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 air from 20.00$^{\circ}$C to 85.00$^{\circ}$C?

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Quizplus · Accepted Answer

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 at constant volume, 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 of gas. The molar mass of air is 28.97 g/mol. So, the number of moles of gas is n = 28.00 g / 28.97 g/mol = 0.966 mol. The change in temperature is ΔT = 85.00^$\circ$C - 20.00^$\circ$C = 65.00^$\circ$C. So, the heat needed to heat the gas is Q = nCvΔT = (0.966 mol) * (5/2 R) * (65.00^$\circ$C) = 1,350 J.

The Molar Specific Heat of a Diatomic Ideal Gas at Constant