Ch.9 - Thermochemistry: Chemical Energy
McMurry8th EditionChemistryISBN: 9781292336145
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- Ch.1 - Chemical Tools: Experimentation & Measurement167
- Ch.2 - Atoms, Molecules & Ions145
- Ch.3 - Mass Relationships in Chemical Reactions162
- Ch.4 - Reactions in Aqueous Solution199
- Ch.5 - Periodicity & Electronic Structure of Atoms91
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory66
- Ch.7 - Covalent Bonding and Electron-Dot Structures59
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure59
- Ch.9 - Thermochemistry: Chemical Energy114
- Ch.10 - Gases: Their Properties & Behavior121
- Ch.11 - Liquids & Phase Changes52
- Ch.12 - Solids and Solid-State Materials72
- Ch.13 - Solutions & Their Properties70
- Ch.14 - Chemical Kinetics84
- Ch.15 - Chemical Equilibrium70
- Ch.16 - Aqueous Equilibria: Acids & Bases86
- Ch.17 - Applications of Aqueous Equilibria101
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium77
- Ch.19 - Electrochemistry137
- Ch.20 - Nuclear Chemistry82
- Ch.21 - Transition Elements and Coordination Chemistry126
- Ch.22 - The Main Group Elements92
- Ch.23 - Organic and Biological Chemistry11
Chapter 9, Problem 12
A table of standard enthalpies of formation (ΔH°f) gives a value of −467.9 kJ/mol for NaNO3(s). Which reaction has a ΔH° value of −467.9 kJ? (a) Na+ (aq) + NO3−(aq) → NaNO3(s) (b) Na(s) + N(g + O3(g) → NaNO3(s) (c) Na(s) + 1/2 N2(g) + 3/2 O2(g) → NaNO3(s) (d) 2 Na(s) + N2(g) + 3 O2(g) → 2 NaNO3(s)
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Related Practice
Textbook Question
A 25.0 g piece of granite at 100.0°C was added to 100.0 g of water of 25.0°C, and the temperature rose to 28.4°C. What is the specific heat capacity of the granite? (The specific heat capacity for water is 4.18 J/(g•°C).) (LO 9.10)
(a) 0.563 J/(g•°C)
(b) 1.53 J/(g•°C)
(c) 0.992 J/(g•°C)
(d) 0.794 J/(g•°C)
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Textbook Question
When 12.5 g of NH4NO3 is dissolved in 150.0 g of water of 25.0 °C in a coffee cup calorimeter, the final temperature of the solution of 19.7 °C. Assume that the specific heat of the solution is the same as that of water, 4.18 J/(g•°C). What is the ΔH per mol of NH4NO3? (LO 9.10) NH4NO3 (s) → NH4+ (aq) + NO3−(aq) ΔH = ? (a) +3.60 kJ (b) +23.0 kJ (c) +21.3 kJ (d) −3.60 kJ
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Textbook Question
Calculate the enthalpy change for the reaction
C(s) + 2 H2(g) → CH4(g) ΔH = ?
Given the enthalpy values for the following reactions
CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(l) ΔH = −890.4 kJ
C(s) + O2(g) → CO2(g) ΔH = −393.5 kJ
H2(g) + 1/2 O2(g) → H2O (g) ΔH = −285.8 kJ
(a) −1569.7 kJ
(b) +211.1 kJ
(c) −1855.5 kJ
(d) −74.7 kJ
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Textbook Question
What is ΔH for the explosion of nitroglycerin? (LO 9.14)
2 C3H5(NO3)3(l) → 3 N2(g) + 1/2 O2(g) + 6 CO2(g) + 5 H2O(g)
(a) −315.0 kJ
(b) −4517 kJ
(c) −3425 kJ
(d) −3062 kJ
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Textbook Question
A piece of dry ice (solid CO2) is placed inside a balloon, and the balloon is tied shut. Over time, the carbon dioxide sub- limes, causing the balloon to increase in volume. Give the sign of the enthalpy change and the sign of work for the sublima-
tion of CO2.
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Textbook Question
Imagine a reaction that results in a change in both volume and temperature: (a) Has any work been done? If so, is its sign positive or negative?
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