0.1 mole of ${{\rm{N}}_2}{{\rm{O}}_4}\left( {\rm{g}} \right)$ was sealed in a tube under one atmospheric conditions at $25^\circ C$. Calculate the number of moles of ${\rm{N}}{{\rm{O}}_2}\left( {\rm{g}} \right)$ present, if the equilibrium ${{\rm{N}}_2}{{\rm{O}}_4}\left( {\rm{g}} \right)\;\leftrightharpoons\;2{\rm{N}}{{\rm{O}}_2}\left( {\rm{g}} \right)\left( {{K_p} = 0.14} \right)$ is reached after some times

NEET UG CHEMISTRY MCQ: Equilibrium

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Application +4 | -1

0.1 mole of

{\mathrm{N}_2}{\mathrm{O}_4}\left( \mathrm{g} \right)

was sealed in a tube under one atmospheric conditions at

25^\circ C

. Calculate the number of moles of

\mathrm{N}{\mathrm{O}_2}\left( \mathrm{g} \right)

present, if the equilibrium

{\mathrm{N}_2}{\mathrm{O}_4}\left( \mathrm{g} \right)\;\leftrightharpoons\;2\mathrm{N}{\mathrm{O}_2}\left( \mathrm{g} \right)\left( {{K_p} = 0.14} \right)

is reached after some times

View answer and explanation

Correct option: A

0.036

Option A is correct because it calculates the number of moles of NO2 at equilibrium using the given Kp value and initial conditions.

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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}