Question

# A. Use the van der Waals equation to calculate the pressure exerted by 1.205 mol of...

A. Use the van der Waals equation to calculate the pressure exerted by 1.205 mol of Cl2 in a volume of 4.990 L at a temperature of 286.5 K .

B. Use the ideal gas equation to calculate the pressure exerted by 1.205 mol of Cl2 in a volume of 4.990 L at a temperature of 286.5 K .

Answer – A) We are given, moles of Cl2 = 1.205 moles , volume = 4.990 L ,     T = 286.5 K

We know the van der Waals equation-

(P + n2a / V2)(V- nb) = nRT

For the Cl2 van der Waals equation constant , a = 6.343 atm L2/mol2 , b = 0.05422 L/mol

(P +(1.205)2*6.343 atm L2/mol2 / (4.990)2) (4.990-1.205 mole0.05422 L/mol) = 1.205 mol*0.0821 atm.L/mol.K * 286.5 K

(P+0.370) *(4.92) = 28.34

4.92 P + 1.82 =28.34

4.92 P = 28.34-1.82

= 26.52

P = 5.38 atm

B) Now using the Ideal gas law –

PV = nRT

P = nRT/V

= 1.205 moles * 0.0821 atm.L.mol-1.K-1*286.5 K / 4.990 L

= 5.68 atm.

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