ForthereactionN_(2)O_(4)(g) hArr 2 NO_(2) (g), the value of K is 50 at 400 K and 1700 at 500 K. Which of the following options is correct ?

ForthereactionN_(2)O_(4)(g) hArr 2 NO_(2) (g), the value of K is 50 at

1.	ForthereactionN_(2)O_(4)(g) hArr 2 NO_(2) (g), the value of K is 50 at 400 K and 1700 at 500 K. Which of the following options is correct ?
Answer» <P>The REACTION is endothermic The reaction is exothermic 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, The entropy of the system increases. Solution :(a) As the value of K increases with increaseof 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.