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Ch.9 - Thermochemistry: Chemical Energy
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All textbooksMcMurry 8th EditionCh.9 - Thermochemistry: Chemical EnergyProblem 98

Chapter 9, Problem 98

What is a compound's standard heat of formation?

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Hello everyone today. We have the following question which of the following statements defines the standard heat of formation of a compound. So this is essentially just asking us the definition of the standard heat of formation. So the standard heat of formation of a compound, this is the answer choice is going to be C. The standard heat of formation of a compound is the amount of heat associated with the formation of one mole of the compound from the standard states of its element. So once again, the standard heat of formation of a compound is the amount of heat associated with the formation of one mole of the compound from the standard states of its element. So in other words, how much he is being generated when you form one mole of this compound? I hope this helped, and until next time.
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Related Practice
Textbook Question
Hess's law can be used to calculate reaction enthalpies for hypothetical processes that can't be carried out in the labo- ratory. Set up a Hess's law cycle that will let you calculate ∆H° for the conversion of methane to ethylene: 2 CH4(g) → C2H4(g) + 2 H2(g) You can use the following information: 2 C2H6(g) + 7 O2(g) → 4 CO2(g) + 6 H2O(l) ∆H° = -3120.8 kJ CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(l) ∆H° = -890.3 kJ C2H4(g) + H2(g) → C2H6(g) ∆H° = -136.3 kJ H2O(l) ∆H°f = -285.8 kJ/mol
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Textbook Question
Find ∆H° in kilojoules for the reaciton of nitric oxide with oxygen, 2 NO(g) + O2(g) → N2O4(g), given the following data: N2O4(g) → 2 NO2(g) ∆H° = 55.3 kJ NO(g) + 1/2 O2(g) → NO2(g) ∆H° = -58.1 kJ
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Textbook Question
Set up a Hess's law cycle, and use the following information to calculate ΔH°f for aqueous nitiric acid, HNO3(aq). You will need to use fractional coefficients for some equations. 3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g) ΔH° = -137.3 kJ 2 NO(g) + O2(g) → 2 NO2(g) ΔH° = -116.2 kJ 4 NH3(g) + 5 O2(g) → 4 NO (g) + 6 H2O(l) ΔH° = -1165.2 kJ NH3(g) ΔH°f = -46.1 kJ/mol H2O(l) ΔH°f = -285.8 kJ/mol
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Textbook Question
How is the standard state of an element defined? Why do elements always have ∆H°f = 0?
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What phase of matter is associated with the standard states of the following elements and compounds? (a) Cl2 (b) Hg (c) CO2 (d) Ga
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Textbook Question
What is the phase of the standard states of the following ele- ments and compounds? (a) NH3 (b) Fe (c) N2 (d) Br2
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