Final answer:
The heat capacity, work, change in internal energy, and change in enthalpy for an ideal gas at constant pressure are calculated using the gas's heat capacity expression, thermodynamic equations, and the first law of thermodynamics.
Step-by-step explanation:
The calculation of heat (q), work (w), change in internal energy (ΔU), and change in enthalpy (ΔH) for an ideal gas under constant pressure involves using thermodynamic equations. The expression for the constant pressure heat capacity (Cp) of a gas is used to find q through the equation q = nCpΔT, where ΔT is the change in temperature and n is the number of moles of gas. The amount of work done by an ideal gas during expansion or compression at constant pressure is given by w = -PΔV. The change in internal energy, ΔU, can be calculated using the first law of thermodynamics as ΔU = q - w, and the change in enthalpy, ΔH, for an ideal gas is given by ΔH = nCpΔT, since ΔH = ΔU + PΔV and under constant pressure, PΔV is nRΔT, which is equivalent to nCpΔT considering that Cp = Cv + R.