A `4.0 dm^(3)` flask containing `N_(2) at 4` bar was connected to a `6.0 dm^(3)` flask containing helium at `6` bar , and the gases were allowed to mix isothermally. The total pressure of the resulting mixture will be

A4 dm flask containing N_(2) at 4 bar was connected to 6 dmflask containing He at 6 bar, and the gases were allowed to mix isothermally, then the total pressure of the resulting mixture will be

A 2 L flask containing nitrogen at 60 cm pressure is connected to a 4 L flask containing carbon monoxide at 48 cm pressure. If the temperature is kept constant, calculate the final pressure of the mixture.

At 100^(@)C a 2 litre flask contains 0.4 g of O_(2) and 0.6 g of H_(2) . What is the total pressure of this gas mixture in the flask?

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 10 L flask contains 0.2 mole of CH_4 and 0.3 mole of hydrogen at 25^@ C and which makes non- reacting gaseous mixture. Then, the total pressure inside the flask is

A 0.5 dm^(3) flask contains gas A and 1 dm^(3) flask contains gas B at the same temperature. If density of A= 3g//dm^(3) and that of B= 1.5g //dm^(3) and the molar mass of A= 1//2 of B , the ratio of pressure excerted by gases 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