What will be the partial pressures of He and `O_(2)` respectively if 200 ml of He at 0.66 atm pressure and 400 ml of `O_(2)` at 0.52 atm pressure are mixed in 400 ml vessel at `20^(@)C` ?

If 200mL of He at 0.66 atm and 400 mL of O_(2) at 0.52 atm pressure are raised in 400 mL vessel at 20^(@)C then find the partial pressures of He and O_(2) ?

If 200mL of He at 0.66 atm and 400 mL of O_(2) at 0.52 atm pressure are raised in 400 mL vessel at 20^(@)C then find the partial pressures of He and O_(2) ?

10 ml of H_(2)O_(2) could release 224 ml of O_(2) at 273K and 2 atm pressure. What is the molarity of that H_(2)O_(2)

A balloon contains 500m^(3) of He at 27^(@)C and 1 atm pressure. Then , the volume of He at -3^(@)C and 0.5 atm pressure will be

0.3 g of a gas has a volume of 112 ml at 0^@C and 2atm pressure. Its Molecular weight is

If 250 mL of N_(2) over water at 30^(@)C and a total pressure of 740 torr is mixed with 300 mL of Ne over water at 25^(@)C and a total pressure of 780 torr, what will be the total pressure if the mixture is in a 500 mL vessel over water at 35^(@)C . (Given : Vapour pressure (Aqueous tension )of H_(2)O at 25^(@)C and 35^(@)C are 23.8, 31.8 and 42.2 torr respectively. Assume volume of H_(2)O(l) is negligible in final vessel)

If 250 mL of N_(2) over water at 30^(@)C and a total pressure of 740 torr is mixed with 300 mL of Ne over water at 25^(@)C and a total pressure of 780 torr, what will be the total pressure if the mixture is in a 500 mL vessel over water at 35^(@)C . (Given : Vapour pressure (Aqueous tension )of H_(2)O at 25^(@)C and 35^(@)C are 23.8, 31.8 and 42.2 torr respectively. Assume volume of H_(2)O(l) is negligible in final vessel)