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 for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter9: Energy And Chemistry
Section: Chapter Questions
Problem 9.65PAE: 9.65 When 0.0157 g of a compound with a heat of combustion of —37.6 kJ/mol is burned in a...
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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.
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