Use the van der Waals equation of state to calculate the pressure of 2.30 mol of

Question

Use the van der Waals equation of state to calculate the pressure of 2.30 mol of CCl_4 at 483 K in a 3.80 L vessel. Van der Waals constants can be found in this table. P = Use the ideal gas equation to calculate the pressure under the same conditions. P = In a 16.0 L vessel, the pressure of 2.30 mol of CCl_4 at 483 K is 5.70 atm when calculated using the ideal as equation and 5.40 atm when calculated using the van der Waals equation of state. Why is the percent difference in the pressures calculated using the two different equations greater when the gas is in the 3.80 L vessel compared to the 16.0 L vessel? The molecular volume is a smaller part of the total volume of the 3.80 L vessel. The molecular volume is a larger part of the total volume of the 3.80 L vessel. The attractive forces between molecules become a greater factor at the higher pressure in the 3.80 L vessel. The attractive forces between molecules become less of a factor at the higher pressure in the 3.80 L vessel.

Explanation / Answer

Pressure calculation

Using Van der Waals equation of state

(P + an^2/V^2) (V - nb) = nRT

Feeding the values,

(P + 19.7483(2.3/3.8)^2) (3.8 - 2.3 x 0.1281) = 2.3 x 0.08205 x 483

P = 18.77 atm

Using ideal gas equation,

P = nRT/V

   = 2.3 x 0.08205 x 483/3.8

   = 23.98 atm

The higher percent difference in the pressure seen in 3.80 L vessel when compared to 16 L vessel is because,

The attractive forces between molecules becomes greater factor at higher pressure in the 3.80 L vessel.

Related Questions

Navigate

• Browse (All)
• Browse U
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.