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 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 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 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)

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)

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?

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).