A, because it is one of only a few on the periodic table that are liquid at room temperature and normal pressure
Answer:
(B)
Explanation:
The colligative properties of any given solution are properties that are dependent on the concentration of the molecules or ions of the solute in the solution, and not on the type or identity of that solute. Examples of colligative properties:
1. Lowering of vapour pressure
2. Elevation of boiling point,
3. Depression of freezing point and
4. Osmotic pressure
(A) is not a colligative property because the scenario talks about the freezing point of a pure solvent and not a solution.
(C) is not a colligative property because the solutions being compared are completely different (the solutes are different).
(B) is a colligative property because it talks about the freezing point of a solution
Answer: The molar mass of is 67.81 g/mol
Explanation:
Molar mass is defined as the mass in grams of 1 mole of a substance.
S.I Unit of Molar mass is gram per mole and it is represented as g/mol.
Atomic Mass of Boron (B) = 10.81 g
Atomic Mass of Flourine (F) = 18.99 g
Molecular mass of = 1 (10.81)+3(18.99) g = 67.81 g
Thus molar mass of is 67.81 g/mol
Answer:
The substance is a mixture
Explanation:
The question lets us know that when solvent X was used as the mobile phase, we obtained only one spot. This may deceive us into thinking that the substance is pure since a pure substance has only one spot on a chromatogram.
However, the same substance yields three spots with solvent Y. This shows that the unknown sample is a mixture of substances and solvent X was unable to fully separate the mixture.