Question

One way to represent this equilibrium is: N2O4(g)2NO2(g) Indicate whether each of the following statements is true, T, or false, F. AT EQUILIBRIUM we can say that: 1. The concentration of NO2 is equal to the concentration of N2O4. 2. The rate of the dissociation of N2O4 is equal to the rate of formation of N2O4. 3. The rate constant for the forward reaction is equal to the rate constant of the reverse reaction. 4. The concentration of NO2 divided by the concentration of N2O4 is equal to a constant.

Answer 1

Answer:

1. The concentration of $NO_2$ is equal to the concentration of $N_2O_4$ : False

2. The rate of the dissociation of $N_2O_4$ is equal to the rate of formation of $N_2O_4$: True

3. The rate constant for the forward reaction is equal to the rate constant of the reverse reaction: False

4. The concentration of $NO_2$ divided by the concentration of $N_2O_4$ is equal to a constant : False

Explanation:

$N_2O_4(g)\rightleftharpoons 2NO_2(g)$

The concentrations of reactant and product is constant and not equal.

The rate of forward and backward reactions are equal. Thus rate of the dissociation of $N_2O_4$ is equal to the rate of formation of $N_2O_4$

For a reversible reaction, the equilibrium constant for the forward reaction is inverse of the equilibrium constant for the backward reaction and not equal.

Equilibrium constant is the ratio of the concentration of products to the concentration of reactants each term raised to its stochiometric coefficients.

$K_c=\frac{[NO_2]^2}{[N_2O_4]}$