Chemistry & Chemical Reactivity
9th Edition
ISBN: 9781305176461
Author: Kotz
Publisher: Cengage
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Chapter 5.5, Problem 2RC
For the reaction 2 CO(g) + O2(g) → 2 CO2(g). ∆rH° = −566 kJ/mol-rxn. What is the enthalpy change for the oxidation of 42.0 g of CO(g)?
- (a) −283 kJ
- (b) −425 kJ
- (c) −566 kJ
- (d) −393.5 kJ
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Identifying the major species in weak acid or weak base equilibria
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Using reaction free energy to predict equilibrium composition
Consider the following equilibrium:
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yes
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Identifying the major species in weak acid or weak base equilibria
The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at
equilibrium. You can leave out water itself.
Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the
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solution.
acids:
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Х
other: ☐
ப
acids:
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1.0 L of a solution that is
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other: ☐
00.
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Chapter 5 Solutions
Chemistry & Chemical Reactivity
Ch. 5.1 - 1. Which of the following processes is...Ch. 5.1 - 2. Your skin cools as perspiration evaporates. Is...Ch. 5.2 - You did an experiment in which you found that 59.8...Ch. 5.2 - A 15.5-g piece of chromium, heated to 100.0 C, is...Ch. 5.2 - Prob. 1RCCh. 5.2 - Prob. 2RCCh. 5.3 - Calculate the amount of energy necessary to raise...Ch. 5.3 - To make a glass of iced tea, you pour 250 mL of...Ch. 5.3 - 1. Which of the following processes requires the...Ch. 5.3 - Ice (5.0 g) at 0 C is added to 25 g of liquid...
Ch. 5.4 - Nitrogen gas (2.75 L) is confined in a cylinder...Ch. 5.4 - Which of the following processes will lead to a...Ch. 5.4 - 2. In which of the following reactions is there a...Ch. 5.5 - The combustion of ethane, C2H6, has an enthalpy...Ch. 5.5 - 1. For the reaction 2 Hg(l) + O2(g) → 2 HgO(s),...Ch. 5.5 - 2. For the reaction 2 CO(g) + O2(g) → 2 CO2(g)....Ch. 5.6 - Assume 200. mL of 0.400 M HCl is mixed with 200....Ch. 5.6 - A 1.00-g sample of ordinary table sugar (sucrose,...Ch. 5.6 - A student used a coffee-cup calorimeter to...Ch. 5.6 - If, in the experiment described in the previous...Ch. 5.7 - Use Hesss law to calculate the enthalpy change for...Ch. 5.7 - Calculate the standard enthalpy of combustion for...Ch. 5.7 - Prob. 1RCCh. 5.7 - The standard enthalpies of formation of KNO3(s)...Ch. 5.7 - Prob. 2QCh. 5.7 - The decomposition of nitroglycerin (C3H5N3O9)...Ch. 5.7 - Prob. 2RCCh. 5 - Define the terms system and surroundings. What...Ch. 5 - What determines the directionality of energy...Ch. 5 - Identify whether the following processes are...Ch. 5 - Identify whether the following processes are...Ch. 5 - The molar heat capacity of mercury is 28.1 J/mol ...Ch. 5 - The specific heat capacity of benzene (C6H6) is...Ch. 5 - The specific heat capacity of copper metal is...Ch. 5 - How much energy as heat is required to raise the...Ch. 5 - The initial temperature of a 344-g sample of iron...Ch. 5 - After absorbing 1.850 kJ of energy as heat, the...Ch. 5 - A 45.5-g sample of copper at 99.8 C is dropped...Ch. 5 - One beaker contains 156 g of water at 22 C, and a...Ch. 5 - A 182-g sample of gold at some temperature was...Ch. 5 - When 108 g of water at a temperature of 22.5 C is...Ch. 5 - A 13.8-g piece of zinc is heated to 98.8 C in...Ch. 5 - A 237-g piece of molybdenum, initially at 100.0 C,...Ch. 5 - How much energy is evolved as heat when 1.0 L of...Ch. 5 - The energy required to melt 1.00 g of ice at 0 C...Ch. 5 - How much energy is required to vaporize 125 g of...Ch. 5 - Chloromethane, CH3CI, arises from microbial...Ch. 5 - The freezing point of mercury is 38.8 C. 