When H_2(g) is mixed with CO_2(g) at 2000 K, the equilibrium is achieved accordi

Question

When H_2(g) is mixed with CO_2(g) at 2000 K, the equilibrium is achieved according to the equation below, H_2(g) + CO_2(g) rightarrow H_2O(g) + CO(g) In one experiment, the following equilibrium concentrations were measured; [H_2] = 0.150 M [CO_2] = 0.400 M [H_2O] = [CO] = 0.550 M Calculate the value of K_c, the equilibrium constant for the reaction. In a different experiment, 0.75 mol H_2(g) is mixed with 0.75 mol of CO_2(g) in a 3.00 liter reaction vessel at 2000 K. Calculate the equilibrium concentrations, in moles per liter of all species at this temperature.

Explanation / Answer

a ) yes first one is correct

b)   use Kc value which you solved in 4a)

molarity of   H2 = 0.75 / 3 = 0.25 M

molarity of CO2 = 0.75 / 3 = 0.25 M

H2   + CO2 <-----------------> CO + H2O

0.25     0.25                            0         0 ----------------> initial

0.25-x 0.25-x                         x        x --------------> equilibrium

Kc = [CO][H2O]/[H2][CO2]

Kc = x^2 / (0.25 -x)^2

5.04 = x^2 / (0.25-x)^2

2.24 = x / 0.25 - x

x = 0.168

equilibrium concentrations :

[H2] = 0.25 - x = 0.25 - 0.168 = 0.082 M

[CO2]= 0.25 - x = 0.25 - 0.168 = 0.082 M

[H2O] = x = 0.168 M

[CO] = x = 0.168 M

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