.2PE

Practice Exercise 2
A 0.5865-g sample of lactic acid (HC₃H₅O₃) reacts with oxygen in a calorimeter whose heat capacity is 4.812kJ/°C. The temperature increases from 23.10 to 24.95 °C. Calculate the heat of combustion of lactic acid

per gram and
per mole.

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Chapter 5.5, Problem 5.7.1PE

Chapter 5.6, Problem 5.8.1PE

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A 150.9-g sample of a metal at 74.5°C is added to 150.9 g H2O at 15.1°C. The temperature of the water rises to 18.4°C. Calculate the specific heat capacity of the metal, assuming that all the heat lost by the metal is gained by the water. The specific heat capacity of water is 4.18 J/°C•g. Specific heat capacity J/°C•9 Submit Answer Try Another Version 3 item attempts remaining Not Visited

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Chapter 5 Solutions

Test Prep Series for AP Chemistry for Chemistry: The Central Science 14th ed AP

Ch. 5.2 - A mixture of gases A2 and B2 are introduced to a...Ch. 5.2 - Practice Exercise 2 Calculate the change in the...Ch. 5.3 - A solid sample of Zn(OH)2 is added to 0.350 L of...Ch. 5.3 - Practice Exercise 2 Calculate the work, in J, if...Ch. 5.3 - Practice Exercise 1 A chemical reaction that gives...Ch. 5.3 - Prob. 5.3.2PE Ch. 5.4 - Prob. 5.4.1PE Ch. 5.4 - Prob. 5.4.2PE Ch. 5.5 - The coinage metals (Group 1B) copper, silver, and...Ch. 5.5 - Prob. 5.5.2PE

