Question

A sample of an unknown compound is vaporized at 150.°C . The gas produced has a volume of 960.mL at a pressure of 1.00atm , and it weighs 0.941g . Assuming the gas behaves as an ideal gas under these conditions, calculate the molar mass of the compound.

Answer 1

34.02 g.

Step-by-step explanation:

Hello!

In this case, since the gas behaves ideally, we can use the following equation to compute the moles at the specified conditions:

`PV=nRT\\\\n=(1.00atm*0.960L)/(0.08206(atm*L)/(mol*K)*(150+273)K) =0.0277mol\\\\`

Now, since the molar mass of a compound is computed by dividing the mass over mass, we obtain the following molar mass:

`MM=(0.941g)/(0.0277mol) \\\\MM=34.02g/mol`

So probably, the gas may be H₂S.

Best regards!