Question

Use the van der Waals equation to calculate the pressure exerted by 1.205 mol of Cl2 in a volume of 4.755 L at a temperature of 302.0 K . Use the ideal gas equation to calculate the pressure exerted by 1.205 mol of Cl2 in a volume of 4.755 L at a temperature of 302.0 K

Answer #1

**Van Der Waals equation,**

(P+ (n^{2}a/V^{2})) (V-nb) = nRT

P = nRT/(V-nb) - (n^{2}a/V^{2})
(1)

In the given problem,

n = 1.205, R = 0.0821 L atm K^{−1} mol^{−1}

T = 302.0 K, V = 4.755 L

a = 6.49 L^{2}·atm/mol^{2}

b = 0.05622 L/mol

Substituting the above values in equation (1)

P = (1.205 X 0.0821 X 302.0)/(4.75-1.205 X 0.05622) –
(1.205^{2} X 6.49/ 4.75^{2})

P = 5.963 atm

**Ideal Gas equation,**

PV = nRT

P = nRT/V

P = (1.205 X 0.0821 X 302.0/4.75)

P = 6.29 atm

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