A) - 17 kcal
B) - 111 kcal
C) - 170 kcal
D) - 85 kcal
Correct Answer: A
Solution :
For reaction, |
\[C(s)+2{{H}_{2}}(g)\xrightarrow[{}]{{}}C{{H}_{4}}(g),\,\Delta {{H}^{o}}=\,?\] |
\[\Delta {{H}^{o}}=-\,[(\Delta {{H}^{o}}\] of combustion of \[C+2\times \Delta H\] of combustion of \[{{H}_{2}})]\] |
\[C+{{O}_{2}}\xrightarrow{{}}C{{O}_{2}};\,\,\,\Delta H=-94\,\,kcal\] ...(i) |
\[2{{H}_{2}}+{{O}_{2}}\to 2{{H}_{2}}O;\Delta H=-68\times 2\,kcal\] (ii) |
\[C{{H}_{4}}+2{{O}_{2}}\to C{{O}_{2}}+2{{H}_{2}}O;\,\,\Delta H=-213\,kcal\] (iii) |
\[=-[(-213)-(-94+2\times -68)]\,kcal/mol\] |
\[=-[-213+230]=-17\,\,kcal/mol\] |
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