In the reactions, ${\rm{PC}}{{\rm{l}}_5}\leftrightharpoons{\rm{PC}}{{\rm{l}}_3} + {\rm{C}}{{\rm{l}}_2},$, the amounts of ${\rm{PC}}{{\rm{l}}_5},{\rm{PC}}{{\rm{l}}_3}$ and ${\rm{C}}{{\rm{l}}_2}$ at equilibrium are $2$ mole each and the total pressure is $3$ $atm$. The equilibrium constant ${K_p}$ is :

NEET UG CHEMISTRY MCQ: Equilibrium

1 Easy

1 of 1

Application +4 | -1

In the reactions,

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

, the amounts of

\mathrm{PC}{\mathrm{l}_5},\mathrm{PC}{\mathrm{l}_3}

and

\mathrm{C}{\mathrm{l}_2}

at equilibrium are

2

mole each and the total pressure is

3

atm

. The equilibrium constant

{K_p}

is :

View answer and explanation

Correct option: A

1.0\mathrm{ }\;atm

Option A (

1.0\mathrm{ }\;atm

) is correct because it is the value of Kp calculated using partial pressures at equilibrium.

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}