Starting with 2.5 mol of N2 gas (assumed to be ideal) in a cylinder at 1.00 atm and 20 degrees Celcius, a chemist first heats the gas at constant volume, adding 1.36x10^4 J of heat, then continues heating and allows the gas to expand at constant pressure to twice its original volume. Calculate (a) the final temperature of the gas; (b) the amount of work done by the gas: (c) the amount of heat added to the gas while it was expanding; (d) the change in internal energy of the gas for the whole process

Boiling Point Elevation/Freezing Point DepressionT = m KWhere: T = T(solution) - T(pure solvent) * m = (# moles solute / Kg solvent) Kb = boiling point elevation constant. Kf = freezing point depression constant. Kb and Kf depend only on the SOLVENT. Below are some common values. Use these values for the calculations that follow. Solvent Formula Kb (°C / m) Kf (°C / m) Water H2O 0.512 -1.86 Ethanol CH3CH2OH 1.22 -1.99 Chloroform CHCl3 3.67   Benzene C6H6 2.53 -5.12 Diethyl ether CH3CH2OCH2CH3 2.02   *Please note that ΔT as defined above will be a negative number for freezing point depression. Therefore, Kf must also be given as a negative number.

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

Calculate the pressure(in atm) of the saturated liquid at 71 °C.