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CH3CO2H, is made industrially by the...Ch. 5 - You mix 125 mL of 0.250 M CsOH with 50.0 mL of...Ch. 5 - You mix 125 mL of 0.250 M CsOH with 50.0 mL of...Ch. 5 - A piece of titanium metal with a mass of 20.8 g is...Ch. 5 - A piece of chromium metal with a mass of 24.26 g...Ch. 5 - Adding 5.44 g of NH4NO3(s) to 150.0 g of water in...Ch. 5 - You should use care when dissolving H2SO4 in water...Ch. 5 - Sulfur (2.56 g) was burned in a constant-volume...Ch. 5 - Suppose you burned 0.300 g of C(s) in an excess of...Ch. 5 - Suppose you burned 1.500 g of benzoic acid,...Ch. 5 - A 0.692-g sample of glucose, C6H12O6, was burned...Ch. 5 - An ice calorimeter can be used to determine the...Ch. 5 - A 9.36-g piece of platinum was heated to 98.6 C in...Ch. 5 - The enthalpy changes for the following reactions...Ch. 5 - The enthalpy changes of the following reactions...Ch. 5 - Enthalpy changes for the following reactions can...Ch. 5 - You wish to know the enthalpy change for the...Ch. 5 - Write a balanced chemical equation for the...Ch. 5 - Write a balanced chemical equation for the...Ch. 5 - (a) Write a balanced chemical equation for the...Ch. 5 - (a) Write a balanced chemical equation for the...Ch. 5 - Use standard enthalpies of formation in Appendix L...Ch. 5 - Use standard enthalpies of formation in Appendix L...Ch. 5 - The first step in the production of nitric acid...Ch. 5 - The Romans used calcium oxide, CaO, to produce a...Ch. 5 - The standard enthalpy of formation of solid barium...Ch. 5 - An important step in the production of sulfuric...Ch. 5 - The enthalpy change for the oxidation of...Ch. 5 - The enthalpy change for the oxidation of styrene....Ch. 5 - Prob. 65GQCh. 5 - Prob. 66GQCh. 5 - For each of the following, define a system and its...Ch. 5 - Prob. 68GQCh. 5 - Use Appendix L to find the standard enthalpies of...Ch. 5 - You have a large balloon containing 1.0 mol of...Ch. 5 - Determine whether energy as heat is evolved or...Ch. 5 - Determine whether energy as heat is evolved or...Ch. 5 - Use standard enthalpies of formation to calculate...Ch. 5 - Which evolves more energy on cooling from 50 C to...Ch. 5 - You determine that 187 J of energy as heat is...Ch. 5 - Calculate the quantity of energy required to...Ch. 5 - You add 100.0 g of water at 60.0 C to 100.0 g of...Ch. 5 - Three 45-g ice cubes at 0 C are dropped into 5.00 ...Ch. 5 - Suppose that only two 45-g ice cubes had been...Ch. 5 - You take a diet cola from the refrigerator and...Ch. 5 - The standard molar enthalpy of formation of...Ch. 5 - Chloromethane, CH3Cl, a compound found throughout...Ch. 5 - Prob. 83GQCh. 5 - Camping stoves are fueled by propane (C3H8),...Ch. 5 - Prob. 85GQCh. 5 - Prob. 86GQCh. 5 - (a) Calculate the enthalpy change, rH, for the...Ch. 5 - You drink 350 mL of diet soda that is at a...Ch. 5 - Chloroform, CHCl3, is formed from methane and...Ch. 5 - Water gas, a mixture of carbon monoxide and...Ch. 5 - Using standard enthalpies of formation, verify...Ch. 5 - A piece of lead with a mass of 27.3 g was heated...Ch. 5 - A 192-g piece of copper is heated to 100.0 C in a...Ch. 5 - Insoluble AgCl(s) precipitates when solutions of...Ch. 5 - Insoluble PbBr2(s) precipitates when solutions of...Ch. 5 - The value of U for the decomposition of 7.647 g of...Ch. 5 - A bomb calorimetric experiment was run to...Ch. 5 - The meals-ready-to-eat (MREs) in the military can...Ch. 5 - On a cold day, you can warm your hands with a heat...Ch. 5 - Without doing calculations, decide whether each of...Ch. 5 - Prob. 102SCQCh. 5 - You want to determine the value for the enthalpy...Ch. 5 - Prepare a graph of specific heat capacities for...Ch. 5 - Prob. 105SCQCh. 5 - You are attending summer school and living in a...Ch. 5 - Prob. 107SCQCh. 5 - Prob. 108SCQCh. 5 - Prob. 109SCQCh. 5 - Peanuts and peanut oil are organic materials and...Ch. 5 - Isomers are molecules with the same elemental...Ch. 5 - Prob. 112SCQCh. 5 - Prob. 113SCQCh. 5 - A piece of gold (10.0 g, CAu = 0.129 J/g K) is...Ch. 5 - Methane, CH4, can be converted to methanol, which,...Ch. 5 - Calculate rH for the reaction 2 C(s) + 3 H2(g) + ...Ch. 5 - You have the six pieces of metal listed below,...Ch. 5 - Sublimation of 1.0 g of dry ice. CO2(s), forms...Ch. 5 - In the reaction of two moles of gaseous hydrogen...
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