14th Edition

ISBN: 9780136873891

Author: Brown

Publisher: PEARSON

Concept explainers

Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that …

Exergonic Reaction

The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energ…

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Textbook Question

Chapter 5, Problem 84E

Use bond enthalpies in Table 5.40 to estimate Chapter 5, Problem 84E, Use bond enthalpies in Table 5.40 to estimate for each of the following reactions: a. b. , example 1 for each of the following reactions:

a. Chapter 5, Problem 84E, Use bond enthalpies in Table 5.40 to estimate for each of the following reactions: a. b. , example 2

b. Chapter 5, Problem 84E, Use bond enthalpies in Table 5.40 to estimate for each of the following reactions: a. b. , example 3

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Chapter 5, Problem 83E

Chapter 5, Problem 85E

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1. In the calorimeter experiment, you mixed 50 mL of 1.0 M NaOH with 50 mL of approximately 1.0 M HC1. Suppose that 50 mL of a more concentrated solution of each were mixed. a. Should any additional heat have been released? Explain. b. Should you have obtained the same AT? Explain. c. Would the true molar enthalpy change, AH, for this reaction be different? Explain.

The enthalpy change for a chemical reaction is the sum of the energy consumed in breaking bonds and the energy released during bond formation. One way to determine the overall energy change for a chemical reaction is to apply Hess’s law to add together a group of reactions which can be arranged such that the chemical equations, when combined, give the overall equation we are trying to characterize. a. Write a balanced chemical equation for the combustion of gaseous propane in gaseous oxygen to produce gaseous carbon dioxide and liquid water. C3H8(g)+ O2(g) ---->CO2(g)+ H2O(g) b. Combine the following equations to determine the enthalpy change for the combustion of 1 mole of propane. Assume that solid carbon is graphite. 3C(s,graphite)+4H2(g)--->C3H8(g) ΔHo = -103.8 kJ/mol C(s,graphite)+O2(g)--->CO2(g) ΔHo= -393.5 kJ/mol H2(g)+1/2 O2(g)--->H2O(g) ΔHo= -285.8 kJ/mol kJ/mol…

MCQ 20: Enthalpy change of atomization involves the production of gaseous atoms from its A. atoms B. solute C. reactants D. products

Chapter 5 Solutions

CHEMISTRY THE CENTRAL SCIENCE >EBOOK<

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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