A mixture of $0.3{\rm{ }}\;mole$ of ${{\rm{H}}_2}$ and $0.3{\rm{ }}\;mole$ of ${{\rm{I}}_2}$ is allowed to react in a 10 L evacuated flask at $500^\circ C$. The reaction is ${{\rm{H}}_2} + {{\rm{I}}_2}\leftrightharpoons2{\rm{HI}},$ the $K$ is found to be 64. The amount of unreacted ${{\rm{I}}_2}$ at equilibrium is

NEET UG CHEMISTRY MCQ: Equilibrium

1 Easy

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Application +4 | -1

A mixture of

0.3\mathrm{ }\;mole

{\mathrm{H}_2}

and

0.3\mathrm{ }\;mole

{\mathrm{I}_2}

is allowed to react in a 10 L evacuated flask at

500^\circ C

. The reaction is

{\mathrm{H}_2} + {\mathrm{I}_2}\leftrightharpoons2\mathrm{HI},

the

K

is found to be 64. The amount of unreacted

{\mathrm{I}_2}

at equilibrium is

View answer and explanation

Correct option: B

0.06\mathrm{ }\;mol

Option B (

0.06\mathrm{ }\;mol

) is correct because it represents the amount of unreacted

{\mathrm{I}_2}

at equilibrium, calculated using the equilibrium constant K.

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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}