An ideal diatomic gas initially has a pressure of 2.00x105Pa, a volume of 4.00 M3, and a temperature of 27 C. It has an isochoric change in pressure to 6.00X105Pa. 1. What are the new volume and temperature? 2. How much work is done to the gas? 3. How much heat is added to the gas? 4. What is the change in the internal energy of the gas?

4.0 moles of krypton gas are in a 0.20m3 container. The pressure is 1.663 x 105 Pa.  a, What is the temperature (to the nearest K)? The volume contracts to 0.10m3. The pressure is held constant.  b, How much work was done by the gas during the volume contraction?  c, What is the temperature after the volume contraction (to the nearest K)?

1. Two moles of helium gas are placed in a cylindrical container with a piston. The gas is at room temperature 27 °C and under a pressure of 3.3.105 Pa. When the pressure from the outside is decreased, while keeping the temperature the same as the room temperature, the volume of the gas doubles. Use that the gas constant R = 8.31 J/(mol K). Think: What kind of process is this? Isobaric, isothermal, adiabatic, isochoric or non-quasi-static? (a) Find the work the external agent does on the gas in the process. W = ext. agent (b) Find the heat exchanged by the gas and indicate whether the gas takes in or gives up heat. Assume ideal gas behavior. Q= ✓J Q is realeased by gas Q is absorbed by the gas

2. Sketch a PV diagram and find the work done by the gas during the following stages. (a) A gas is expanded from a volume of 1.0 L to 3.0 L at a constant pressure of 3.0 atm. (b) The gas is then cooled at constant volume until the pressure falls to 2.0 atm. (c) The gas is then compressed at a constant pressure of 2.0 atm from a volume of 3.0 L to 1.0 L. Note: Be careful of signs. (d) The gas is heated until its pressure increases from 2.0 atm to 3.0 atm at a constant volume. (e) Find the net work done during the complete cycle.