For complete combustion of methanol $C H_{3} O H (l) + \frac{3}{2} O_{2} (g) \to C O_{2} (g) + 2 H_{2} O (l)$ The amount of heat produced as measured by bomb calorimeter is $726 k J m o l^{- 1}$ at $27 º C$ . The enthalpy of combustion at constant pressure for the reaction is $- x k J m o l^{- 1}$ , where $x$ is _______(nearest integer) (Given : $R = 8.3 J K^{- 1} m o l^{- 1}$ )

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727

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276

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answer is A.

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Detailed Solution

$C H_{3} O H_{(l)} + \frac{3}{2} O_{2 (g)} \to C O_{2} (g) + 2 H_{2} O (l)$

At $27^{0} C Δ n = 1 - 1.5 = - 0.5$

$Δ H = Δ U + Δ n R T$

$= - 726 + (- 0.5) (300) \times 8.3 \times 10^{- 3} = - 726 - 1.24$

$= - 727.24 k J$

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