Two unknown molecular compounds were being studied. A solution containing 5.00 g of compound A in 100. g of water froze at a lower temperature than a solution containing 5.00 g of compound B in 100. g of water. Which compound has the greater molar mass

Compound B has greater molar mass.

Explanation:

The depression in freezing point is given by ;

..[1]

Where:

i = van't Hoff factor

= Molal depression constant

m = molality of the solution

According to question , solution with 5.00 g of A in 100.0 grams of water froze at at lower temperature than solution with 5.00 g of B in 100.0 grams of water.

The depression in freezing point of solution with A solute:

Molar mass of A =

The depression in freezing point of solution with B solute:

Molar mass of B =

As we can see in [1] , that depression in freezing point is inversely related to molar mass of the solute.

This means compound B has greater molar mass than compound A,

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