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What amount of energy (KJ) is released in the combustion of 5.8 gr of $C_{4} H_{10} (g)$
$2 C_{4} H_{10} (g) + 13 O_{2} (g) \to 8 {CO}_{2} (g) + 10 H_{2} O (ℓ) ΔH = - 5756 KJ$

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575.6

287.8

182

57.56

answer is B.

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Detailed Solution

$2 \times 58 gr$ of $C_{4} H_{10} \to - 5756 KJ$
$5 .8 gr of C_{4} H_{10} \to ?$
$\Rightarrow 287 .8 KJ$

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