For the reaction N_2O_(4(g)) hArr 2NO_(2(g)) ,the value of K is 50 at 400 K and 1700 at 500 K. Which of the following options is/are correct ?

For the reaction N_2O_(4(g)) hArr 2NO_(2(g)) ,the value of K is 50 at

1.	For the reaction N_2O_(4(g)) hArr 2NO_(2(g)) ,the value of K is 50 at 400 K and 1700 at 500 K. Which of the following options is/are correct ?
Answer» The reaction is endothermic The reaction is exothermic 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. The entropy of the system increases. Solution :For the reaction, `N_2O_(4(g)) hArr 2NO_(2(g))` At 400 K, K=50 At 500 K, K=1700 (a) If the value of K increase with increase of temperature and `K_f/K_b`, Because of that `K_f`increases, i.e., forward reaction is TAKE PLACE. So, reaction is endothermic. (c) As, number of moles of gaseous products are greater than the number of moles of gaseous reactants. So, higher pressure favours the backward reaction. More `N_2O_(4(g))` will be obtained, if `P_"product" GT P_"reactant"` (d) As reaction is accompanied by increase in the number of moles, entropy increases.