Question

For the equilibrium: CO(g) + H2O(g) ⇌ CO2(g) + H2(g) KC = 10.0

If 1.6 mol of CO and 1.6 mol of water are initially added to a 2.0 liter flask and the flask is then heated
until the system comes to equilibrium, the concentration of hydrogen will then be _______ M

Answer 1

The balanced chemical equation for the given equilibrium is:

CO(g) + H2O(g) ⇌ CO2(g) + H2(g)

The equilibrium constant (Kc) is given as 10.0.

Initially, we have 1.6 mol of CO and 1.6 mol of H2O in a 2.0 liter flask. The initial concentration of CO and H2O can be calculated as follows:

[CO] = 1.6 mol / 2.0 L = 0.8 M
[H2O] = 1.6 mol / 2.0 L = 0.8 M

Let the concentration of H2 at equilibrium be x M. Then, the concentrations of CO2 and H2O at equilibrium will also be x M.

Using the equilibrium constant expression, we can write:

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

Substituting the values, we get:

10.0 = x^2 / (0.8) * (0.8)

Simplifying, we get:

x^2 = 6.4

x = 2.53 M

Therefore, the concentration of hydrogen at equilibrium will be 2.53 M.