For the reaction, ${{\rm{N}}_2}\left( {\rm{g}} \right) + {{\rm{O}}_2}\left( {\rm{g}} \right)\;\leftrightharpoons\;2{\rm{NO}}\left( {\rm{g}} \right)$, the value of ${K_c}$ at $800^\circ C$ is 0.1. When the equilibrium concentration of both the reactants is 0.5 mole, what is the value of ${K_p}$ at the same temperature?

NEET UG CHEMISTRY MCQ: Equilibrium

1 Easy

1 of 1

Application +4 | -1

For the reaction,

{\mathrm{N}_2}\left( \mathrm{g} \right) + {\mathrm{O}_2}\left( \mathrm{g} \right)\;\leftrightharpoons\;2\mathrm{NO}\left( \mathrm{g} \right)

, the value of

{K_c}

800^\circ C

is 0.1. When the equilibrium concentration of both the reactants is 0.5 mole, what is the value of

{K_p}

at the same temperature?

View answer and explanation

Correct option: B

0.1

Option B (0.1) is correct because

{K_p} = {K_c}

when the change in the number of moles of gas is zero.

Practice All Chapter MCQs →

Mg{(HC{O_3})_2}

MgC{O_3}

Mg{(OH)_2}

MgC{O_3}

K_{\mathrm{P}}

\mathrm{CaCO}_3

4.5 \times 10^{-2}

\mathrm{C}(\mathrm{s})+\mathrm{CO}_2(\mathrm{g}) \rightleftharpoons 2 \mathrm{CO}(\mathrm{g}),

K_{\mathrm{P}}

2.0 \mathrm{~atm}.

\mathrm{CaO}

\mathrm{CaCO}_3

+

\leftrightharpoons

\mathrm{PC}{\mathrm{l}_5}\leftrightharpoons\mathrm{PC}{\mathrm{l}_3} + \mathrm{C}{\mathrm{l}_2}

{K_{\mathrm{eq}}} = 0.41

\mathrm{p}{K_a}