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b. Use the Vander Waal equation to calculate the pressure of 1.00 mol of Cl₂ in a volume of 30.0L at a temperature of 600.0K. And determine the relationship between the Vander Waal and the ideal gas equation. (Please check the Vander Waal constants online) [5 marks]​

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The value of the pressure calculated from the Vander Waal equation is slightly less than that is calculated from the ideal gas equation.

What is the pressure?

We know that the ideal gas equation assumes that there is no interaction that exists between gas molecules. The ideal gas equation corrects the ideology with the addition of constants that take care of possible interaction between gases.

Now, using the ideal gas equation;

PV =nRT

P = ?

V =  30.0L

T = 600.0K

n = 1.00 mol

R = 0.082 atmLK-1mol-1

P = nRT/V

P =  1.00 mol *  0.082 atmLK-1mol-1 *  600.0K/30.0L

P = 1.64 atm

Using the Vander Waal equation

a = 6.49

b = 0.0562

Thus;

P = RT/V - b  -  a/V^2

P = 0.082 * 600.0/30.0 - 0.0562 - 6.49/(30)^2

P = 49.2/29.9438 - 6.49/900

P = 1.64 - 0.00721

P = 1.63 atm

Thus the value of the pressure calculated from the Vander Waal equation is slightly less than that is calculated from the ideal gas equation.

Learn more about ideal gas equation:https://brainly.com/question/4147359

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