Question

the van der waals equation for n moles of a real gas is p + a(n/v)^2(v - nb) = nrt. if a and b are van der waals constants, which constant accounts for the finite size of gas molecules? * 1 point
r
t
a
b

for a given gas, the van der waals constant a is a measure of: * 1 point
the frequency of collisions between the molecules and the container walls.
the average kinetic energy of the molecules.
the strength of the attractive forces between the molecules.
the volume occupied by one mole of the gas.

a container holds 2.0 moles of nitrogen gas (n2) at 273 k in a volume of 22.4 l. assuming ideal gas behavior, the pressure would be 2.0 atm. however, nitrogen is a real gas. to calculate the actual pressure more accurately, we would use:

Explanation:

1. In the van der Waals equation $[P + a(n/V)^2](V - nb)=nRT$, the constant 'b' accounts for the finite size of gas molecules. It represents the volume occupied by the gas molecules themselves.
2. The van der Waals constant 'a' is a measure of the strength of the attractive forces between the molecules. It corrects for the intermolecular - force effects on pressure.
3. To calculate the actual pressure of a real gas more accurately, we use the van der Waals equation $[P + a(n/V)^2](V - nb)=nRT$ instead of the ideal - gas law $PV = nRT$.

Answer:

1. D. b
2. C. The strength of the attractive forces between the molecules.
3. The van der Waals equation $[P + a(n/V)^2](V - nb)=nRT$