At constant temperature `200 cm^(3)` of `N_(2)` at 720 mm and `400 cm^(3)` of `O_(2)` at 750 mm presure are put together in a litre flask. The final pressure of mixture is

At constant temperature 200 cm^(3) of N_(2) at 720 mm and 400 cm^(3) of O_(2) at 750 mm pressure are put together in a litre flask. The final pressure of mixture is

At constant temperature 200 cm^(3) of N_(2) at 720 mmHg and 400 cm^(3) of O_(2) at 750 mmHg pressure are put together in a liter flask. The final pressure of mixture will be

At a constant temperature, 250 mL of argon at 760 mm pressure and 600 mL of nitrogen at 500 mm pressure are put together in a one litre flask. Calculate the final pressure.

200 ml of O_2 gas maintained at 700mm pressure and 250ml of N_2 gas maintained at 720mm pressure are put together in one litre flask. If the temperature is kept constant, the final pressure of the mixture in mm is

400 mL of N_(2) gas at 700 mm and 300 mL of H_(2) gas at 800 mm are introduced into a vessel of 2 L at the same temperature. Calculate the final pressure of the gas mixture.

400 mL of N_(2) gas at 700 mm and 300 mL of H_(2) gas at 800 mm are introduced into a vessel of 2 L at the same temperature. Calculate the final pressure of the gas mixture.

200 mL of hydrogen and 250 mL of nitrogen each measured at 15^(@)C and 760 mm pressure are but together in a 500 mL flask. What will be the final pressure of the mixture at 15^(@)C ?

At constant temperature 2L of N_(2) gas at 750 mm Hg pressure I mixed with 3L of O_(2) gas. As a result the pressure and volume of the gas mixture are found to be 732 mm Hg and 5 L respectively. What is the initial pressure of O_(2) gas?