Question

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 #1

**Answer – A)** We are given, moles of
Cl_{2} = 1.205 moles , volume = 4.990 L ,
T = 286.5 K

We know the van der Waals equation-

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

For the Cl_{2} van der Waals equation constant , a =
6.343 atm L^{2}/mol^{2} , b = 0.05422 L/mol

(P +(1.205)^{2}*6.343 atm L^{2}/mol^{2}
/ (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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Problem 18.41
For oxygen gas, the van der Waals equation of state achieves its
best fit for a=0.14N⋅m4/mol2 and
b=3.2×10−5m3/mol.
Part A
Determine the pressure in 1.7 mol of the gas at 9 ∘C if its
volume is 0.50 L , calculated using the van der Waals equation.
Express your answer using two significant figures.
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Determine the pressure in 1.7 mol of the gas at 9 ∘C if its
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