I have no idea how to do these!!!! help please!!! A solution is prepared by mixi
ID: 822535 • Letter: I
Question
I have no idea how to do these!!!! help please!!!A solution is prepared by mixing 0.0200 mol CH2Cl2 and 0.0500 mol of CH2Br2 at 25 I have no idea how to do these!!!! help please!!!
A solution is prepared by mixing 0.0200 mol CH2Cl2 and 0.0500 mol of CH2Br2 at 25 I have no idea how to do these!!!! help please!!!
A solution is prepared by mixing 0.0200 mol CH2Cl2 and 0.0500 mol of CH2Br2 at 25 I have no idea how to do these!!!! help please!!!
A solution is prepared by mixing 0.0200 mol CH2Cl2 and 0.0500 mol of CH2Br2 at 25 I have no idea how to do these!!!! help please!!!
A solution is prepared by mixing 0.0200 mol CH2Cl2 and 0.0500 mol of CH2Br2 at 25
Explanation / Answer
Total mol in solution = 0.0200 + 0.0500 = 0.0700 mol
?(CH2Cl2) =
0.0200/0.0700 = 0.2857;
?(CH2Br2) =
0.0500/0.0700 = 0.71428
P(CH2Cl2) = ? x P(pure solvent) = 0.2857 x 133 = 38 torr.
P(CH2Br2) = ? x P(pure solvent) = 0.7143 x 11.4 = 8.143 torr.
P(total) = P(CH2Cl2) + P(CH2Br2) = 38 + 8.143 = 46.143 torr
Mole fraction of the substance in vapor phase can be calculated using the relationship of the ideal gas law for
each pressure (since gases in a mixture must occupy the same volume and will exist at the same temperature, the
ratio of the partial pressure of one gas to the total pressure of the mixture is the mole fraction of that gas in the
vapor phase):
?(CH2Cl2) = n(CH2Cl2)/n(total) = P(CH2Cl2)/P(total) = 38/46.143 = 0.8235
?(CH2Br2) = n(CH2Br2)/n(total) =P(CH2Br2)P(total) = 8.143/46.143 = 0.1764