At constant temperature in one litre vessel, when the reaction, $2{\rm{S}}{{\rm{O}}_3}\left( {\rm{g}} \right)\;\leftrightharpoons\;2{\rm{S}}{{\rm{O}}_2}\left( {\rm{g}} \right) + {{\rm{O}}_2}\left( {\rm{g}} \right)$ is at equilibrium, the ${\rm{S}}{{\rm{O}}_2}$ concentration is $0.6\;M$, initial concentration of ${\rm{S}}{{\rm{O}}_3}$ is $1M$. The equilibrium constant is :

NEET UG CHEMISTRY MCQ: Equilibrium

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Application +4 | -1

At constant temperature in one litre vessel, when the reaction,

2\mathrm{S}{\mathrm{O}_3}\left( \mathrm{g} \right)\;\leftrightharpoons\;2\mathrm{S}{\mathrm{O}_2}\left( \mathrm{g} \right) + {\mathrm{O}_2}\left( \mathrm{g} \right)

is at equilibrium, the

\mathrm{S}{\mathrm{O}_2}

concentration is

0.6\;M

, initial concentration of

\mathrm{S}{\mathrm{O}_3}

1M

. The equilibrium constant is :

View answer and explanation

Correct option: D

0.675

Option D is correct because it accurately calculates the equilibrium constant based on the given concentrations and stoichiometry of the reaction.

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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}