0.03 m3 of nitrogen contained in a cylinder behind apiston is initially at 1.05 bar and 15ºC. The gas iscompressed isothermally and reversibly until the pressureis 4.2 bar. Calculate the change of entropy, the heat flow,and the work done, and sketch the process on a p-v andT-s diagrams. Assume nitrogen to act as a perfect gas.Molecular weight of nitrogen = 28.

what table and column are you looking at to get 103 kj for the enthalpy , and how are you getting the 163 , for 1866-163?.

A 2.80-mol sample of helium gas initially at 300 K, and 0.400 atm is compressed isothermally to 1.40 atm. Note that the helium behaves as an ideal gas. (a) Find the final volume of the gas. m³ (b) Find the work done on the gas. kJ (c) Find the energy transferred by heat. kJ

The pressure change during a particular reversible process is given by T = AP2 where A is a constant. A monatomic ideal gas is taken through this process from a temperature of 4T0 to 16T0. The sample of gas consists of n moles. (Hint: You must express the pressure in terms of volume using the equation for the process and the ideal gas law.) Compute the work done by the gas in terms of n, R, and T0 (and appropriate numerical constants) only. Compute the change in heat for the gas in terms of n, R, and T0 (and appropriate numerical constants) only. Compute the change in entropy for the gas in terms of n, R, and T0 (and appropriate numerical constants) only.