| \[2NO(g)+{{O}_{2}}(g)\xrightarrow[{}]{}2N{{O}_{2}}(g)\,;\] \[\Delta {{H}^{o}}=-114\,kJ/mole\] |
| \[4N{{O}_{2}}(g)+{{O}_{2}}(g)\xrightarrow[{}]{{}}2{{N}_{2}}{{O}_{2}}(g)\,;\] \[\Delta {{H}^{o}}=-102.6\,kJ/mole\] |
A) \[15.1\]
B) \[30.2\]
C) \[-36.2\]
D) \[-46.8\]
Correct Answer: A
Solution :
\[{{N}_{2}}(g)+\frac{5}{2}{{O}_{2}}(g)\xrightarrow{{}}{{N}_{2}}{{O}_{5}};\,\,\Delta {{H}_{f({{N}_{2}}{{O}_{5}})}}=5\] \[2NO(g)+{{O}_{2}}(g)\xrightarrow{{}}2N{{O}_{2}}(g);\] \[\Delta H_{f}^{o}=114\,\,kJ/mole\] ?(1) \[4NO(g)+{{O}_{2}}(g)\xrightarrow{{}}2{{N}_{2}}{{O}_{5}}(g);\]\[\Delta H_{f}^{o}=102.6kJ/mole\] ?(2) \[\frac{1}{2}N{{O}_{2}}(g)+\frac{1}{2}{{O}_{2}}(g)\xrightarrow{{}}NO(g);\] \[\Delta H_{f}^{o}=+90.2\,\,kJ/mole\] ?(3) \[\frac{1}{2}\times Eq(2)+2\times Eq(3)+Eq(1)\] \[2NO+{{O}_{2}}\xrightarrow{{}}2N{{O}_{2}};\,\,\Delta {{H}_{f}}=-114\] \[2N{{O}_{2}}+\frac{1}{2}{{O}_{2}}\xrightarrow{{}}{{N}_{2}}{{O}_{5}};\] \[\Delta {{H}_{2}}=-\frac{102.6}{2}=-51.3\] \[\frac{{{N}_{2}}+{{O}_{2}}\xrightarrow{{}}2NO;\,\,\Delta {{H}_{3}}=90.2\times 2=180.4}{{{N}_{2}}+\frac{5}{2}{{O}_{2}}\xrightarrow{{}}{{N}_{2}}{{O}_{5}};\,\,\Delta H=15.1\,\,kJ/mole}\]
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