Question

Experiments have shown that the equilibrium constant Kp for the reaction NO(g) + NO2(g) ⇌ N2O3(g) is 0.03. A chamber with a constant total pressure initially contains NO with a partial pressure of 200 MPa, NO2 with a partial pressure of 250 MPa, and N2O3 with a partial pressure of 50 MPa. What will occur over time?

Answer 1

Answer:

The reaction will shift to the right

Explanation:

In the reaction:

NO(g) + NO₂(g) ⇌ N₂O₃(g)

Kp of reaction is:

$kP = \frac{P_{N_2O_3} }{P_{NO}P_{NO_{2}}}$ = 0.03

Where P represents the pressures in equilibrium

Replacing in the kP formula the initial pressures:

$\frac{50MPa}{200MPa*250MPa}$ = 0.001

As the Reaction quotient (Q) is less than kP, the reaction will shift to the right producing more N₂O₃ until Q = kP.