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?

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 =

                =

                = 0.0247 moles

Temperature = = 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

            =

                   P =

                      = 92.371 torr

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

petroleum? coal maybe?

2b2t

explanation:

2b2t