.The vapor pressure of a volatile liquid can be determined by slowly bubbling a known volume of gas through it at a known temperature and pressure. In an experiment, 5.01 L of N2 gas is passed through 7.9286 g of liquid benzene, C6H6, at 27.3 ∘C and atmospheric pressure. The liquid remaining after the experiment weighs 5.9987 g . Assuming that the gas becomes saturated with benzene vapor and that the total gas volume and temperature remain constant, what is the vapor pressure of the benzene in torr?

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OlaMacgregor OlaMacgregor · Answer 1 · 2019-09-16T08:16:23+02:00

Explanation:

It is given that the initial mass of benznene is 7.9286 g

Mass of benzene left = 5.9987 g

So, mass of benzene with which gas get saturated will be calculated as follows.

= 7.9286 g - 5.9987 g = 1.9299 g

Therefore, moles of benzene with which gas get saturated = [tex]\frac{mass}{ molar mass}[/tex]

= [tex]\frac{1.9299 g}{78.112 g/mol}[/tex]

= 0.0247 moles

Temperature = [tex]27.3^{o}C[/tex] = 27.3 + 273.15 = 300.45 K

Volume = 5.01 L

So, according to ideal gas equation PV = nRT

Putting the given values into the ideal gas equation as follows.

PV = nRT

[tex]P \times 5.01 L[/tex] = [tex]0.0247 mol \times 62.36 torr-liter/mol K \times 300.45 K[/tex]

P = [tex]\frac{462.781 torr-liter}{5.01 L}[/tex]

= 92.371 torr

Hence, we can conclude that vapor pressure of benzene is 92.371 torr.