Initial volume of a gas is `1 L` at temperature `100 K`. What is the volume of a gas at `300 K`.

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

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

What is the change in enthalapy (kcal) when 1 mole of ideal monoatomic gas is expended reversibly and adibatically from initial volume of 1 L and initial temperature 300 K to final volume of 8 L :

1 mole of an ideal diatomic gas undergoes a reversible polytropic process (PV^(2)=K) .The gas expands from initial volume of 1L to 3L and initial temperature of 300K what is the change in internal energy |Delta U| in cal [(R=2calmol^(-1)K^(-1))]

One mole of an ideal gas expands at a constant temperature of 300 K from an initial volume of 10 litres to a final volume of 20 litres. The work done in expanding the gas is (R=8.31J/mole-K)

Calculate the volume of one mole of any gas at STP and at room temperature (300K) with the same pressure 1 atm.

0.5 mole of gas at temperature 300 K expands isothermally from an initial volume of 2.0L to final volume of 6.1L. How much heat is supplied to the gas?.

0.5 mole of gas at temperature 300 K expands isothermally from an initial volume of 2.0L to final volume of 6.0L. What is the work done by the gas ? (R = 8.31 J mol^(-1) K^-(1)

Two moles of an ideal monoatomic gas occupy a volume 2V at temperature 300K, it expands to a volume 4V adiabatically, then the final temperature of gas is