Using the van der Waals equation, determine the pressure of 500.0 g of SO2 (g) in a 6.30-L vessel at 633 K. For SO2 (g), a = 6.865 L2 • atm/mol2 and b = 0.05679 L/mol. (R = 0.0821 L • atm / (K • mol))

Question

Savanah

Chemistry

31 January, 15:55

Using the van der Waals equation, determine the pressure of 500.0 g of SO2 (g) in a 6.30-L vessel at 633 K. For SO2 (g), a = 6.865 L2 • atm/mol2 and b = 0.05679 L/mol. (R = 0.0821 L • atm / (K • mol))

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Nelson Walsh · Answer 1

The pressure is 58.75 atm.

Explanation:

From Vanderwaal's equation,

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

n is the number of moles of SO2 = mass/MW = 500/64 = 7.81 mol

R is gas constant = 0.0821 L. atm/mol. K

T is temperature of the vessel = 633 K

V is volume of the vessel = 6.3 L

a & b are Vanderwaal's constant = 6.865 L^2. atm/mol^2 and 0.0567 L/mol respectively.

P = (7.81*0.0821*633) / (6.3 - 7.81*0.05679) - (7.81^2 * 6.865) / 6.3^2 = 69.30 - 10.55 = 58.75 atm