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In a constant volume calorimeter, 3.5 g of gas with molar mass $28 g m o l^{- 1}$ was burn 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 $2.5 k J K^{- 1}$ , the numerical value for the enthalpy of combustion of the gas in $k J m o l^{- 1}$ is:

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answer is 9.

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Detailed Solution

Total energy released during combustion of 3.5 g gas = (mS) x ∆T = 2.5 x 0.45 = 1.125 kJ
$∴$ Heat released by 1 mole of gas combustion.
$= \frac{28}{3.5} \times 1.125$ (molar mass of gas = 28)
$= 9 k J m o l^{- 1}$

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