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A chemist isolated a gas in a glass bulb...

A chemist isolated a gas in a glass bulb with a volume of 255 mL at a temperature of `25^(@)C` and a pressure (in the bulb) of `10.0` torr. The gas weighed `12.1 mg`. What is the molecular mass of the gas?

A

`78.9g mol^(-1)`

B

`35.2g mol^(-1)`

C

`88.2g mol^(-1)`

D

`96.3g mol^(-1)`

Text Solution

Verified by Experts

The correct Answer is:
C
`n=(PV)/(RT)=((10.0" torr")((1 atm)/(760" torr "))(255mL)((1L)/(1000mL)))/((0.0821(L atm)/(mol K))(298.2K))=1.37xx 10^(-4)mol`
Molecular mass `=(" Mass ")/(" Number of moles ")= ((12.1 mg)((1g)/(1000 mg)))/(1.37xx 10^(-4)mol)= 88.2g mol^(-1)`.
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