2.9 g of a gas at `95^@C` occupied the same volume as 0.184 g of dihydrogen at `17^@C`, at the same pressure. What is the molar mass of the gas?

Explanation

Density of dioxygen `(O_(2))` at `4.5 "bar"` pressure and `10^(@)C`
`rho_(O_(2))=(PM)/(RT)=(4.5xx32)/(Rxx283.15)`
`rho_(oxide)=(PM)/(RT)=(1.5xxM)/(Rxx293.15)`
Now, `rho_(O_(2))=rho_(oxide)`
`:. (4.5xx32)/(Rxx283.15)=(1.5xxM)/(Rxx293.15)`
or `M=(4.5xx293.15xx32)/(283.15xx15)=99.39 g mol^(-1)`
Therefore, the molecular mass of oxygen dioxide is `99.39 g mol^(-1)`