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_(2) O_(4)(g)` are mixed at 400 K at partial pressures 20 bar and 2 bar respectively, more `N_(2)O_(4) (g)` will be formed,
D. The entropy of the system increases.

Answer

A, C, D

Explanation

(a) As the value of K increases with increase of temperature and `K=(k_(f))/(k_(b))`, this means that `k_(f)` increases, i.e., formard reaction is favoured. Hence, reaction is endothermic.
(c) At 400 K, `Q=(p_(NO_(2))^(2))/(p_(N_(2)O_(4)))=((20)^(2))/(2) = 200 `. Thus `Q gt K`. Equilibrium will shift backward to form more `N_(2)O_(4)`.
(d) As reaction is accompanied by increase in the number of moles , entropy increases.