`16 g` of `O_(2)` gas and `x g` of `H_(2)` occupy the same volume at the same temperature and pressure. Then `x =`

If 16 gm of oxygen and x gm of hydrogen has the same volume at the same temperature and pressure, then find the value of x.

If 0.2g of a gas 'X' occupies a volume of 440 ml and if 0.1 g of CO_(2) gas occupies a volume of 320 ml at the same temperature and pressure , X could be

0.2 g of a gas 'x' occupy a volume of 440 ml . If 0.1 g of CO_2 gas occupy a volume of 320 ml at the same temperature and pressure , then the gas 'x' could be

3.4g of a gas at 17^@C occupied sam e volume as 0.16 gram of H_2 at the same temperature and pressure Molecular mass of the gas is

Assetion (A): 1 mol H_(2) and N_(2) have same volume at same temperature and pressure. Reason (R ): 1 mol gas at STP occupies 24.4L volume.

Assetion (A): 1 mol H_(2) and N_(2) have same volume at same temperature and pressure. Reason (R ): 1 mol gas at STP occupies 24.4L volume.

A mixture of CH_(4) and C_(2)H_(2) occupied a certain volume at a total pressure equal to 63 torr. The same gas mixture was burnt to CO_(2) and H_(2)O(l).CO_(2)(g) alone was collected in the same volume and at the same temperature, the pressure was found to be 99 torr. What was the mole fraction of CH_(4) in the original gas mixture?

A mixture of CH_(4) and C_(2)H_(2) occupied a certain volume at a total pressure equal to 63 torr. The same gas mixture was burnt to CO_(2) and H_(2)O(l).CO_(2)(g) alone was collected in the same volume and at the same temperature, the pressure was found to be 99 torr. What was the mole fraction of CH_(4) in the original gas mixture?