A gaseous compound has a density of 1.17 g/L at 25.5 °C and 1.18 atm. What is the molar mass of the compound?

Answer 1

PV = nRT

P = pressure = 1.18 atm

V = volume = assume 1 L

n = moles = ?

R = gas constant = 0.0821 Latm/Kmol

T = temperature in K = 25.5 + 273 =. 298.5K

solve for n …

n = PV/RT. = (1.18)(1)/(0.0821)(298.5)

n = 0.00481 moles

molar mass = g/moles = 1.17g / 0.00481 moles

molar mass = 243 g/mole