What are the boiling point and freezing point of a 0.516 m aqueous solution of any nonvolatile, nonelectrolyte solute?

Explanation:

1. Boling point

The boiling point of a solvent will increase when a solute is added. The boiling point elevation is a colligative property.

When a nonvolatile, nonelectrolyte solute is added to a solvent, the increase of the boiling point may be calculated using the formula:

Where m is the molality and Kb is the the molal boiling point constant (for water, Kb = 0.512ºC/m ).

Substitute and compute:

Hence, add the increase in the boiling point to the normal boiling point of water: 100.000ºC

2. Freezing point

The freezing point of a solve will decrease when a solute is added. The depression on the freezing point is another colligative property.

When a nonvolatile, nonelectrolyte solute is added to a solvent, the depression of the boiling point may be calculated using the formula:

Where m is the molality and Kf is the the molal freezing point constant (for water, Kf = 1.86 ºC/m ).

Substitute and compute:

Subtract the decrease on the freezing point from the normal freezing point of water: 0.000ºC

more info ? ? i don't understand what the question is

explanation:

the electronic configuration of an atom with eight electrons is 1s²2s²2p⁴. the orbital diagrams are shown in the figure.

as per the hunds rule:

1. electrons tend to avoid being in the same orbital as per as practicable.

2. electrons in different orbitals of the same energy will have their spin parallel.

this can be illustrated from the multiplicity of the orbitals of the atom. as there are four electrons in the p orbital and p orbital has 3 sub-shells. the electrons can be fed in different ways as shown in the figure but the correct orbital diagram will be as per the hunds rule.