For the reaction `N_(2)O_(4)(g)hArr2NO_(2)(g)`, the value of K is 50 at 400 K and 1700 at 500 K. Which of the following options is correct?

Options

A. The reaction is endothermic
B. The reaction is exothermic
C. If `NO_2` (g) and `N_2O_4(g)` are mixed at 400 K at partial pressures 20 bar and 2 bar respectively, more `N_2O_4(g)` will be formed.
D. The entropy of the system increases.

Answer

A, C, D

Explanation

(a) K increases with increase in temperature.
(c) Since Q is larger than K, therefore, reaction proceeds in the backward direction.
(d) Since `Deltan_g` is +ve, `Delta`S will increase.