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)

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 H_2 gas is 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 of 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)

An ideal gas is expanded adiabatically at an initial temperature of 300 K, so that it's volume is doubled. The final temperature of the hydrogen gas is (Take, gamma = 1.40).

The temperature of an ideal gas is 340 K. the gas is heated to a temperature at constant pressure. As a result, its volume increases by 18%. What is the final temperature of the gas?