The amount of heat must be supplied to 2.0×10–2kg of nitrogen (at room temperature) to rise its temperature by 450C at constant pressure is (Molecular mass of N2 = 28; R = 8.3J mol–1K–1)

A
933 J
B
1037 J
C
1868 J
D
467 J

Solution:

$\begin{array}{l} m = 2 .0 \times 10^{- 2} kg; N_{2} \to gas; dT = 45^{\circ} C \\ 7 {rNN}_{2}, M = 28 gm = 28 \times 10^{- 3} kg, Cp = \frac{7}{2} R \\ R = 8 .3 J / mole - K \\ C_{P} = \frac{1}{n} \times \frac{(dQ)_{P}}{dT} = \frac{7}{2} R \\ (dQ)_{P} = \frac{2 \times 10^{- 2} \times 1 .4 \times 8 .3}{28 \times 10^{- 3} \times 0 .4} \times 45 = 945 J \end{array}$

The amount of heat must be supplied to 2.0×10^–2kg of nitrogen (at room temperature) to rise its temperature by 45⁰C at constant pressure is (Molecular mass of N₂ = 28; R = 8.3J mol^–1K^–1)

Solution:

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