CH4 (g) + H2O (g) <- -> CO (g) + 3 H2 (g) Kc=5.2 at 1768 K
a) What is the equilibrium expression for this reaction in terms of Kc?
b) Suppose that the initial concentrations of all species at 1768 K are:
[CH4] = 0.210 M, [H2O] = 0.171 M, [CO] = 0.533 M, and [H2] = 0.987 M
I. Determine the value for the reaction quotient.
II. In what direction will the reaction proceed at this temperature? Justify your answer.
c) Calculate the value of the equilibrium constant, Kp, for this reaction at 1768 K.
d) Calculate the value for the free energy change, Delta G^O 1768 K, of this reaction. Include units with your answer.
e) The equilibrium concentrations of CO and H2 increase when the temperature of the system increases. Is the forward reaction exothermic or endothermic? Justify your answer.
f) A chemist who works for a company that produces hydrogen gas suggests that they could increase the yield of H2 (g) by adjusting the volume of the equilibrium system. Should the volume be increased or decreased? Explain.
g) Calculate the value of Kc for the following reaction.
CO (g) + 3 H2 (g) <- -> CH4 (g) + H2O (g)