What is the molar mass of a pure gaseous compound having a density of 2.95 g/l at 32⁰c and 860 mm hg? (1 atm = 760 mm hg)?

Given:
ρ = 2.95 g/L = 2.95 kg/m³, the density
T = 32°C = 32+273 K = 305 K, the temperature
p = 860 mm Hg = (860/760) atm = 1.1316 atm
   = 1.1316*101325 Pa
   = 1.14657 x 10⁵ Pa

The ideal gas law is
p = ρ*(R/M)*T
where
R = 8.314 J/(mol-K), the gas constant
M = molar mass, kg/mol

The molar mass is

The molar mass is 0.0652 kg/mol = 65.2 g/mol

65.2 g/mol

What does that mean you dum bum

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