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How much heat energy must be supplied to 14 g of nitrogen gas at room temperature to raise its temperature by $40^{\circ} C$ at a constant pressure?

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Solution

14 g of $N_{2} = \frac{14}{28} = \frac{1}{2} m o l e s o f N_{2}$
Given, $Δ T = 40^{\circ} C$
For a diatomic gas, $C_{p} = \frac{7 R}{2}$
Heat required, $Δ H = n C_{p} Δ T = n (\frac{7 R}{2}) Δ T = \frac{1}{2} (\frac{7}{2} \times 8.314) \times 40 = 581.98 J$

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