All real gases devices to some extent from the behavior of perfect gases. At sta

Question

All real gases devices to some extent from the behavior of perfect gases. At standard conditions, the density of O_2(g) is 0.0014290 g/mL, that of H_2(g) is 0.00008988 g/mL, and that of CO_2(g) is 0.0019769 g/mL. Using these values and the exact atomic weights, calculate the molar volume of milliliters, to five significant figures. Correlate the molar mass, molecular size, and bond polarity of these three gases with the molar volume of a perfect gas. Which gas deviates least? ____ Which gas deviates most? ____

Explanation / Answer

a)

Molar volume = Volume / moles

so..

D = mass / volume

1/D = Volume / mass

mass = mol/MW so..

Moalr V = 1/D*(MW) = MW/D

so..

ai)

O2 = 0.0014290 g/mL

MW of O2 = 15.9994

Molar V = (15.9994 )/0.0014290 = 11196.22 mL per mol

aii)

H2= 0.00008988 g/mL

MW of H2 = 2.01588

Molar V = (2.01588 )/0.00008988 = 22428.57 mL per mol

aiii)

CO2 = 0.0019769 g/mL

MW of H2 = 44.01

Molar V = (44.01 )/0.0019769 = 22262.127 mL per mol

b)

at STP = 1 mol = 22.4L

meaning 22400 mL per mol

O2 = 22400 -11196.22 = 11203.78

H2 = 22400 -22428.57 = -28.57

CO2 = 22400 -22262.127 = 137.873

the gas that must deviate the least ---> H2

the gas that deviates the most --> O2

This must be due to their interacitons (O2 is pretty electronegative, whereas CO2 will be polar)

H2 deviates the least due to smallest size in molecules

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