When 3.00 moles of O2(g) is heated at a constant pressure of 3.25
atm, its temperature increases from 260K to 285K. given that the
molar heat capacity of oxygen at constant pressure is 29.4
J/K·mol, calculate Q and ∆U
To calculate Q, we can use the equation Q = nCpΔT, where Q is the heat transferred, n is the number of moles of the gas, Cp is the molar heat capacity at constant pressure, and ΔT is the change in temperature.
Q = (3.00 mol)(29.4 J/K·mol)(285 K - 260 K) = 3.00 mol * 29.4 J/K·mol * 25 K = 22,050 J
To calculate ΔU (the change in internal energy), we can use the equation ΔU = Q - W, where W is the work done by or on the gas. Since the problem states that the pressure is constant, the work done is zero. Therefore, ΔU = Q.
ΔU = 22,050 J