A) \[\text{16}\text{.25}\,\text{J}\]
B) \[\text{16}\text{.25}\,k\text{J}\]
C) \[32.5\,J\]
D) \[32.5\,kJ\]
Correct Answer: B
Solution :
The enthalpy of combustion of\[{{C}_{6}}{{H}_{6}}(l)=-3250\,kJ\] By burning 78 gm. of \[{{C}_{6}}{{H}_{6}}\]liberated heat \[=3250\text{ kJ}\] [Mol. wt. of benzene \[=12\times 6+1\times 6=78\,J\] On buring \[\text{0}\text{.39}\,\text{gm}\text{.}\] of \[{{\text{C}}_{\text{6}}}{{\text{H}}_{\text{6}}}\]liberated heat \[\text{=}\frac{0.39}{78}\] \[=3250\] \[=16.25\,kJ\]
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