The density of a gas is 1.48 g/L at a temperature of 24 ∘C and a pressure of 0.784 atm . Calculate the molar mass of the gas.?

Density, d = 1.48 g/L
Temperature, T = (273 + 24) K = 297 K
Pressure, P = 0.784 atm
Gas constant, R = 0.08206 L•atm/(mol•K)
Molar mass, M = ? g/mol

PV = nRT and n = m/M
Hence, PV = (m/M)RT
M = (m/V)RT/P
Since, d = m/V, M = dRT/P

Molar mass, M = 1.48 × 0.08206 × 297 / 0.784 g/mol = 46.0 g/mol

1.48 g/L at a temperature of 24 ∘C and a pressure of 0.784 atm .  .......  Separate density into 2 parts ..  1.48g = mass  ...  1L = volume

   PV = nRT  .....  n  =  (PV)/(RT)
   n  =  (0.784 X 1) / (0.0821 X 297)
   n = 0.03215 moles

   molar mass = 1.48g / 0.03215 moles
    =  46.0 g/mol