The number of moles of water which must be electrolyzed to produce `22.4L` of `O_(2)` at `273K` and 2 atmospheric pressure is

Calculate the number of molecules of carbon dioxide present in 300 mL of gas at 273K and 2.5 atm pressure.

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)

What will be the volume occupied by 2 gm of hydrogen at 300 K and 4 atmospheric pressure if at 273 k and 1 atmospheric pressure the gas occupies 22.4 L.

Show that the volume of 1 gram-molecule of any gas at 273K temperature and 1 atm pressure is 22.4 L.