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Question: 1 mole of NO and 1 mole of \(\mathrm { O } _ { 3 }\) are taken in a 10 L vessel and heated. At equi...

1 mole of NO and 1 mole of O3\mathrm { O } _ { 3 } are taken in a 10 L vessel and heated. At equilibrium, 50% of NO (by mass) reacts with O3\mathrm { O } _ { 3 }according to the equation:

NO(g)+O3( g)\mathrm { NO } _ { ( \mathrm { g } ) } + \mathrm { O } _ { 3 ( \mathrm {~g} ) } NO2( g)+O2( g)\mathrm { NO } _ { 2 ( \mathrm {~g} ) } + \mathrm { O } _ { 2 ( \mathrm {~g} ) }

What will be the equilibrium constant ofr this reaction?

A

1

B

2

C

3

D

4

Answer

1

Explanation

Solution

:

NO(g)\mathrm { NO } _ { ( \mathrm { g } ) } + O3( g)\mathrm { O } _ { 3 ( \mathrm {~g} ) } NO2( g)\mathrm { NO } _ { 2 ( \mathrm {~g} ) } + O2( g)\mathrm { O } _ { 2 ( \mathrm {~g} ) }
Initial conc.1100
At equilibrium0.50.50.50.50.50.50.50.5
Conc.0.510\frac { 0.5 } { 10 }0.510\frac { 0.5 } { 10 }0.510\frac { 0.5 } { 10 }0.510\frac { 0.5 } { 10 }