Ch. 5.5 - Practice Exercise 1 When 0.243 g of Mg metal is...Ch. 5.5 - Practical exercise 2 When 50.0 mL of 0.100MAgNO3...Ch. 5.5 - Prob. 5.7.1PE Ch. 5.5 - Practice Exercise 2 A 0.5865-g sample of lactic...Ch. 5.6 - Prob. 5.8.1PE Ch. 5.6 - Prob. 5.8.2PE Ch. 5.6 - Calculate H for the reaction C(s)+...Ch. 5.6 - Prob. 5.9.2PE Ch. 5.7 - Prob. 5.10.1PE Ch. 5.7 - Prob. 5.10.2PE Ch. 5.7 - Prob. 5.11.1PE Ch. 5.7 - Prob. 5.11.2PE Ch. 5.7 - Practice Exercise 1 Given 2SO2(g) + 02(g) —>...Ch. 5.7 - Prob. 5.12.2PE Ch. 5.8 - Use the average bond enthalpies in Table 5.41to...Ch. 5.8 - Use the average bond enthalpies in Table 5.4 to...Ch. 5.9 - Prob. 5.14.1PE Ch. 5.9 - Prob. 5.14.2PE Ch. 5 - One of the important ideas of thermodynamics is...Ch. 5 - Two positively charged spheres, each with a charge...Ch. 5 - SI The accompanying photo shows a pipevine...Ch. 5 - Consider the accompanying energy diagram. Does...Ch. 5 - The contents of the closed box in each of the...Ch. 5 - Imagine that you are climbing a mountain. Is the...Ch. 5 - The diagram shows four states of a system, each...Ch. 5 - You may have noticed that when you compress the...Ch. 5 - Imagine a container placed in a tub of water, as...Ch. 5 - In the accompanying cylinder diagram, a chemical...Ch. 5 - Prob. 10E Ch. 5 - Consider the two diagrams that follow. Based on...Ch. 5 - Consider the conversion of compound A into...Ch. 5 - What is the electrostatic potential energy (in...Ch. 5 - What is the electrostatic potential energy (in...Ch. 5 - The electrostatic force (not energy) of attraction...Ch. 5 - Use the equations given in Problem 5.15 to...Ch. 5 - A sodium ion, Na+, with a charge of 1.6 x 10-19 C...Ch. 5 - A magnesium ion, Mg2+, with a charge of 3.2 x...Ch. 5 - Identify the force present and explain whether...Ch. 5 - Identify the force present and explain whether...Ch. 5 - Which of the following cannot leave or enter a...Ch. 5 - Prob. 22E Ch. 5 - According to the first law of thermodynamics, what...Ch. 5 - Write an equation that expresses the first law of...Ch. 5 - Calculate AB and determine whether the process is...Ch. 5 - For the following processes, calculate the change...Ch. 5 - A gas is confined to a cylinder fitted with a...Ch. 5 - Consider a system consisting of two oppositely...Ch. 5 - What is meant by the term state function? Give an...Ch. 5 - Indicate which of the following is independent of...Ch. 5 - During a normal breath, our lungs expand about...Ch. 5 - How much work (in J) is involved in a chemical...Ch. 5 - Why is the change in enthalpy usually easier to...Ch. 5 - Under what condition will the enthalpy change of a...Ch. 5 - Assume that the following reaction occurs at...Ch. 5 - Suppose that the gas-phase reaction 2NO(g) + 02(g)...Ch. 5 - A gas is confined to a cylinder under constant...Ch. 5 - A gas is confined to a cylinder under constant...Ch. 5 - The complete combustion of ethanol, C2H5OH(l), to...Ch. 5 - The decomposition of Ca(OH)2(s) into CaO(s) and...Ch. 5 - Ozone, 03(9), is a form of elemental oxygen that...Ch. 5 - 5.42 Without referring to tables, predict which...Ch. 5 - Consider the following reaction: 2 Mg(s) + 02(g)2...Ch. 5 - 544 Consider the following reaction: 2...Ch. 5 - When solutions containing silver ions and chloride...Ch. 5 - At one time, a common means of forming small...Ch. 5 - 5.47 Consider the combustion of liquid methanol,...Ch. 5 - 5.48 Consider the decomposition of liquid...Ch. 5 - 5.49 a What are the units of molar heat...Ch. 5 - Two solid objects, A and B, are placed in boiling...Ch. 5 - What is the specific heat of liquid water? What is...Ch. 5 - 5.52 a. Which substance in Table 5.2 requires...Ch. 5 - The specific heat of octane, C8H18(l), is 2.22...Ch. 5 - 6.54 Consider the data about gold metal in...Ch. 5 - When a 6-50-g sample of solid sodium hydroxide...Ch. 5 - 5.56 a. When a 4 25-g sample of solid ammonium...Ch. 5 - A 2.200-g sample of quinone (C5H402) is burned in...Ch. 5 - 8.68 A 1.800-g sample of phenol (C6H5OH) was...Ch. 5 - Under constant-volume conditions, the heat of...Ch. 5 - 5.60 Under constant-volume