Consider the following reaction at 25 °C: 3 NiO(s) + 2 NH₃(g) → 3 Ni(s) + N₂(g) + 3 H₂O(g) a. If ∆G° = -18.1 kJ/mol, determine the value of the equilibrium constant at 25 °C. b. Estimate the temperature at which this reaction would be at equilibrium assuming that enthalpy and entropy are independent at temperature. c. Determine the value of delta G assuming that a mixture contains 57.6g of NiO, 182.3 g of Ni, 0.24 atm of NH3, 8.54 atm of N2 and 10.07 atm of H2O.
Consider the following reaction at 25 °C: 3 NiO(s) + 2 NH₃(g) → 3 Ni(s) + N₂(g) + 3 H₂O(g) a. If ∆G° = -18.1 kJ/mol, determine the value of the equilibrium constant at 25 °C. b. Estimate the temperature at which this reaction would be at equilibrium assuming that enthalpy and entropy are independent at temperature. c. Determine the value of delta G assuming that a mixture contains 57.6g of NiO, 182.3 g of Ni, 0.24 atm of NH3, 8.54 atm of N2 and 10.07 atm of H2O.
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter4: Energy And Chemical Reactions
Section: Chapter Questions
Problem 59QRT: Which molecule, HF, HCl, HBr, or HI, has the strongest chemical bond?
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Consider the following reaction at 25 °C:
3 NiO(s) + 2 NH₃(g) → 3 Ni(s) + N₂(g) + 3 H₂O(g)
a. If ∆G° = -18.1 kJ/mol, determine the value of the equilibrium constant at 25 °C.
b. Estimate the temperature at which this reaction would be at equilibrium assuming that enthalpy and entropy are independent at temperature.
c. Determine the value of delta G assuming that a mixture contains 57.6g of NiO, 182.3 g of Ni, 0.24 atm of NH3, 8.54 atm of N2 and 10.07 atm of H2O.
Transcribed Image Text:Compound AH° (kJ/mol)
(J/mol·K)
NiO (s)
-239.7
38.0
Ni (s)
29.9
NH3 (g)
-46.0
192.5
N2 (g)
191.5
H2O (g)
-241.8
188.7
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