Consider a system that contains 3 moles of an ideal gas in a cylindrical syringe. Initially the temperature of the system is T1 = 500 K and the pressure is 1 atm. Now, the gas is slowly cooled (at a constant pressure of 1atm) until the gas reaches a temperature of T2 = 350 K. During this constant pressure process, the volume changes to a value V2 and the energy of the gaseous system changes from E1 to E2. a) Compute the change in energy (ΔE = E2 - E1) for this gas in units of kilojoules(kJ).

b) Find the change in volume (ΔV) for this gas in units of L.

c) Now find the work (w = -PΔV) of the system, in kilojoules (kJ). Is the gas doing work, or is work being done on the gas? Does the sign of w in your answer make sense to you?Note: 1 L-atm is equivalent to 101 J because 8.315 J / mole - K = 101 J /L-atm 0.0820 l - atm / mol - K

d) Using your answers in (a) and (c), and the First Law of Thermodynamics, compute the heat, in kilojoules, that must have been transferred between the gas and the surroundings in the process described. What is the direction of the heat transfer?