A quantity of gas occupies an initial volume `V_(0)` at pressure `p_(0)` and temperature `T_(0)`. It expands to a volume V (a) constant temperature and (b) constant pressure. In which case does the gas do more work ?

One mole of an ideal gas at pressure P_(0) and temperature T_(0) is expanded isothermally to twice ist volume and then compressed at constant pressure to (V_(0) // 2) and the gas is brought bac to original state by a process in which P alpha V (pressure is direclty proportional to volume). The correct temperature of the process is

Three moles of an ideal gas (C_p=7/2R) at pressure p_0 and temperature T_0 is isothermally expanded to twice its initial volume. It is then compressed at a constant pressure to its original volume. (a) Sketch p-V and p-T diagram for complete process. (b) Calculate net work done by the gas. (c) Calculate net heat supplied to the gas during complete process. (Write your answer in terms of gas constant =R)

A sample of an ideal gas has pressure p_(0) , volume V_(0) and tempreture T_(0) . It is isothermally expanded to twice its oringinal volume.it is then compressed at constant pressure to have the original volume V_(0) . Finally, the gas is heated at constant volume to get the original tempreture.(a) show the process in a V-T diagram (b) calculate the heat absorbed in the process.

A gas has a volume of 6.0L at a pressure of 0.80 atm. What is the volume if the pressure is changed to 0.20atm at constant temperature?

An ideal gas is found to obey an additional laq P^(2) V = constant. The gas is initially at temperature volume V . When it expands to a volume 2V , the temperature becomes-

A gas is found to obey the law P^(2)V = constant . The initial temperature and volume are T_(0) and V_(0) . If the gas expands to a volume 3 V_(0) , its final temperature becomes