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 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 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

A five litre flask contains 3.5gm of N_2 3g of H_2 and 8g of O_2 at 27^@C . The total pressure exerted by the mixture of these gases is

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))

An enclosure of volume 4 litres contains a mixture of 8 g of oxygen 14 g of nitrogen nand22 g of carbon dioxide. If the temperature of the mixture is 27^(@)C find the pressure of the mixture of gases. Given R=8.315JK^(-1)"mol"^(-1)

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) .

One half mole each of nitrogen, oxygen and carbon dioxide are mixed in enclosure of volume 5 litres and temperature 27^(@) C . Calculate the pressure exerted by the mixture. Given R = 8.31 J mol^(-1) K^(-1) .

One half mole each of nitrogen, oxygen and carbon dioxide are mixed in enclosure of volume 5 litres and temperature 27^(@) C . Calculate the pressure exerted by the mixture. Given R = 8.31 J mol^(-1) K^(-1) .

A vessel of capacity 10 litres contains 0.5 moles of CO_(2) , 1.3 moles ofnitrogen and 0.20 mole of oxygen at 30^(@)C . Assuming the gases to be ideal, find the pressure of the mixture , R = 8.31 J m o l^(-1) K^(-1) .