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Question: The expression for equilibrium constant, \(\mathrm { K } _ { \mathrm { c } }\) for the following r...

The expression for equilibrium constant, Kc\mathrm { K } _ { \mathrm { c } } for the following reaction is.

2Cu(NO3)2( s)2 \mathrm { Cu } \left( \mathrm { NO } _ { 3 } \right) _ { 2 ( \mathrm {~s} ) } 2CuO(s)+4NO2( g)+O2( g)2 \mathrm { CuO } _ { ( \mathrm { s } ) } + 4 \mathrm { NO } _ { 2 ( \mathrm {~g} ) } + \mathrm { O } _ { 2 ( \mathrm {~g} ) }

A

Kc=[CuO(s)]2[NO2( g]4[O2( g)][Cu(NO3)2( s)]2\mathrm { K } _ { \mathrm { c } } = \frac { \left[ \mathrm { CuO } _ { ( \mathrm { s } ) } \right] ^ { 2 } \left[ \mathrm { NO } _ { 2 ( \mathrm {~g} } \right] ^ { 4 } \left[ \mathrm { O } _ { 2 ( \mathrm {~g} ) } \right] } { \left[ \mathrm { Cu } \left( \mathrm { NO } _ { 3 } \right) _ { 2 ( \mathrm {~s} ) } \right] ^ { 2 } }

B

C

Kc=[NO2( g)]4[O2( g)]\mathrm { K } _ { \mathrm { c } } = \left[ \mathrm { NO } _ { 2 ( \mathrm {~g} ) } \right] ^ { 4 } \left[ \mathrm { O } _ { 2 ( \mathrm {~g} ) } \right]

D

Answer

Kc=[NO2( g)]4[O2( g)]\mathrm { K } _ { \mathrm { c } } = \left[ \mathrm { NO } _ { 2 ( \mathrm {~g} ) } \right] ^ { 4 } \left[ \mathrm { O } _ { 2 ( \mathrm {~g} ) } \right]

Explanation

Solution

: 2CuO(s)+4NO2( g)+O2( g)2 \mathrm { CuO } _ { ( \mathrm { s } ) } + 4 \mathrm { NO } _ { 2 ( \mathrm {~g} ) } + \mathrm { O } _ { 2 ( \mathrm {~g} ) }

Since conc. Of solids is taken as 1, the expression for becomes

Kc=[NO2( g)]4[O2( g)]\mathrm { K } _ { \mathrm { c } } = \left[ \mathrm { NO } _ { 2 ( \mathrm {~g} ) } \right] ^ { 4 } \left[ \mathrm { O } _ { 2 ( \mathrm {~g} ) } \right]