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Natalka [10]
3 years ago
5

What would be the pressure of a 5.00 mol sample of Cl₂ at 400.0 K in a 2.00 L container found using the van der Waals equation?

For Cl₂, a = 6.49 L²・atm/mol² and b = 0.0652 L/mol.
Chemistry
1 answer:
marusya05 [52]3 years ago
8 0

Answer:

57.478atm

Explanation:

T = 400k

n = 5mol

v = 2.00

a = 6.49L^{2}

b = 0.0652L/mol

R = 0.08206

Formula

P =  \frac{RT}{(\frac{v}{n} )-b} - \frac{a}{(\frac{v}{n} )^{2} }

P = \frac{0.08206 * 400}{(\frac{2.00}{5.00} )-0.0652} - \frac{6.49}{(\frac{2.00}{5.00} )^{2} }

P = \frac{32.824}{0.3348} - \frac{6.49}{0.16}  

P = 98.041 - 40.563

P = 57.478atm

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