The molar specific heat of a diatomic ideal gas at constant volume is Cv = 5/2 R. What is the heat needed to heat 28.00 g of nitrogen gas from 20.00 °C to 85.00 °C?

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The molar specific heat of a diatomic ideal gas at constant volume is Cv = 5/2 R. The heat needed to heat a gas is given by Q = nCvΔT, where n is the number of moles of gas, Cv is the molar specific heat, and ΔT is the change in temperature. The number of moles of gas is given by n = m/M, where m is the mass of gas and M is the molar mass. The molar mass of nitrogen gas is 28.02 g/mol. So, the number of moles of gas is n = 28.00 g / 28.02 g/mol = 1.000 mol. The change in temperature is ΔT = 85.00 °C - 20.00 °C = 65.00 °C. So, the heat needed to heat the gas is Q = nCvΔT = (1.000 mol)(5/2 R)(65.00 °C) = 1,350 J.

The Molar Specific Heat of a Diatomic Ideal Gas at Constant