Question

This reaction is carried out at a different temperature with initial concentrations of [CO]=0.27M and [H2]=0.49M. At equilibrium, the concentration of CH3OH is 0.11 M. Find the equilibrium constant at this temperature.

Answer 1

Answer:

9.43 is the equilibrium constant at this temperature.

Explanation:

Initial concentrations of CO = [CO] = 0.27M

Initial concentrations of hydrogen = $[H_2]$ =0.49M.

Equilibrium concentration of methanol = $[CH_3OH]=0.11 M$

$CO+2H_2\rightleftharpoons CH-3OH$

initially

0.27 M      0.49 M     0

At equilibrium

(0.27-0.11) M   (0.49-2 × 0.11)M       0.11 M

The expression of an equilibrium constant can be written as:

$K_c=\frac{[CH_3OH]}{[CO][H_2]^2}$

$K_c=\frac{0.11 M}{(0.27-0.11)((0.49-2\times 0.11))^2}$

$K_c=9.43$

9.43 is the equilibrium constant at this temperature.