The vapor pressure of liquid acetone, ch3coch3, is 100 mm hg at 281 k. a 6.06e-2 g sample of liquid ch3coch3 is placed in a closed, evacuated 360. ml container at a temperature of 281 k. calculate what the ideal gas pressure would be in the container if all of the liquid acetone evaporated.

Explanation:

According to ideal gas equation, product of pressure and volume equals the product of number of moles, gas constant and temperature.

Mathematically,     PV = nRT

where          P = pressure,               V = volume

                  n = no. of moles,         R = gas constant = 0.0821 atm L/mol

                   T = temperature

Since, it is known that number of moles equal mass divided by molar mass.

Hence, number of moles of given sample of acetone are as follows.

              No. of moles =

                                    =  

                                    = mole

Therefore, putting the values in ideal gas equation as follows.

                         PV = nRT

                           = 0.359 atm

In 1 atm equal to 760 mm Hg. So, convert 0.359 atm into mm Hg as follows.

                       = 272.84 mm Hg

Hence, pressure of the ideal gas will be 100 mm Hg + 272.84 mm Hg = 372.84 mm Hg

Thus, we can conclude that the ideal gas pressure in the container if all of the liquid acetone evaporated is 372.84 mm Hg.

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explanation:

covalent bonds

consist of pairs of electrons shared by two atoms, and bind the atoms to fixed orientation and requre high energies to break them

ionic bonds

when two atoms differ considerably in their electronegativity, then one of the atoms will lose its electron to the other atom. this results in a positively charged ion(cation) and a negatively charged ion (anion)

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