A) 135.6
B) \[-135.6\]
C) 125.6
D) \[-125.6\]
Correct Answer: B
Solution :
Given, (i)\[{{C}_{2}}{{H}_{4}}(g)+3{{O}_{2}}(g)\xrightarrow[{}]{{}}2C{{O}_{2}}(g)+2{{H}_{2}}O(l)\] \[\Delta H=-1410\text{ }kJ\text{ }mo{{l}^{-1}}\] (ii) \[{{H}_{2}}(g)+\frac{1}{2}{{O}_{2}}(g)\xrightarrow[{}]{{}}{{H}_{2}}O(l);\] \[\Delta H=-286.\text{ }2\text{ }kJ\text{ }mo{{l}^{-1}}\] (iii) \[{{C}_{2}}{{H}_{6}}(g)+3\frac{1}{2}{{O}_{2}}(g)\to 2C{{O}_{2}}(g)+3{{H}_{2}}O(l)\] \[\Delta H=-1560.\text{ }6\text{ }kJ\text{ }mo{{l}^{-1}}\] Required reaction is \[{{C}_{2}}{{H}_{4}}+{{H}_{2}}(g)\xrightarrow[{}]{{}}{{C}_{6}}{{H}_{6}}(g),\]\[\Delta H=?\] Equation (i) + Equation (ii) - Equation (iii) gives \[{{C}_{2}}{{H}_{4}}+{{H}_{2}}(g)\xrightarrow[{}]{{}}{{C}_{2}}{{H}_{6}}(g),\] \[\Delta H=-1410.\text{ }0+(-286.\text{ }2)-(-1560.6)\] \[=-135.6\text{ }kJ\text{ }mo{{l}^{-1}}\]
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