If 500 mL of gas A at 1000 torr and 1000 mL of gas B at 800 torr are placed in a 2 L container, ...

If 1 L of gas A at 600 torr and 500 mL of gas B at 1000 torr are placed in 2 L flask , the final pressure will be

1000 ml of a gas A at 600 "torr" and 500 ml of a gas B at 800 "torr" are placed in a 2L flask. The final pressure will be

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.

500 mL of nitrogen at 0.936 bar pressure and 1000 mL oxygen at 0.80 bar pressure are put together in a 2 L flask. IF temperature is kept constant, calculate the final pressure of the mixture.

400mL of CO_(2) gas at 0.892 bar pressure and 800mL of CH_(4) gas at 0.921 bar pressure are put into a 2L flask. Calculate the total pressure of the mixture assuming temperature is kept constant.

The pressure of sodium vapour in a 1.0 L container is 10 torr at 1000^(@)C . How many atoms are in the container?

Two gases in adjoining vessels were brought into correct by opening a stopcock between them. The one vessel measured 0.25 L and contained NO gas at 800 torr and 220 K , the other measured 0.1 L contained O_(2) gas at 600 torr and 220 K . The reaction to form N_(2)O_(4)(s) exhausts the limiting reagent completely, ( a ) Neglacting the vapour pressure of N_(2)O , what is the pressure of the gas remaining at 220 K after complection of the reaction? ( b ) What weight of N_(2)O is formed?