The calorific value of methane in the following reaction is about-
$2 C H_{4} + 4 O_{2} \to 2 C O_{2} + 4 H_{2} O + 1780 k J$

$55 k J / g$

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$110 k J / g$

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$110 J / g$

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$55 J / g$

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Solution

The correct option is A
$55 k J / g$

Option (A)
Calorific value means heat energy produced by specific amount of fuel or food.
$2 C H_{4} + 4 O_{2} \to 2 C O_{2} + 4 H_{2} O + 1780 k J$ is the given reaction
We know that molar mass of methane is $16.04 g / m o l$
Therefore, $2 C H_{4} = 32 g$ .
$32 g$ of $C H_{4}$ is producing $= 1780 k J$
$1 g$ of $C H_{4}$ is producing $= \frac{1780}{32} = 55.625 \approx 55 k J / g$ .
Hence, option (A) is the correct option.

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The calorific value of methane in the following reaction is about-2CH4+4O2→2CO2+4H2O+1780kJ

The calorific value of methane in the following reaction is about-
$2 C H_{4} + 4 O_{2} \to 2 C O_{2} + 4 H_{2} O + 1780 k J$