Two identical containers each hold 1 mole of an ideal gas at 1 atm. Container A holds a monatomic gas and container B holds a diatomic gas. The gas in each container is compressed at constant pressure to half its original volume. (a) What is the ratio WA/WB of the work done on gas A to the work done on gas B? (b) What is the ratio ∆UA/∆UB of the change in internal energy for gases A and B? (c) What is the ratio QA/QB of the energy transferred to gases A and B ?

An ideal gas in a container with a sliding piston is held at atmospheric pressure. Heat is added and the volume increases from 1 m^3 to 3 m^3. The initial temp of the gas is 0 degrees celcius.  Question A: How many moles of gas are in this container?  Question B: How much work does the gas perform on the piston? Please answer in J Question C: What is the final temperature of the gas? Please answer in degrees celcius Question D: what is the change in internal energy of the gas? Please answer in J  Question E: How much heat was added to the gas? Please answer in J

Suppose 1.70 mol of oxygen is heated at a constant pressure of 1.00 atm from 10.0°C to 23.0°C.     What is the magnitude of the work done by the gas during this expansion?   The magnitude of the work done by the gas is  J.

The volume of an ideal gas is increased from 1 m3 to 3 m3 at a constant pressure of 1000 Pa          How much work is done by the gas in the expansion?                          W= _________ J          If no heat has been added or removed, what is the change in internal energy of the gas?           DU = ________ J