At temperatures near 800 °C, steam passed over hot coke (a form of carbon obtained from coal) reacts to form CO and H2:C(s) + H2O(g) ⇌ CO(g) + H2(g)The mixture of gases that results is an important industrial fuel called water gas. (a) At 800 °C the equilibrium constant for thisreaction is Kp = 14.1. What are the equilibrium partial pressures of H2O, CO, and H2 in the equilibrium mixture at this temperatureif we start with solid carbon and 0.100 mol of H2O in a 1.00-L vessel? (b) What is the minimum amount of carbon requiredto achieve equilibrium under these conditions? (c) What is the total pressure in the vessel at equilibrium? (d) At 25 °C the valueof Kp for this reaction is 1.7x 10-21. Is the reaction exothermic or endothermic? (e) To produce the maximum amount of COand H2 at equilibrium, should the pressure of the system be increased or decreased?
At temperatures near 800 °C, steam passed over hot coke (a form of carbon obtained from coal) reacts to form CO and H2:
C(s) + H2O(g) ⇌ CO(g) + H2(g)
The mixture of gases that results is an important industrial fuel called water gas. (a) At 800 °C the equilibrium constant for this
reaction is Kp = 14.1. What are the equilibrium partial pressures of H2O, CO, and H2 in the equilibrium mixture at this temperature
if we start with solid carbon and 0.100 mol of H2O in a 1.00-L vessel? (b) What is the minimum amount of carbon required
to achieve equilibrium under these conditions? (c) What is the total pressure in the vessel at equilibrium? (d) At 25 °C the value
of Kp for this reaction is 1.7x 10-21. Is the reaction exothermic or endothermic? (e) To produce the maximum amount of CO
and H2 at equilibrium, should the pressure of the system be increased or decreased?
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