Question

Calculate the equilibrium constant for the reaction using the balanced chemical equation and the concentrations of the substances at equilibrium.

Use the

appropriate significant figures in reporting the answers.

CO(g) + H2O(g) ⇌ CO2(g) + H2(g) [CO] = 0.0590 M; [H2O] = 0.00600 M;

[CO2] = 0.0410 M; [H2] = 0.0410 M

K =______________-

Answer 1

The equilibrium constant for the reaction CO(g) + H₂O(g) ⇌ CO₂(g) + H₂(g) can be calculated using the concentrations of the substances at equilibrium. The equilibrium constant is approximately 0.991.

Step-by-step explanation:

The equilibrium constant for the reaction CO(g) + H₂O(g) ⇌ CO₂(g) + H₂(g) can be calculated using the concentrations of the substances at equilibrium. The equilibrium constant (K) is given by the ratio of the relative concentrations of the products and reactants. In this case, the equilibrium constant can be calculated as:

K = ([CO₂] * [H₂]) / ([CO] * [H₂O])

Substituting the given concentrations into the equation, we have:

K = (0.0410 * 0.0410) / (0.0590 * 0.00600)

Calculating the values, we find that the equilibrium constant for this reaction is approximately 0.991.

Answer 2

4.75 is the equilibrium constant for the reaction.

Step-by-step explanation:

`CO(g)+H_2O(g)\rightleftharpoons CO_2(g)+H_2(g)`

Equilibrium concentration of reactants :

`[CO]=0.0590 M,[H_2O]=0.00600 M`

Equilibrium concentration of products:

`[CO_2]=0.0410 M,[H_2]=0.0410 M`

The expression of an equilibrium constant is given by :

`K_c=([CO_2][H_2])/([CO][H_2O])`

`K_c=(0.0410 M* 0.0410 M)/(0.0590M* 0.00600 M)`

`K_c=4.75`

4.75 is the equilibrium constant for the reaction.