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Consider the following equilibrium: MnO(s) + H2(g)– Mn(s) + H2O(g) a) Using the standard chemical thermodynamic properties listed below, calculate the equilibrium constant for the reaction at T = 1000 K. Be sure to show any intermediate values in your calculation, but you do not need to write out the equations. MnO(s) H2(g) Substance AH° (298.15 K) [kJ mol-1] S° (298.15 K) [J K-1 mol-1]. Mn(s) H2O(g) -385.22 -241.82 59.71 130.57 32.01 188.72

Consider the following equilibrium: MnO(s) + H2(g)– Mn(s) + H2O(g) a) Using the standard chemical thermodynamic properties listed below, calculate the equilibrium constant for the reaction at T = 1000 K. Be sure to show any intermediate values in your calculation, but you do not need to write out the equations. MnO(s) H2(g) Substance AH° (298.15 K) [kJ mol-1] S° (298.15 K) [J K-1 mol-1]. Mn(s) H2O(g) -385.22 -241.82 59.71 130.57 32.01 188.72

Chemistry by OpenStax (2015-05-04)
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter16: Thermodynamics
Section: Chapter Questions
Problem 61E: The evaporation of one mole of water at 298 K has a standard free allergy change of 8.58 kJ....
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Consider the following equilibrium: MnO(s) + H2(g) S Mn(s) + H2O(g) a) Using the standard chemical thermodynamic properties listed below, calculate the equilibrium constant for the reaction at T = 1000 K. Be sure to show any intermediate values in your calculation, but you do not need to write out the equations. Substance MnO(s) H2(g) Mn(s) H2O(g) AH° (298.15 K) [kJ mol-1] S° (298.15 K) [J K-1 mol-1] -385.22 -241.82 59.71 130.57 32.01 188.72 b) Indicate the assumption(s) that you made in part a). c) At T = 1000 K, a fixed container was filled with 25 atm H2(g), 80 atm H20(g), 120 g MnO(s) and 50 g Mn(g). Calculate the reaction quotient and identify towards which direction the equilibrium will shift.
Transcribed Image Text:Consider the following equilibrium: MnO(s) + H2(g) S Mn(s) + H2O(g) a) Using the standard chemical thermodynamic properties listed below, calculate the equilibrium constant for the reaction at T = 1000 K. Be sure to show any intermediate values in your calculation, but you do not need to write out the equations. Substance MnO(s) H2(g) Mn(s) H2O(g) AH° (298.15 K) [kJ mol-1] S° (298.15 K) [J K-1 mol-1] -385.22 -241.82 59.71 130.57 32.01 188.72 b) Indicate the assumption(s) that you made in part a). c) At T = 1000 K, a fixed container was filled with 25 atm H2(g), 80 atm H20(g), 120 g MnO(s) and 50 g Mn(g). Calculate the reaction quotient and identify towards which direction the equilibrium will shift.
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