Arrange the following gases in order of increasing rate of effusion at 298 deg K. (Hint:...

Arrange the following gases in order of increasing rate of effusion at 298 deg K. (Hint:

Look up the correct chemical formulas of these.)

a. Argon b. Hydrogen bromide c . Ethane (formula?) d. Carbon monoxide

__________ ___________ ____________ _____________ Slowest

2- a. Under what two circumstances is the ideal gas equation not obeyed by ordinary gases?

b. What is the importance of van der Waals equation?

Expert Solution

molar masses : HBr= 1+80=81 , Argon =40, Ethane (C2H6)= 2*12+6*1= 30, CO =12+16=28

The rate of effusion, according to Grahm's law is inversely proportional to square root of molar massese. So higher the molar mass,lower the effusin rate. Hence the order of effusion rate ( from lower to higher)

HBr<Ar<C2H6<CO

2. Ideal gas law is not obeyed at high pressure and low temperature. Because in case of ideal gas, the interaction between molecules is ignored. At high pressure or at low temperature, the molecules are close apart so that they will be under the influence of attractive forces.

3. The Vanderwaal equation for one moles of gas is (P+a/V2)*(V-b)=RT

a/V2 is takes care of interaction between molecules of gas.

"b" is a correction for finite molecular size and its value is the volume of one mole of the atoms or molecules

the Vanderwaal constants "a" and "b" can be used to determine the critical constant. since

Vc= 3b and Pc= a/27b²

a=

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