In a constant volume calorimeter, 3.5 g of a gas with molecular weight 28 was burnt in excess oxygen at 298.0 K . The temperature of the calorimeter was found to increase from 298.0 K to 298.45 K due to the combustion process. Given that the heat capacity of the calorimeter is $2.5 \mathrm{~kJ} \mathrm{~K}^{-1}$, the numerical value for the enthalpy of combustion of the gas in $\mathrm{kJmol}^{-1}$ is
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Solution
Energy release at constant volume due to combustion of 3.5 gm of a gas $=2.5 \times 0.45$
Hence energy released due to the combustion of 28 gm (i.e., 1 mole) of a gas $=2.5 \times 0.45 \times \frac{28}{3.5}=9 \mathrm{kJmol}^{-1}$
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