A flask is charged with 3.00 atm of dinitrogen tetroxide gas and 2.00 atm of nitrogen dioxide gas at 25ºC and allowed to reach equilibrium.

N2O4 (g) - ->2 NO2 (g) Kp = 0.316

Which of the following best describes the system within the flask once equilibrium has been established?

The rate of the decomposition of N2O4 (g) is equal to the rate of formation of NO2 (g).

The partial pressure of N2O4 (g) is equal to the partial pressure of NO2 (g).

The rate of the decomposition of N2O4 (g) is greater than the rate of formation of NO2 (g).

The rate of the decomposition of N2O4 (g) is less than the rate of formation of NO2 (g).

Question

Angelo Hayden

Chemistry

26 May, 08:53

A flask is charged with 3.00 atm of dinitrogen tetroxide gas and 2.00 atm of nitrogen dioxide gas at 25ºC and allowed to reach equilibrium.

N2O4 (g) - ->2 NO2 (g) Kp = 0.316

Which of the following best describes the system within the flask once equilibrium has been established?

The rate of the decomposition of N2O4 (g) is equal to the rate of formation of NO2 (g).

The partial pressure of N2O4 (g) is equal to the partial pressure of NO2 (g).

The rate of the decomposition of N2O4 (g) is greater than the rate of formation of NO2 (g).

The rate of the decomposition of N2O4 (g) is less than the rate of formation of NO2 (g).

+3

Answers (1)

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Caden Fields · Answer 1

The correct answer is The rate of decomposition of N2O4 is equal to the rate of formation of NO2.

Explanation:

According to theory of reaction kinetics we all know that at equilibrium the amount of reactant is equal to the amount of product.

In other word it can be stated that the rate of the decomposition of N2O4 is equal to the rate of the formation of NO2.