Question

Assume that all samples listed below have the same pressure and temperature. Which would have the greatest volume? A.1 gram of O2 B.all have the same volume C.1 gram of Ar D.1 gram of H2 E.not enough information

Answer 1

Answer: 1 gram of
`H_2`.

Explanation: Avogadro's Law: This law states that volume is directly proportional to the number of moles of the gas at constant pressure and temperature.

`V\propto n` (At constant temperature and pressure)

`(V_1)/(n_1)=(V_2)/(n_2)`

where,

`V_1` = initial volume of gas

`V_2` = final volume of gas

`n_1` = initial number of moles

`n_2` = final number of moles

a) 1 gram of
`O_2`

`Moles=\frac{\text{Given mass}}{\text{Molar mass}}=(1g)/(32g/mol)=0.03125moles`

c) 1 gram of Ar

`Moles=\frac{\text{Given mass}}{\text{Molar mass}}=(1g)/(40g/mol)=0.025moles`

d) 1 gram of
`H_2`

`Moles=\frac{\text{Given mass}}{\text{Molar mass}}=(1g)/(2g/mol)=0.5moles`

Thus the one having highest number of moles will have highest volume which is for 1 gram of
`H_2`.