Given below is the data for the reaction 2 NO(g) leftharpoons N_2(~g)+O_2(~g) where ' k_ f ' and ' k_ b ' are rate constants of the forward and reverse reactions respectively Temperature (K) k_ f (mol^ -1 dm^3 ~s^ -1 )

Correct answer: C. exothermic and K_ eq at 1400 ~K=1.8 × 10^5 No Solution

Olympiad workbook

Olympiad workbook · NSEC · Chemical Equilibrium

Given below is the data for the reaction 2 NO(g) leftharpoons...

Given below is the data for the reaction

2 \mathrm{NO}(\mathrm{g}) \rightleftharpoons \mathrm{N}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g})

where '

\mathrm{k}_{\mathrm{f}}

' and '

\mathrm{k}_{\mathrm{b}}

' are rate constants of the forward and reverse reactions respectively

Temperature (K)	$k_{f} \left(mol^{-1}dm^3 ~s^{-1}\right)$	$k_{b} \left(mol^{-1}dm^3 ~s^{-1}\right)$
$1400$	$0.20$	$1.1 \times10^{-6}$
$1500$	$1.3$	$1.4 \times10^{-5}$

The reaction is

Aexothermic and $K_{e q}$ at $1400 \mathrm{~K}=3.79 \times 10^{-6}$
Bendothermic and $K_{e q}$ at $1400 \mathrm{~K}=2.63 \times 10^{-5}$
Cexothermic and $\mathrm{K}_{\mathrm{eq}}$ at $1400 \mathrm{~K}=1.8 \times 10^5$
Dendothermic and $K_{e q}$ at $1500 \mathrm{~K}=9.28 \times 10^{-4}$

C. exothermic and $\mathrm{K}_{\mathrm{eq}}$ at $1400 \mathrm{~K}=1.8 \times 10^5$

No Solution