A sample of an unknown compound is vaporized at 170 (degrees) C. The gas produced has a volume of 1980. mL at a pressure of 1.00atm, and it weighs 5.17g.

Assuming the gas behaves as an ideal gas under these conditions, calculate the molar mass of the compound. Round your answer to 3 significant digits. In g/mol.

Question

Jamie Webster

Chemistry

4 March, 08:24

A sample of an unknown compound is vaporized at 170 (degrees) C. The gas produced has a volume of 1980. mL at a pressure of 1.00atm, and it weighs 5.17g.

Assuming the gas behaves as an ideal gas under these conditions, calculate the molar mass of the compound. Round your answer to 3 significant digits. In g/mol.

+2

Answers (1)

Know the Answer?

Rambler · Answer 1

The answer to your question is: 0.28 g/mol

Explanation:

Data

T = 170°C = 443°K

V = 1980 ml

P = 1 atm

m = 5.17 g

R = 0.082 (atm l) / (mol°K)

Formula

PV = nRT

Process

n = RT / PV

Substitution

n = (0.082 x 443) / (1 x 1.98 l)

n = 36.33 / 1.98

n = 18.35 moles

Molar mass = 5.17 / 18.35

= 0.28 g/mol