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+ (n²a/V²)) (V-nb) = nRT

P = nRT/(V-nb) - (n²a/V²)                (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 L²·atm/mol²

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) – (1.205² X 6.49/ 4.75²)

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