An aqueous solution containing 17.5 g of an unknown molecular compound in 100.g water was found to have a freezing point of-1.8°C. Calculate the molar mass of this unknown compound. You can use the following steps to solve this problem. Show your work. What is the freezing point change (AT) from pure water? The freezing point of water is 0.0°C a. What is the freezing point depression constant (K of water? moles of solute b. What is the molality of the solution? (m= kg of solvent Horizontal (Value) Axis Major Gridlines moles of solute kg of solvent*Kr) c. S olve the moles of the solute . d. (A7-mxKf- Knowing the mass of the compound, and the moles of the compound, solve the molar mass of the compound.

The answer to your question is 178.6 g

Explanation:

Data

ΔT = 1.8 °C

mass = 17.5 g

mass of water = 100 g

Kc = 1.86

Process

1.- Calculate the molality using the following formula

    ΔTc = mKc

solve for m

    m = ΔTc/Kc

substitution

     m = 1.8/1.86

result

     m = 0.968

2.- Calculate the number of moles

    m = # of moles/kg of solvent

kg of solvent = 0.1 kg

     # of moles = m x kg of solvent

     # of moles = 0.968 x 0.1

     # of moles = 0.0968

3.- Calculate the molar mass

        x g molar mass 1 mol

       17.5 g                   0.0968 moles

       x = (1 x 17.5)/0.0968

      x = 178.6 g

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.