Question

Fill in the Blanks Consider 1.75 g of an unknown gas. This gas is stored in a 2.35 L flask at 53.0 °C and 1.05 atm The density of the gas B/L The molar mass of the gas g/mol

Answer 1

Given: Mass of gas = 1.75 g Volume = 2.3 L Temperature = 53.0 °C +273K = 326 K Pressure = 1.05 atm The ideal gas equation is PV=nRT Mass Molar mass PV=I – Mass P Molar mass= RT V P Molar mass=dxRT PxMolar mass d= RT Calculate the molar mass s follows for calculating the density: PV=nRT PV 1 RT n 1.05 atm x 2.3L 0.08206L atm/K mol 326K =0.0903 mol Also, Mass Molar mass= Moles 1.75g 0.093 mol =0.163g/mol

Mass Molar mass= Moles 1.75g 0.093 mol =0.163g/mol Calculate the density as follows: d= PxMolar mass RT 1.05 atm 0.163 g/mol 0.08206L atm/K mol326K d=0.0064g/L Hence, The density of the gas is 0.0064 g/L). The molar mass of the gas is 0.163 g/mol.

Answer 2

Density is actually 0.745 and molar mass is 18.9- other answer is wrong

Answer 3

molar mass is 19.0