Ncert Exercises & Solutions

12.2 What amount of heat must be supplied to 2.0 × 10 $^{- 2}$ kg of nitrogen (at room temperature) to raise its temperature by 4°C at constant pressure? (Molecular mass of $N_{2}$ = 28; R = 8.3 J ${mol}^{- 1} K^{- 1}$ )

Number of moles, $n = \frac{m}{M}$ = $\frac{2 \times 10^{- 2} \times 10^{3}}{28}$ = 0.714

Nitrogen is a diatomic gas, so molar specific heat at constant pressure for nitrogen, $C_{P} = \frac{7}{2} R$

$= \frac{7}{2} \times 8.3$

= 29.05 J mol^-1 K^-1

The total amount of heat to be supplied is given by:

ΔQ = ${nC}_{P} ΔT$ = 0.714 × 29.05 × 45 = 933.38 J

Therefore, the amount of heat to be supplied is 933.38 J.

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