Calculate the temperature of 4.0 mol of a gas occupying 5 `dm^3` at 3.32 bar.
(R=0.083 bar `dm^3 K^(-1) mol^(-1)`)

Calculate the pressure in atm of 1.0 mol of helium in a 2.0 dm^3 container at 20.0^@C .

Calculate the volume occupied by 8.8g of CO_2 at 31.1^@C and 1 bar pressure R=0.083 bar dm^3 K^-1 mol^-1 .

Calculate the pressure in atm of 1.0mole of helium in a 2.0dm^3 container at 20^@ C solution:

Calculate the total pressure in a mixture of 8g of dioxygen and 4 g dihydrogen confined in a vessel of 1 dm^3 at 27^@ C R = 0.083 a bar dm^3 K^(-1)

Calculate the total pressure in a mixture of 8g of dioxygen and 4 g dihydrogen confined in a vessel of 1 dm^3 at 27^@ C R = 0.083 a bar dm^3 K^(-1)

Pay load is defined as the difference between the mass of displaced air and the mass of the ballon. Calculate the pay load when a ballon of radius 10m, mass 100kg is filled with helium at 1.66 bar at 27^@C (Destiy of air = 1.2 kg m^(-3) and R=0.083 bar dm^3 K^-1 mol^-1 .

The volume occupied by 1.8 g of water vapour at 374 ^@C and 1 bar pressure will be . [Use R = 0.083 ba r L K^(-1) mol^(-1) ]

If 1.71g of sugar (molarmass = 342) are dissolved in 500 cm3 of a solution at 300K, what will be its osmotic pressure? (R = 0.082 L bar K^(-1) mol^(-1)) .

At constant temperature, a quantity of an ideal gas occupies 50 dm^3 at 0.5 atm pressure. At what volume, the pressure will be 0.25 atm?