At 200^(@)C, the equilibrium N_(2)O_(4)(g)hArr2NO_(2)(g) is achieved in the following two pathways: (i) 0.1 mol N_(2)O_(4) is heated in a closed vassel of 1 L volume. (ii) a mixture of 0.05 mol N_(2)O_(4)(g) and 0.05 mol NO_(2)(g) is heated at 200^(@)C in a closed vessel of 1 L volume. in these two cases, will the equilibrium concentrations of N_(2)O_(4)(g) and NO_(2)(g) and the values of equilibrium constants be the same?

At 200^(@)C, the equilibrium N_(2)O_(4)(g)hArr2NO_(2)(g) is achieved i

1.	At 200^(@)C, the equilibrium N_(2)O_(4)(g)hArr2NO_(2)(g) is achieved in the following two pathways: (i) 0.1 mol N_(2)O_(4) is heated in a closed vassel of 1 L volume. (ii) a mixture of 0.05 mol N_(2)O_(4)(g) and 0.05 mol NO_(2)(g) is heated at 200^(@)C in a closed vessel of 1 L volume. in these two cases, will the equilibrium concentrations of N_(2)O_(4)(g) and NO_(2)(g) and the values of equilibrium constants be the same?
Answer» SOLUTION :The value of equilibrium constant of a reaction depends only on TEMPERATURE it does not depend on the initial CONCENTRATIONS of the reactants. Since temperature is the same for both experiments, the value of equilibrium constant will be the same in both cases. the initial concentrations of the reactant(s) in the two experiment are not the same. As a RESULT, the molar concentrations of `N_(2)O_(4)(g) and NO_(2)(g)` at equilibrium will be different in the two experiments.