4g of `O_(2) and 2g " of " H_(2)` are confined in a vessel of capacity 1 litre at `0^(@)C`. Calculate
the total pressure of the gaseous mixture.

4 g of O_2 and 2g of H_2 are confined in a vessel of capacity 1 litre at 0^@C . Calculate the partial pressure of each gas, and

4 g of O_2 and 2g of H_2 are confined in a vessel of capacity 1 litre at 0^@C . Calculate the number of moles of each gas

Pressure of a mixture of 4 g of O_2 and 2 g of H_2 confined in a bulb of 1 litre at 0^@C is

A gaseous mixture containing 8g of O_(2) and 227 mL of N_(2) at STPis enclosed in flask of 5 L capacity at 0^(@)C . Find the partial pressure of each gas and calculate the total pressure in the vessel.

2g of H_2 and 17g of NH_3 are placed in a 8.21 litre flask at 27^@C . The total pressure of the gas mixture is?

A flask of 1.5 L capacity contains 400 mg of O_(2) and 60 mg of H_(2) at 100^(@)C . Calculate the total pressure of the gaseous mixture. If the mixture is permitted to react to form water vapour at 100^(@)C , what materials will be left and what will be their partial pressures?

1 mole of sample of O_2 and 3 mole sample of H_2 are mixed isothermally in a 125.3 litre container at 125^@C the total pressure of gaseous mixture will be

A gaseous mixture containing 0.35g of N_(2) and 5600 ml of O_(2) at STP is kept in a 5 litres flask at 300K. The total pressure of the gaseous mixture is

A vessel of capacity 3 litres contains 22g of CO_(2) and 28 g of nitrogen at 30^(@)C . Calculate the partial pressure and hence the total pressure exerted by the gas mixture. R = 8.31 J m o l^(-1) K^(-1) .

32 g of oxygen and 2 g of hydrogen are placed in 1.12 litre flask at 0^∘C . Find the total pressure in atm of the gas mixture.