Listed in the table are forward and reverse rate constant for the reaction:
`2NO(g)hArrN_(2)(g)-O_(2)(g)`
`{:("Temperature "(K),K_(f)[M^(-1)s^(-1)],K_(b)[M^(-1)s^(-1)]),(1400,0.29,1.1xx10^(-6)),(1500,1.3,1.4xx10^(-5)):}`
Select the correct statement

Options

A. Reaction is exothermic and value of equilibrium constant `(K_(eq))` at 1400 K is `3.79xx10^(-6)`
B. Reaction is endothermic and value of equilibrium constant `(K_(eq))` at 1400 K is `2.63xx10^(5)`
C. Reaction is exothermic and value of `K_(eq)` at 1400 K is `2.63xx10^(5)`
D. Reaction is endothermica and value of `K_(eq)` at 1500 K is `9.28xx10^(4)`

Answer

C

Explanation

`K_(eq)` at 1400 K `=(0.29)/(1.1xx10^(-6))=0.26xx10^(6)`
`=26xx10^(4)`
`K_(eq)` at `1500K=(1.3)/(1.4xx10^(-5))=0.92xx10^(5)`
`=92xx10^(3)`
Since, `K_(eq)` decreases on increasing temperature So reaction is exothermic