1 mole of `H_(2)` gas is contained in a box of volume `V=1.00m^(3)` at T=300 K. The gas is heated to a temperature of T=300 K and the gas gets converted to a gas of hydrogen atoms. The final pressure would be (considering all gases to be ideal)

1 mole of H_(2) gas is contained in box of volume V= 1.00 m^(3) at T = 300 K . The gas is heated to a temperature of T = 3000 K and the gas gets converted to a gas of hydrogen atoms. The final pressure would be (considering all gases to be ideal)

1 mole of H_(2) gas in contained in a box of volume V 1.00 m^(3) at T =300 K. The gas is heated to a temperature of T= 3000K and the gas gets converted to a gas of hydrogen atoms. The final pressure would be (considering all gases to be ideal)

One mole of a certain gas is contained in a vessel of volume V = 0.250 1 . At a temperature T_1 = 300 K the gas pressure is p_1 = 90 atm , and at a temperature T_2 = 350 K the pressure is p_2 = 110 atm . Find the Van der Walls parameters for this gas

An ideal gas is expanded adiabatically at an initial temperature of 300 K so that its volume is doubled. The final temperature of the hydrogen gas is lambda=1.40)

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

300 ml of a gas at 300 K is cooled to 276 K at constant pressure. The final volume is

Find the average momentum of molecules of hydrogen gas in a container at temperature 300K .