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At constant temperature & volume, 50% of ozone is decomposed out of 2 atm of ozone taken initially and the equilibrium $\large 2{O_{3(g)}}\, \rightleftharpoons \,\,3{O_{2\left( g \right)}}$ is established, Kp for the decomposition of ozone is

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Detailed Solution

\large 2{O_3}\left( g \right) \rightleftharpoons 3{O_2}\left( g \right)

Initial pressure of O₃ = 2 atm

degree of decomposition =

Decrease in pressure due to decomposition of O₃ = 0.5 x 2

= 1 atm

2 moles of O₃ → 3 moles of O₂

1 moles of O₃ → 'x' moles of O2

Number of moles $α$

partial pressure

\large {K_P} = \frac{{P_{{O_2}}^3}}{{P_{{O_3}}^2}}

\large {K_P} = \frac{{{{\left( {1.5} \right)}^3}}}{{{{\left( 1 \right)}^2}}}

\large {K_P} = {\left( {\frac{3}{2}} \right)^3}

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