A flask of `4.48 L` capacity contains a mixture of `N_(2)` and `H_(2)` at `0^(@)C` and `1 atm` pressure. If thed mixture is made to react to form `NH_(3)` gas at the same temperature, the pressure in the flask reduces to `0.75 atm`. Select statement(s) :

A container of 1 L capacity contains a mixture of 4 g of O_(2) and 2 g H_(2) at 0 ^(@)C . What will be the total pressure of the mixture ?

A 2L flask contains 0.4 g O_(2) and 0.6 g H_(2) at 100^(@)C . Calculate the total pressure of the gas mixture in the flask.

A container of 1 L capacity contains a mixture of 4 g of O_(2) and 2 g H_(2) at 0 .^(@)C . What will be the total pressure of the mixture ? (a) 50 . 42 atm (b) 25 . 21 atm (C) 15 . 2 atm (d) 12 . 5 atm

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?

Two flasks A and B of 1L each are filled with O_(2) and SO_(2) gas at 27^(@) C and 1 atm pressure. The flasks will contain .

A 1.0 L flask contains 2.0 g of N_(2), 0.4 g H_(2) and 9.0 of O_(2) at 27^(@)C . What is the pressure in the flask?

If the pressure of a mixture of 56 g of N_(2) and 44.0 g CO_(2) is 3 atm , the partial pressure of N_(2) in the mixture is :

At 127^(0)C and 1 atm pressure, a mixture of a gas contains 0.3 moles of N_(2),0.2 moles of O_(2) ,the volume of the mixture is ( in L )