Question

yuu al cyuIUM? 16. Consider the reaction C(s) + H2O (1) CO(g) + Hz (g) (a) At a certain temperature, K for this reaction is 0.569. If one starts with 0.200 moles of carbon and water, and 0.300 atm of CO and 0.300 atm of H2, in which direction will the reaction proceed? (b) What is the equilibrium partial pressure of the CO gas at the same temperature? SSD SSD bewonn an to

Answer 1

6.

(a)

The concentrations of solids and pure liquids do not appear in the equilibrium constant expression.

The equilibrium constant $K=P^{eq}_{CO} \times P^{eq}_{H2}$

The reaction quotient $Q=P_{CO} \times P_{H2}$

$Q=0.300 \times 0.300$

$Q=0.0900$

The equilibrium constant $K=0.569$

The reaction quotient Q is less than the equilibrium constant K.

Hence, the product partial pressure is less than equilibrium value.

Hence, the reaction will proceed in forward direction to produce more CO and hydrogen.

(b)

$K=P^{eq}_{CO} \times P^{eq}_{H2}$

But

$P^{eq}_{CO} = P^{eq}_{H2}$

Hence,

$K=P^{eq}_{CO} \times P^{eq}_{CO}$

$K=\left ( P^{eq}_{CO} \right )^2$

$P^{eq}_{CO} =\sqrt{K}$

$P^{eq}_{CO} =\sqrt{0.569}$

$P^{eq}_{CO} =0.754 \ atm$