In the combustion of $2 g$ of methane, $25 k c a l$ heat is liberated. Find the molar heat of combustion of methane.

100 k c a l

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200 k c a l

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75 k c a l

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150 k c a l

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Solution

The correct option is B $200 k c a l$
Reaction: $C H_{4} + 2 O_{2} \to C O_{2} + 2 H_{2} O$
Molar mass of $C H_{4} = 16 g$
We know, molar heat of combustion is the heat released when 1 mole of a substance is completely burned.
So, heat evolved by combustion of 2 g of $C H_{4} = 25 k c a l$
Heat evolved by $16 g$ of $C H_{4}$ = $\frac{25 \times 16}{2} = 200 k c a l$

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