Asample of an unknown compound is vaporized at 170 c. the gas produced has a volume of 1980 ml at a pressure of 1 atm, and it weighs 5.17 gr. 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.

The molar mass is 95.7 g/mol

Explanation:

As the vapor formed is showing ideal gas behavior, it will obey ideal gas law.

PV = nRT

Where

P = Pressure = 1 atm

V = volume = 1980 mL = 1.98 L

n = moles of gas

R = gas constant = 0.0821 L atm /mol K

T = Temperature = 170 °C = 170+273 = 443 K

Putting values

1 X 1.98 = n X 0.0821 X 443

n = moles = 0.054 mol

the relation between moles and molar mass and mass is:

Therefore

atomic mass = 39

number of neutrons = 20

number of protons= 19

electronic configuration = 1s2 2s2 2p6 3s2 3p6 4s1

the number of electron in first shell = 2

number of electrons in n=3 shell = 8