The volume of 2 moles of a diatomic ideal gas at 300 K is doubled keeping its pressure constant. Find the change in the internal energy of the gas. Given R = 8.3 JK- mol.

A 2.00 mol sample of an ideal diatomic gas at a pressure of 1.10 atm and temperature of 420 K undergoes a process in which its pressure increases linearly with temperature. The final temperature and pressure are 720 K and 1.70 atm . Fid the change in internal energy, work done by the gas, and heat added.

Consider one mole of a simple ideal gas enclosed in a cylindrical piston with rigid impermeable adiabatic walls. The piston has a cross sectional area ofA = 0.10 m^2 and the cylinder enclosing the gas has a height of h = 1.0 cm. The gas inside the piston has a temperature T = 300.K. Recall that the internal energy for an ideal gas is U= n cV,mT, where cV,m= 1.5 R is the molar heat capacity for the ideal gas. Calculate the pressure and the internal energy of the ideal gas.

An ideal gas, initially at a pressure of 10.3 atm and a temperature of 312 K, is allowed to expand adiabatically until its volume doubles.   What is the gas’s final temperature, in kelvin, if the gas is monatomic?  What is the gas’s final pressure, in atmospheres, if the gas is diatomic?