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 react 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 ans (a,c,d)

Answer

A, C, D

Explanation

For the reaction,` N_(2)O_(4) (g) Lefttrightarrow 2NO_(2) (g)` at 400K, K=500 at 500K, K=1700
(a) As the value of K increase with increase of temperature and `K=(K_(f))/(K_(b))`, this means that `K_(f)` increases, i.e, forward reaction is favoured.
Hence, reaction is endothermic.
(c) Since, number of moles of gaseous products are greater than the number of moles of gaseous reactants. Thus, higher pressure favours the backward reaction, i.e., more `N_(2)O_(4) (g)` will be obtained, if `P_("product") gt P_("reactant")`
d) As reaction is accomlpanied by increase in the number of moles, entropy increases.