2.15 g of an unknown gas at 71 degrees C and 1.10 atm is stored in a 1.75 L flask.

What is the density of the gas?

What is the molar mass of the gas?

Applying gas law:

PV=nRT

n/V = (1.10 atm) / ((0.08205746 L atm/K mol) x (71 + 273) K) = 0.0389 mol/L

density:

(1.10 g) / (1.75 L) = 0.628 g/L

molar mass:

(0.628 g/L) / (0.0389 mol/L) = 16.14 g/mol

its molar mass is nearly equal to NH3 that is 17.