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Heat of Formation

The standard ...

Question

The standard heat of formation of $C H_{4 (g)}, C O_{2 (g)}$ and $H_{2} O_{(g)}$ are $- 76.2, - 398.8, - 241.6$ $k J m o l^{- 1}$ respectively. the amount of heat evolved $(i n k J)$ by burning 1 $m^{3}$ of methane measured under normal conditions is

A

805

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B

35973

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C

22.4

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D

3121

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Solution

The correct option is B 35973
The combustion reaction for methane is
$C H_{4 (g)} + 2 O_{2 (g)} \to C O_{2 (g)} + 2 H_{2} O_{(g)}; △ H = ? △ H^{\circ} = △ H_{f (p r o d u c t s)}^{\circ} - △ H_{f (r e c t a n t s)}^{\circ} = △ H_{f (C O_{2})}^{\circ} + 2 \times △ H_{f (H_{2} O)}^{\circ} - △ H_{f (C H_{4})}^{\circ} - 2 △ H_{f (O_{2})}^{\circ} = - 398.8 - 2 \times 241.6 - (- 76.2) - 2 \times 0 = - 805.8 k J m o l^{- 1}$
Heat evolved by burning 22.4 litre (1 mole) methane
= $805.8 k J$
So, heat evolved by burning 1000 Litre $(1 m^{3})$ methane
$= \frac{1000}{22.4} \times 805.8 = 35973.2 k J$

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Standard XIII Chemistry

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