Problem: A chemist vaporized a liquid compound to determine its molar mass. If the density of the vaporized liquid (collected in a 120 mL flask) at 97°C is 3.24 g/L, and the pressure exerted by the vaporized liquid is 0.958 atm, what is its molar mass?(a) 103 g/mol (b) 121 g/mol (c) 187 g/mol (d) 31.6 g/mol(e) Insufficient information was given to calculate molar mass.

FREE Expert Solution

We’re being asked to calculate for the molar mass at 97°C and 0.958 atm. 

To calculate for the molar mass, we’re going to use the ideal gas equation.

PV=nRTPVV=nRTVP=nRTV

n=mass mmolar mass M


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Problem Details

A chemist vaporized a liquid compound to determine its molar mass. If the density of the vaporized liquid (collected in a 120 mL flask) at 97°C is 3.24 g/L, and the pressure exerted by the vaporized liquid is 0.958 atm, what is its molar mass?

(a) 103 g/mol 

(b) 121 g/mol 

(c) 187 g/mol 

(d) 31.6 g/mol

(e) Insufficient information was given to calculate molar mass.

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Our tutors have indicated that to solve this problem you will need to apply the The Ideal Gas Law: Density concept. You can view video lessons to learn The Ideal Gas Law: Density Or if you need more The Ideal Gas Law: Density practice, you can also practice The Ideal Gas Law: Density practice problems .