1. Molecules of an ideal gas are abstract points in space and have no volume, wh

Question

1. Molecules of an ideal gas are abstract points in space and have no volume, whereas, a real gas is composed of actual molecules whose atoms occupy some space and interact with each other. The actual gas law for real gases hollows the equation: n a (P+, -) * (V-nb) = nRT Where P, V, n, R and T are the same variables as in the ideal gas law; and the constants and b depend on the nature of the gas. Using the above equation, calculate the pressu 22.4 L. Compare-this pressure to the pressure of an ideal gas and explain if temperature can effect the variation from ideal by 2.5 moles of CoHo at 500°C and in a volume of ior. (10 points) a=18.00 atmL2/mol- 500°C 293-743h + b = 0.1154 L/mol n 2.

Explanation / Answer

the moles "n" must be used in the equation

they do not need to be hcanged to mass

Simply substitute

The Van der Waals equation is a description of real gases, it includes all those interactions which we previously ignore in the ideal gas law.

It considers the repulsion and collision, between molecules of gases. They are no longer ignored and they also are not considered a"point" particle.

The idel gas law:

PV = nRT

P(V/n) = RT ; let V/n = v; molar volume

P*v = RT

now, the van der Waals equation corrects pressure and volume

(P+ a/v^2) * (v - b) = RT

where;

R = idel gas law; recommended to use the units of a and b; typically bar/atm and dm/L

T = absolute temperature, in K

v = molar volume, v = Volume of gas / moles of gas

P = pressure of gas

Knowing this data; we can now substitute the data

given

a = 3.6551

b = 0.04281

(P+ a/v^2) * (v - b) = RT

Get v = V/n = 22.4/2 = 11.4 V/mol

(P + 18 / 11.4 ) * (11.4 - 0.1154) = 0.082*(500+273)

slve for P

P = 0.082*(500+273)/ (11.4 - 0.1154) -  18 / 11.4

P = 4.0380 atm

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