The heats of combustion of carbon, hydrogen and acetylene are $- 394 k J, - 286 k J$ and $- 1301$ kJ respectively. Calculate heat of formation of $C_{2} H_{2}$ ?

621

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454

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- 227 k J

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227

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Solution

The correct option is D $227$ kJ
Solution:- (D) $227 k J$
Given:-
$C + O_{2} ⟶ C O_{2} Δ H = - 394 k J$
$2 \times [C + O_{2} ⟶ C O_{2} Δ H = - 394 k J]$
$2 C + 2 O_{2} ⟶ 2 C O_{2} Δ H = - 788 . . . . . (1)$
$H_{2} + \frac{1}{2} O_{2} ⟶ H_{2} O Δ H = - 286 k J . . . . . (2)$
$C_{2} H_{2} + \frac{5}{2} O_{2} ⟶ 2 C O_{2} + H_{2} O Δ H = - 1301 k J$
$2 C O_{2} + H_{2} O ⟶ C_{2} H_{2} + \frac{5}{2} O_{2} Δ H = 1301 k J . . . . . (3)$
Adding ${e q}^{n} (1), (2) & (3)$ , we have
$2 C + H_{2} ⟶ C_{2} H_{2} Δ H = 227 k J$
Hence the heat of formation of $C_{2} H_{2}$ is $227 k J$ .

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The heats of combustion of carbon, hydrogen and acetylene are −394kJ,−286kJ and −1301kJ respectively. Calculate heat of formation of C2H2?

The heats of combustion of carbon, hydrogen and acetylene are $- 394 k J, - 286 k J$ and $- 1301$ kJ respectively. Calculate heat of formation of $C_{2} H_{2}$ ?