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

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.

If 1 mole of H_(2) , 2 moles of O_(2) and 3 moles of N_(2) are mixed in a vessel and total pressure was found to be 12 atm then the partial pressure exerted by N_(2) in the vessel will be

If 1 mole of H_(2) , 2 moles of O_(2) and 3 moles of N_(2) are mixed in a vessel and total pressure was found to be 12 atm then the partial pressure exerted by N_(2) in the vessel will be

A mixture of CH_(4), N_(2) and O_(2) is enclosed in a container of 1 litre capacity at 0^(@)C . Total pressure of gaseous mixture is 2660 mm Hg. If the ratio of partial pressures of the gases is 1 : 4 : 2 respectively, the number of moles of oxygen present in the vessel is:

At STP, a container has 1 mole of Ar, 2 mole of CO_(2) , 3 moles of O_(2) and 4 moles of N_(2) . Without changing the total pressure if one mole of O_(2) is removed, the partial pressure of O_(2)

At STP, a container has 1 mole of Ar, 2 mole of CO_(2) , 3 moles of O_(2) and 4 moles of N_(2) . Without changing the total pressure if one mole of O_(2) is removed, the partial pressure of O_(2)

A gaseous mixture of 2 moles of A, 3 moles of B, 5 moles of C and 10 moles of D is contained in a vessel. Assuming that gases are ideal and the partial pressure of C is 1.5 atm, total pressure is