Answer:
Information shadow:
The reaction is:
\[2S{{O}_{2}}(g)+{{O}_{2}}(g)\rightleftharpoons 2S{{O}_{3}}(g)\]
The equilibrium
concentrations are:
\[[S{{O}_{2}}]=0.6M;\,\,[{{O}_{2}}]=0.82M;\,\,\,\,[S{{O}_{3}}]=1.90M\]
Problem
solving strategy:
The
expression for equilibrium constant is:
\[{{K}_{c}}\frac{{{[S{{O}_{3}}]}^{2}}}{{{[S{{O}_{2}}]}^{2}}[{{O}_{2}}]}\,\,\,\,\,\,\,\,\,\,\,\,......(i)\]
Working
it out:
Substituting
the values in equation (i) we get,
\[{{K}_{c}}=\frac{{{(1.90)}^{2}}}{{{(0.6)}^{2}}\times
(0.82)}\]
\[=12.228mo{{l}^{-1}}L\]
You need to login to perform this action.
You will be redirected in
3 sec