Two balloons A and B containing `0.2` mole and ` 0.1` mole of helium at room temperature and ` 2.0` atm, respectively, are connected. When equilibrium is setablished, the final pressure of He in the system is

Two balloons A and B containing 0.2 mole and 0.1 mole of helium at room temperature and 2.0 atm, respectively, are connected. When equilibrium is established, the final pressure of He in the system is

How many moles of Helium gas occupy 22.4L at 0C and 1atm pressure

In a thermally isolated system, two boxes filled with an ideal gas are connected by a valve. When the valve is in closed position, states of the box 1 and 2, respectively, are (1 atm, V, T) and (0.5 atm, 4V, T). When the valve is opened, the final pressure of the system is approximately

Two mole of Hydrogen and three mole of Helium are mixed at room temperature and at atmospheric pressure P_a and the mixture occupies a volume V.

Two mole of Hydrogen and three mole of Helium are mixed at room temperature and at atmospheric pressure P_a and the mixture occupies a volume V.

A vessel contains 0.25 moles of Helium and 0.15 moles of neon at 298K and 2.4 atmosphere pressure. Calculate the partial pressure of each gas in the mixture.

A container is divided into two chambers by a partition. The volume of first chamber is 4.5 litre and second chamber is 5.5 litre. The first chamber contain 3.0 moles of gas at pressure 2.0 atm and second chamber contain 4.0 moles of gas at pressure 3.0 atm. After the partition is removed and the mixture attains equilibrium, then, the common equilibrium pressure existing in the mixture is "x"xx10^(-1) atm. Value of x is "___" .

How many moles of Helium gas occupy 22.4 L at 0^(@)C at 1 atm pressure?