How much heat energy in joules must be supplied to $14 g$ of nitrogen at room temperature to raise its temperature by $40^{o} C$ at constant pressure? (Mol. wt of $N_{2} = 28 g m, R =$ constant)

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Solution

The correct answer is option(C).
Mass of nitrogen, $m = 14 g$
Rise in temperature, $Δ T = 40 ° C$
Molecular weight of nitrogen $M = 28$
Number of moles, $n = \frac{m}{M} = \frac{14}{28} = 0.5$
Molar specific heat at constant pressure for nitrogen, $C_{P} = \frac{7}{2} R$
The total amount of heat to be supplied is given by the relation:
$Δ Q = n C_{P} Δ T = 0.5 \times \frac{7}{2} R \times 40 = 70 R J$
is the amount of heat to be supplied.

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