Question

5. A sample of gas was measured to have a mass of 0.245 g, pressure 0.998 atm, volume 145.1 mL, and temperature of 99.9 °C. Using this information, determine the molar mass of the compound.

Answer 1

Auswer: we know that PV=NRT (Ideal gas equation) Griven; P = pressure - 0.998 atm V = volume = 1451 mL = 0.14512 T = Temperature = 99.9°c or (273 +99.9)k - 372.9k R = 0.082 L'atmk-moir n = no. of moler = 16 mass of given campanard Molar mass of compound n = 0. 245g M PV = nRT 0.998 atm x 0.1451 L = 0.245 g x 0.082 Latmany X 372.9K me 0.245 x 0.082 X 372.94 04998 X0-1451 + / mo /mol = 51.73379 Mo) Molar mass, M = 51.73378/mol.