A solution of chloroform (CHCl3) and acetone((CH3)2CO) exhibits a negative deviation from Raoult's law. This result implies that
: W. chloroform-chloroform and acetone-acetone interactions are stronger than chloroform-acetone interactions. X. chloroform-chloroform and acetone-acetone interactions are weaker than chloroform-acetone interactions. Y. acetone-acetone interactions are stronger than chloroform-chloroform interactions. Z. acetone-acetone interactions are weaker than chloroform-chloroform interactions.
The answer is W. chloroform-chloroform and acetone-acetone interactions are stronger than chloroform-acetone interactions. This is because the bond between acetone-acetone is a dipole-dipole interactions and chloroform-chloroform dipole-dipole compared to the weaker hydrogen-bonding between acetone-chloroform.
It turns out that this hydrogen-bonding happens to be stronger the original dipole-dipole forces, so this shows NEGATIVE DEVIATION from Raoult's law.
Chloroform Chloroform and acetone acetone interactions are stronger than chloroform acetone interactions.
Explanation:
When chloroform and acetone mixed together, it will form a solution with negative deviation from Raoult's law because chloroform form hydrogen bond with acetone molecules. If a vapour mixture is lower that what is expected, negative deviation arises.
If you apply white light and it reflects only red, you see it red, all the other wavelentghs absorbed. If it reflects all wavelength (i think listed all red-orange....) then it should be white.
