1. Consider the following reaction and thermodynamic data. Compound AH,° (kJ/mol) (J/mol·K) 3 Ni(s) + N:(g) + 3 H:O(g)3 NiO(s) + 2 NH:(g) NIO (s) -239.7 38.0 Ni (s) 29.9 a) Calculate AH° for the reaction. NH, (g) -46.0 192.5 b) Calculate AS° for the reaction. N2 (g) 191.5 c) Determine the standard free energy for the reaction at 25 °C. H20 (g) -241.8 188.7 d) Determine the value of the equilibrium constant at 25 °C. e) Estimate the temperature at which this reaction would be at equilibrium (assuming that enthalpy and entropy are independent of temperature).
1. Consider the following reaction and thermodynamic data. Compound AH,° (kJ/mol) (J/mol·K) 3 Ni(s) + N:(g) + 3 H:O(g)3 NiO(s) + 2 NH:(g) NIO (s) -239.7 38.0 Ni (s) 29.9 a) Calculate AH° for the reaction. NH, (g) -46.0 192.5 b) Calculate AS° for the reaction. N2 (g) 191.5 c) Determine the standard free energy for the reaction at 25 °C. H20 (g) -241.8 188.7 d) Determine the value of the equilibrium constant at 25 °C. e) Estimate the temperature at which this reaction would be at equilibrium (assuming that enthalpy and entropy are independent of temperature).
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter17: Spontaneity, Entropy, And Free Energy
Section: Chapter Questions
Problem 24Q: What information can be determined from G for a reaction? Does one get the same information from G,...
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please solve subparts d. and e.
Transcribed Image Text:1. Consider the following reaction and thermodynamic data.
Compound AH;° (kJ/mol)
(J/mol·K)
3 Ni(s) + N:(g) +3 H:O(g)
3 NiO(s) + 2 NH(g)
NIO (s)
-239.7
38.0
Ni (s)
29.9
a) Calculate AH° for the reaction.
NH3 (g)
-46.0
192.5
b) Calculate AS° for the reaction.
N2 (g)
191.5
c) Determine the standard free energy for the reaction at 25 °C.
H20 (g)
-241.8
188.7
d) Determine the value of the equilibrium constant at 25 °C.
e) Estimate the temperature at which this reaction would be at equilibrium (assuming that enthalpy and
entropy are independent of temperature).
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