Part A. We’re being asked to calculate the pressure exerted by a chlorine gas that deviates from ideal behavior. For this, we shall use the Van der Waal’s equation.
The Van der Waals equation is shown below:
▪ P = pressure, atm
▪ V = volume, L
▪ n = # of moles, mol
▪ R = gas constant = 0.08206 (L∙atm)/(mol∙K)
▪ T = temperature, K
▪ a = polarity coefficient
▪ b = size coefficient
In Sample Exercise 10.16 in the textbook, we found that one mole of Cl2 confined to 22.41 L at 0 oC deviated slightly from ideal behavior. Calculate the pressure exerted by 1.00 mol Cl2 confined to a smaller volume, 6.00 L , at 25 oC.
Why is the difference between the result for an ideal gas and that calculated using van der Waals equation greater when the gas is confined to 6.00 L compared to 22.4 L?
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