Example For each of the following solutions, would you...

Example For each of the following solutions, would you expect it to be relatively ideal (with respect to Raoult’s Law), show a positive deviation, or show a negative deviation? a) Hexane (C6H14) and chloroform (CHCl3) b) Ethyl alcohol (C2H5OH) and water c) Hexane (C6H14) and octane (C8H18)

Transcript

00:01 So we have to predict the vapor pressure with the help of rolflow application here.

00:07 So first of all we have given hexane and chloroform.

00:20 So hexane is c6h14 and chloroform is chcl3.

00:31 Now this hexane is non -polar it do not have polarity there is no dipole moment then we have chloroform this is polar in nature okay so whenever there is a interaction between non -polar and polar that will be weak okay so this will lead to weak interactions weak interactions known polar plus polar leads to weak interactions between solute and solvent hence leads to positive deviation from rawls law okay, law and if there is positive deviation from drought's law hence okay so this is what we have to do here only okay we do not need to predict here about vapor pressure so this the answer for first one is positive deviation from route law okay now we have second one b part we have ethyl alcohol and water.

02:40 So now ethyl alcohol is c2h5 -oh -h ethanol, okay, and water is h2o.

02:55 Now both are polar, okay? but let me draw the diagram.

03:04 So here since we have c2h5 -oh -h, so there is interaction of hydrogen with electronegative oxygen atom.

03:14 Here we have water molecule and there is interaction of hydrogen atom with electronegative atom whenever there is a interaction of hydrogen atom with electrone negative atom such as oxygen nitrogen fluorine so then we say that we have hydrogen bonding in that case when we have different molecules okay this hydrogen bonding if this interaction of hydrogen and electronegative atom is present between different molecules then that is called intermolecular hydrogen bonding okay hydrogen bonding between different molecules so this molecule has intermolecular hydrogen bonding and hence the interaction between solute and solvent that is very strong right so intermolecular hydrogen bonding between solute and solvent and solvent okay which let me add it here so these whenever there is intermolecular hydrogen bonding such interactions are very strong okay strong interactions due to intermolecular hydrogen bonding between solute and solvent okay hence this leads to negative deviation from lovl's law.

05:28 So the answer is negative deviation.

05:34 Now c part we have given hexane and octane...

Question

Example For each of the following solutions, would you expect it to be relatively ideal (with respect to Raoult’s Law), show a positive deviation, or show a negative deviation? a) Hexane (C6H14) and chloroform (CHCl3) b) Ethyl alcohol (C2H5OH) and water c) Hexane (C6H14) and octane (C8H18)

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