Vapor pressure data are given here for octane, C8H18. Temperature(c) Vapor Pressure (mm Hg) 25 13.6 50 45.3 75 127.2 100 310.8 Use the Clausius–Clapeyron equation to calculate the molar enthalpy of vaporization of octane and its normal boiling point

please label when values are from steam table

For a van der Waals gas: (∂Um∂V)=aV2m In this problem, you will compare the change in energy with temperature and volume for N2, treating it as a van der Waals gas. 1) Calculate ΔU per mole of N2(g) at 1 bar pressure and 298 K if the volume is increased by 7.00 % at constant T. Approximate the molar volume with the ideal gas value. a(N2)=1.370dm6⋅bar⋅mol−2 .Express your answer with the appropriate units. 2) Calculate ΔU per mole of N2(g) at 1 bar pressure and 298 K if the temperature is increased by 7.00 % at constant V. CP,m for N2(g) at 298 K is 29.13 J⋅K−1⋅mol−1 .Express your answer with the appropriate units.