1. The problem statement, all variables and given/known data Argon is heated from T1 to T2. Assume ideal gas behaviour. Calculate the energy input. Assume a constant volume, mass and constant specific heat capacity. Pressure variable T1=523.15 K T2=823.15 K M= 0.03995 kg m=50 kg R=8.31 Cv=0.0125 kJ/(mol.K) 2. Relevant equations Enthalpy change in gas ΔH = ΔU + nRΔT ΔU=CvΔT n= m/M ΔH=CvΔT+ (m/M)RΔT 3. The attempt at a solution ΔH=((0.0125)*(300))+(50/0.03995)*( 8.31)*(300)…kj Is this equal to the heat energy input? Would this equal the amount of energy it would take to cool the gas, i.e. the reverse process?