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Refer to the reaction system C(s) + H2O(g) ↔ CO(g) + H2(g) at equilibrium for which...

Refer to the reaction system C(s) + H2O(g) ↔ CO(g) + H2(g) at equilibrium for which ΔH°rxn = +131 kJ. Assume ideal gas behavior. Predict the direction in which the above equilibrium will shift as a result of the stated change in conditions.

a) An increase in the reaction temperature.

b) A decrease in the amount of C(s).

c) A decrease in the reactor volume.

d) An increase in PH2O.

e) Addition of N2 gas to the reaction mixture.

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Answer #1

C(s) + H2O(g) ↔ CO(g) + H2(g ΔH°rxn = +131 kJ.

forward reaction is endothermic reaction.

a) An increase in the reaction temperature.

The temperature is increases the equilibrium shift to forward direction.

b) A decrease in the amount of C(s).

conc of reactants are decreases the equilibrium shift to reverse direction. So conc of C decreases the equilibrium shift to reverse direction.

c) A decrease in the reactor volume.

The equilibrium shift to reverse direction.

d) An increase in PH2O.

The pressure increases the volume or no of moles decreases side shift the equilibrium.

PH2O increases the equilibrium shift to reverse direction.

e.Addition of N2 gas to the reaction mixture.

The equilibrium shift to forward direction

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