A) 1412 kJ
B) 9884 kJ
C) 353 kJ
D) 706 kJ
Correct Answer: C
Solution :
\[{{C}_{2}}{{H}_{4}}(g)+3{{O}_{2}}(g)\xrightarrow{{}}2C{{O}_{2}}(g)+2{{H}_{2}}O(l);\] \[\Delta H=?\] \[\Delta H=\sum{\Delta {{\Eta }_{f}}}\]product \[-\sum{\Delta {{\Eta }_{f}}}\]reactant \[=[2(-394)+2(-286)]=[(52+0)]\] \[=[2(-394)+2(-286)]-[(52+0)]\] \[=[-788-572]-[52]\] \[=-1412\,\text{kJ}\,\text{mo}{{\text{l}}^{-1}}\] \[\because \]Amount of heat evolved by burning 28 g of\[{{C}_{2}}{{H}_{4}}=1412\,kJ\] \[\therefore \]Amount of heat evolved by burning 7 g of \[{{C}_{2}}{{H}_{4}}=\frac{1412}{28}\times 7=353\,kJ\]You need to login to perform this action.
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