A) \[1.65\times {{10}^{4}}\text{ }kJ\]
B) \[5.25\times {{10}^{3}}\text{ }kJ\]
C) \[7.38\times {{10}^{5}}\text{ }kJ\]
D) \[3.51\times {{10}^{5}}\text{ }kJ\]
Correct Answer: A
Solution :
Molecular weight of \[{{C}_{12}}{{H}_{22}}{{O}_{11}}\] \[=12\times 12+22+11\times 16\] \[=144+22+176=342\] \[\because \] heat evolved on combustion of 342 g sucrose \[=5.65\times {{10}^{3}}\text{ }kJ\] \[\therefore \] heat evolved on combustion of 1000 g sucrose \[=\frac{5.65\times {{10}^{3}}}{342}\times 1000=16.52\times {{10}^{3}}\,kJ\]
You need to login to perform this action.
You will be redirected in
3 sec
