Question

Pall An experiment shows that a 114 mL gas sample has a mass of 0.170 g at a pressure of 723 mmHg and a temperature of 34 °C. What is the molar mass of the gas? ΑΣΦ g/mol Submit Request Answer

Answer 1

Given v= 114 ml = 1149103 L P = 723 mm Hg - 723 atm 760 m = 0.170 P = 0.95 atm T = 273 +34 = 307k R = 0.0821 Latm/k-mol from Ideal gas egn. PV = nRT 0.95 x 114 4 10 3 = 0.170 40.08214 307 M IM = 39.56 g/mol Ans. Hence nolar mass of gas is 39.56 almal V = 2484 10 L P - 753 – 0.99 atm. 760 m = 0.436 g T = 29+273 = 302 k from Ideal gas ean. PV = nRT o.gg x 248 A 10 3 - 0.436 x 0. 0821 × 302 M = 44 g/mol) Ans

Given m = 279 , m = 44 (CO₂) no n = - 2 44 1 T = 20 + 273 T = 293K n = 0.61 mol P - 756 760 – nigg atm from Ideal gas eqn. PV = nRT 0.99 x V = 0.61 X0.0821 x 293 Iv - 14.82 L Ang