Ten moles of a diatomic perfect gas are allowed to expand at constant pressure. The initial volume and temperature are `V_0` and `T_0` respectively. If `7/2RT_0` heat is transferred to the gas, then the final volume and temperature are

An ideal gas is found to obey the law V^2T = constant . The initial pressure and temperature are P_0 and T_0 . If gas expands such that its pressure becomes (P_0)/4 , then the final temperature of the gas will be

A gas is found to be obeyed the law p^2V = constant . The initial temperature and volume are T_0 and V_0 . If the gas expands to a volume 3 V_0 , then the final temperature becomes.

A gas is found to be obeyed the law p^2V = constant . The initial temperature and volume are T_0 and V_0 . If the gas expands to a volume 3 V_0 , then the final temperature becomes.

One mole of a monatomic ideal gas has an initial pressure, volume, and temperature of P_0 , V_0 , and 438 K, respectively. It undergoes an isothermal expansion that triples the volume of the gas. Then, the gas undergoes an isobaric compression back to its original volume. Finally, the gas undergoes an isochoric increase in pressure, so that the final pressure, volume, and temperature are p_0 V_0 and 438 K, respectively. Find the total heat for this three-step process, and state whether it is absorbed by or given off by the gas.

An ideal gas is found to obey a gas law, Vp^2 = constant .Initial temperature and volume of the gas are T and V respectively. IF the gas expands to a volume 2V, what will be the effect on temperature?

4 moles of an ideal gas is at 0^(@) C . At constant pressure it is heated to double its volume, then its final temperature will be