| \[{{N}_{2}}+3{{H}_{3}}\overset{{}}{leftrightarrows}2{{N}_{3}};{{K}_{1}}\] |
| \[{{N}_{2}}+{{O}_{2}}\overset{{}}{leftrightarrows}2NO;{{K}_{2}}\] |
| \[{{H}_{2}}+\frac{1}{2}{{O}_{2}}\overset{{}}{leftrightarrows}{{H}_{2}}O;{{K}_{3}}\] |
| The equilibrium constant for the oxidation of \[N{{H}_{3}}\]by oxygen to give NO is: |
A) \[{{K}_{1}}\times {{K}_{2}}/{{K}_{3}}\]
B) \[{{K}_{2}}\times \,K_{3}^{3}/{{K}_{1}}\]
C) \[{{K}_{2}}\times \,K_{3}^{2}/{{K}_{1}}\]
D) \[K_{2}^{2}\,{{K}_{3}}/{{K}_{1}}\]
Correct Answer: B
Solution :
[b] \[{{K}_{2}}\,K_{3}^{3}/{{K}_{1}}\] \[Aim:2N{{H}_{3}}+\frac{5}{2}{{O}_{2}}\overset{{}}{leftrightarrows}2NO+3{{H}_{2}}O\] \[K=\frac{{{[NO]}^{2}}{{[{{H}_{2}}O]}^{3}}}{[N{{H}_{3}}]{{[{{O}_{2}}]}^{1/2}}}\] \[{{K}_{1}}=\frac{{{[N{{H}_{3}}]}^{2}}}{[{{N}_{2}}]{{[{{H}_{2}}]}^{3}}}\] \[{{K}_{2}}=\frac{{{[NO]}^{2}}}{[{{N}_{2}}][{{O}_{2}}]}\] \[{{K}_{3}}=\frac{[{{H}_{2}}O]}{[{{H}_{2}}]{{[{{O}_{2}}]}^{1/2}}}\] \[Hence,\,\,K=\frac{{{K}_{2}}K_{3}^{3}}{{{K}_{1}}}\]
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