What amount of heat must be supplied to 2.0 × 10–2 kg of nitrogen (at room temperature) to raise its temperature by 45 °C at constant pressure? (Molecular mass of N2 = 28; R = 8.3 J mol–1 K–1.)

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Mass of nitrogen, m = 2.0 × 10–2 kg = 20 g Rise in temperature, ΔT = 45°C Molecular mass of N2, M = 28 Universal gas constant, R = 8.3 J mol–1 K–1 Number of moles, Molar specific heat at constant pressure for nitrogen, The total amount of heat to be supplied is given...
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Mass of nitrogen, m = 2.0 × 10–2 kg = 20 g Rise in temperature, ΔT = 45°C Molecular mass of N2, M = 28 Universal gas constant, R = 8.3 J mol–1 K–1 Number of moles, Molar specific heat at constant pressure for nitrogen, The total amount of heat to be supplied is given by the relation: ΔQ = nCP ΔT = 0.714 × 29.05 × 45 = 933.38 J Therefore, the amount of heat to be supplied is 933.38 J. read less
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