Question

A flask with a volume of 3.16 L contains 9.33 g of an unknown gas at 32.0°C and 1.00 atm. What is the molar mass of the gas? (R = 0.08206 L • atm/K • mol) Multiple Choice 18 Ο 776 g/mol Ο 144 g/mol Ο 66.1 g/mol Ο 739 g/mol Ο 81.4 g/mol

Answer 1

Solution:

Solution! AS Ideal Gas equation, PV = nRT where, P= Press are of gas v = volume of the gas n= no ob moles R=0.08206 Latm k mol. - Cuniversal Gias constant) T = Temperature Given, p=1.00 atm , v= 3.16L. W (Given = 9.33g TCR)= 32.0+273-15 - mass of gas) = 305.15 R. Putting all values in Ideal gas equation so n = 1.000 3.16 0.08206× 305.15 = 10-126 mol Now, as n (no of moles) = Given mass malar mass Molar mass = Given mass no of moles Molar mass of gas = 9.33 0:1261 = 79.9 g/mol Hence, molar mass of gas = 73.9g mal] Correct and (d) 79.9 g/mol

By using Ideal gas equation, molar mass of the gas is 73.9g/mol. So, correct option is (d) 73.9g/mol, other options are not correct.

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