A gas heated from 273 k to 373k at 1atm pressure if the initial volume of the gas is 10L its fin...

A gas is heated from 0^(@)C to 100^(@)C at 1.0 atm pressure. If the initial volume of the gas is 10.0L, its final volume would be:

Two moles of a gas expand reversibly and isothermally at temperature of 300K. Initial volume of the gas is 1 L while the final pressure is 4.926 atm . The work done by gas is

One mole of an ideal gas is heated from 273K to 546K at constant pressure of 1 atmosphere. Calculate the work done by the gas in the process.

One mole of an ideal monoatomic gas expands isothermally against constant external pressure of 1 atm from initial volume of 1L to a state where its final pressure becomes equal to external pressure. If initial temperature of gas is 300K then total entropy change of system in the above process is: [R=0.082L atm mol^(-1) K^(-1)-=8.3J mol^(-1) K^(-1)]

One mole of an ideal monoatomic gas expands isothermally against constant external pressure of 1 atm from intial volume of 1L to a state where its final pressure becomes equal to external pressure. If initial temperature of gas in 300 K then total entropy change of system in the above process is: [R=0.0082L atm mol^(-1)K^(-1)=8.3J mol^(-1)K^(-1)]

One mole gas is first colled from 300 K to 150 K at constant volume and then heated from 150K to 300 K at constant pressure. The net heat absorbeed by the gas is

One litre gas at 400K and 300atm pressure is compressed to a pressure of 600 atm and 200K . The compressibility factor is changed from 1.2 to 1.6 respectively. Calculate the final volume of the gas.