conditions, the heat...Ch. 5 - 5.61 Can you use an approach similar to Hess's...Ch. 5 - 5.62 Consider the following hypothetical...Ch. 5 - Calculate the enthalpy change for the reaction...Ch. 5 - From the enthalpies of reaction calculate H for...Ch. 5 - From the enthalpies of reaction Calculate H for...Ch. 5 - Given the data use Hess's law to calculate H for...Ch. 5 - 5.67 What is meant by the term standard...Ch. 5 - S 5.68 What is the value of the standard enthalpy...Ch. 5 - For each of the following compounds, write a...Ch. 5 - Write balanced equations that describe the...Ch. 5 - The following is known as the thermite reaction:...Ch. 5 - 5.72 Many portable gas heaters and grills use...Ch. 5 - Using values from Appendix C , calculate the...Ch. 5 - 5.74 Using values from Appendix C, calculate the...Ch. 5 - Complete combustion of 1 mol of acetone (C2H6O)...Ch. 5 - Calcium carbide (CaC2) reacts with water to form...Ch. 5 - 5.77 Gasoline is composed primarily of...Ch. 5 - Prob. 78E Ch. 5 - Ethanol (C2H5OH) is blended with gasoline as an...Ch. 5 - 5.80 Methanol (CH3OH) is used as a fuel in race...Ch. 5 - 5.81 Without doing any calculations, predict the...Ch. 5 - 5.82 Without doing any calculations, predict...Ch. 5 - Use bond enthalpies in Table 5.4 Q to estimate for...Ch. 5 - Use bond enthalpies in Table 5.40 to estimate for...Ch. 5 - Use enthalpies of formation given in Appendix C to...Ch. 5 - 5.86 The nitrogen atoms in an N2 molecule are...Ch. 5 - 5.87 Consider the reaction 2H(g) + O2(g) ...Ch. 5 - 5.88 Consider the reaction H2(g) + I2(s) ...Ch. 5 - 5.89 What is meant by the term fuel value? Which...Ch. 5 - 5.90 Which releases the most energy when...Ch. 5 - 5.91 A serving of a particular ready-to-serve...Ch. 5 - 5.92 A pound of plain M&M® candies contains 96 g...Ch. 5 - 5.93 The heat of combustion of fructose,...Ch. 5 - 5.94 The heat of combustion of ethanol,...Ch. 5 - 5.95 The standard enthalpies of formation of...Ch. 5 - 5.98 It is interesting to compare the ‘fuel...Ch. 5 - At the end of 2012, global population was about...Ch. 5 - 5.98 The automobile fuel called E85 consists of...Ch. 5 - The air bags that provide protection in...Ch. 5 - 5.100 An aluminum can of a soft drink is placed...Ch. 5 - 5.101 Consider a system consisting of the...Ch. 5 - A sample of gas is contained in a...Ch. 5 - Limestone stalactites and stalagmites are formed...Ch. 5 - Consider the systems shown in Figure 5.10. In one...Ch. 5 - 5.105 A house is designed to have passive solar...Ch. 5 - 5.108 A coffee-cup calorimeter of the type shown...Ch. 5 - 5.107 When a 0.235-9 sample of benzoic acid is...Ch. 5 - 5.108 Meals-ready-to-eat (MREs) are military...Ch. 5 - 5.109 Burning methane in oxygen can produce three...Ch. 5 - Prob. 110AE Ch. 5 - 5.111 From the following data for three...Ch. 5 - The hydrocarbons acetylene (C2H2) and benzene...Ch. 5 - Ammonia (NH3) boils at -33 °C; at this temperature...Ch. 5 - 5.114 Three common hydrocarbons that contain four...Ch. 5 - 5.115 A 201-lb man decides to add to his exercise...Ch. 5 - 5.116 TheSun supplies about 1.0 kilowatt of...Ch. 5 - 5.117 Itis estimated that the net amount of...Ch. 5 - 5.118 At 20 °C (approximately room temperature)...Ch. 5 - Suppose an Olympic diver who weighs 52.0 kg...Ch. 5 - 5.120 Consider the combustion of a single...Ch. 5 - 5.121 Consider the following unbalanced...Ch. 5 - Consider the following acid-neutralization...Ch. 5 - 5.123 Consider two solutions, the first being...Ch. 5 - The precipitation reaction between AgNO3(aq) and...Ch. 5 - 5.125 A sample of a hydrocarbon is combusted...Ch. 5 - 5.126 The methane molecule, CH4, has the geometry...Ch. 5 - 5.127 One of the best-selling light, or...

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Practice Exercise 2 A 0.5865-g sample of lactic acid (HC 3 H 5 O 3 ) reacts with oxygen in a calorimeter whose heat capacity is 4.812kJ/°C. The temperature increases from 23.10 to 24.95 °C. Calculate the heat of combustion of lactic acid per gram and per mole.

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Chapter 5 Solutions