In a flask of volume 8.2 litres there is a mixture of "1" mole of `N_(2)` and 1 mole of He at `27^(@)C` .The pressure exerted by the mixture in atmospheres is (R=0.082L atm `K^(-1)mol^(-1))`

A vessel of volume 4 litres contains a mixture of 8g of O_(2), 14g of N_(2) and 22 g of CO_(2) at 27^(0)C . The pressure exerted by the mixture is

A vessel of volume 4 litres contains a mixture of 8 grams of O_(2) , 14 grams of N_(2) and 32 grams of SO_(2) at 27^(@) C . Find the pressure exerted by the mixture. Given, R = 8.3 J mol_(-1) K_(-1) .

A five litre flask contains 3.5gm of N_(2), 3g of H_(2) and 8g of O_(2) at 27^(0)C . The total pressure exerted by the mixture of these gases

An enclosure of volume 3 litre contains 16g of oxygen, 7 g of nitrogen and 11 g of carbon - di-oxide at 27^(@)C . The pressure exerted by the mixture is approximately [R = 0.0821 lit "atm mole"^(-1) K^(-1)]

In a flask of volume V litres, 0.2 mole of oxygen, 0.4 mole of nitrogen, 0.1 mole of NH_(3) and 0.3 mole of He are enclosed at 27^(@)C . If the total pressure exerted by these non-reacting gases is one atmosphere, the partial pressure exerted by nitrogen is

In a flask of volume V litres, 0.2 mol of oxygen 0.4 mol of nitrogen, 0.1 mole of NH_(3) and 0.3 mol of He are enclosed at 27^(@)C . If the total pressure exerted by these non reacting gases is one atmosphere, the partial pressure exerted by nitrogen is

If two moles of an ideal gas at 500 K occupies a volume of 41 litres, the pressure of the gas is (R = 0.082 L atm K^(-1) mol^(-1))