At a given temperature, the vapor pressure of pure acetone (ch3coch3, 58.00 g/mol) is 342 torr. at the same temperature, the vapor pressure of pure chloroform (chcl3, 119.35 g/mol) is 230 torr. consider a solution containing 23.2 g of acetone and 73.8 g of chloroform. calculate the total vapor pressure above the solution (in torr to 0 decimal places)

Total vapor pressure = 274 torr

Explanation:

According to Raoult´s law, the partial  pressure of a volatile compound in a mixture of two volatile components is

PA = Xa PºA where PA = partial pressure of component A

                                XA = mole fraction of A= mol A / (molA + Mol B)

                                PºA = vapor pressure of pure A

and the total pressure will be given by the sum of the partial pressures.

mol CH3COCH3 = 23.2 g/ 58 g/mol = 0.40 mol

mol CHCl3 = 73.8 g/ 119.35 g/mol = 0.62 mol

total mol = 0.40 mol +0.62 mol =  1.02 mol

XCH3COCH3  = 0.40 mol / 1.02 mol = 0.39

XCHCl3 = 0.62 mol / 1.02 mol = 0.61

PCH3COCH3 = 0.39 x 342 torr = 133.4 torr

PCHCl3 = 0.61 x 230 torr = 140.3 torr

Ptotal = 133.4 torr + 140.3 torr = 274 torr

sodium (na), for example, has one electron in its valence shell. this is an unstable state because that valence shell needs eight electrons to be full. in order to fill its valence shell, find a way to add seven electrons to its valence shell

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