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.

Answer 2

Answer:

B. The partial pressure of N2O3 will increase.

Explanation:

To predict the direction of a reaction, compare the reaction quotient Qp with the equilibrium constant Kp. The reaction quotient for this reaction is calculated as follows:

Qp = PN2O3PNO ⋅ PNO2 = 50.0200 ⋅ 250 = 0.001

Because Qp is less than Kp (0.03), there is an excess of reactants and a deficit of products. As the reaction proceeds, the amount of the product (N2O3) will increase until the reaction quotient is equal to the equilibrium constant.

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