A) \[+3.51\times {{10}^{5}}kJ\]
B) \[+7.38\times {{10}^{5}}kJ\]
C) \[+5.25\times {{10}^{3}}kJ\]
D) \[+1.65\times {{10}^{4}}kJ\]
Correct Answer: D
Solution :
Combustion of sucrose takes place as \[\underset{sucrose}{\mathop{{{C}_{12}}{{H}_{22}}{{O}_{11}}(s)}}\,+{{120}_{2}}(g)\xrightarrow{{}}12C{{O}_{2}}(g)\] \[+11{{H}_{2}}O(l)\] Molecular weight of sucrose \[=12\times 12+22\times 1+11\times 16\] = 144 + 22 + 176 = 342g \[\Delta H=-5.65\times {{10}^{3}}\,kJ\] \[\because \] 342 g of sucrose on complete combustion gives out heat \[=5.65\times {{10}^{3}}\,kJ\] \[\therefore \] 1000 g of sucrose of complete combustion will give out heat \[=\frac{5.65\times {{10}^{3}}}{342}\times 1000\] \[=1.6\times {{10}^{4}}kJ\]
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