Given: $C a O + C O_{2} \to$ $C a C O_{3} + 40 k c a l / m o l e .$ If $176 g$ of $C O_{2}$ are consumed, then how many $k c a l$ of heat are released?

80 k c a l

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100 k c a l

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120 k c a l

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160 k c a l

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Solution

The correct option is D $160 k c a l$
$C a O$ $+$ $C O_{2}$ $=$ $C a C O_{3}$ $+$ $40 k c a l / m o l e$
From $1$ mole of $C O_{2}$ , $40 k c a l$ of heat are released.
$1$ mole of $C O_{2}$ weighs $44$ grams.
Thus $44$ grams of $C O_{2}$ give $40 k c a l$ of heat
$1$ gram of $C O_{2}$ gives $\frac{40}{44}$ $k c a l$ of heat
Thus, $176$ gram of $C O_{2}$ give $\frac{40}{44}$ $\times$ $176$ , that is $160 k c a l$ of heat.
Option $E$ is the correct answer.

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