A volatile liquid is evaporated in a flask in a boiling a water bath (

Temperature = 100°C) with a volume of 297ml. The evaporated gas is

condensed in the flask and it is found to have a mass of 0.435g.

Atmospheric pressure for that day is 765mmHg. What is the Molar Mass of

the Volatile liquid? Show work

Question

John Ruiz

Chemistry

23 March, 11:42

A volatile liquid is evaporated in a flask in a boiling a water bath (

Temperature = 100°C) with a volume of 297ml. The evaporated gas is

condensed in the flask and it is found to have a mass of 0.435g.

Atmospheric pressure for that day is 765mmHg. What is the Molar Mass of

the Volatile liquid? Show work

+1

Answers (1)

Know the Answer?

Bowen · Answer 1

Molecular Weight of gas = 44.418 grams/mole

Explanation:

PV = nRT = (mass/f. wt.) RT = > f. wt. = mass·R·T/P·V

mass = 0.435g

R = 0.08206·L·atm/mol·K

T = 100°C = 372K

P = (765/760) Atm = 1.01Atm

V = 297ml = 0.297L

f. wt. = (0.435g) (0.08206L·Atm/mol·K) (372K) / (1.01Atm) (0.297L) = 44.418 grams/mole