Question

Nitrogen and water react to form nitrogen monoxide and hydrogen, like this: N2(g) + 2H2O(g) → 2NO(g) +2H2(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of nitrogen, water, nitrogen monoxide, and hydrogen has the following composition: compound concentration at equilibrium H20 NO H2 0.25 M 1.3 M 0.33 M 1.2 M Calculate the value of the equilibrium constant Kc for this reaction. Round your answer to 2 significant digits

Answer 1

Answer:

Kc for this reaction is 0.43

Explanation:

This is the equilibrium:

N₂(g) + 2H₂O(g) → 2NO(g) +2H₂(g)

And we have all the concentration at equilibrium:

N₂: 0.25M

H₂ : 1.3M

NO: 0.33M

H₂: 1.2M

They are ok, because they are in MOLARITY. (mol/L)

Let's make the expression for Kc

Kc = ( [NO]² . [H₂]² ) / ([N₂] . [H₂O]²)

Kc = (0.33² . 1.2²) / (0.25 . 1.2²)

Kc = 0.4356

In two significant digits. 0.43