When of alanine are dissolved in of a certain mystery liquid , the freezing point of the solution is lower than the freezing point of pure . on the other hand, when of iron(iii) nitrate are dissolved in the same mass of , the freezing point of the solution is lower than the freezing point of pure . calculate the van't hoff factor for iron(iii) nitrate in . be sure your answer has a unit symbol, if necessary, and round your answer to significant digits.

i = 3,5

Explanation:

There are missing the following values:

132 g Alanine

1150g of X

4,4°C the first freezing point dercreasing

132g of Iron(III) nitrate

5,6°C the second freezing point decreasing.

The freezing point depression is a colligative property that describes the decrease of the freezing point of a solvent on the addition of a non-volatile solute.

The formula is:

ΔT = i kf mb

Where ΔT is freezing point decreasing, i is Van't Hoff factor, kf, is cryoscopic constant and mb is molality of solution.

For alanine Van't Hoff factor is 1 (Ratio between particles in dissolution and before dissolution), molality is:

132g×(1mol/89,09g) = 1,48mol / 1,150kg = 1,29 mol/kg

Replacing:

4,4K = 1 kf 1,29mol/kg

kf = 3,41 K·kg/mol

Now, for Iron(III) nitrate molality is:

132g×(1mol/241,86g) = 0,546mol / 1,150kg = 0,475 mol/kg

Replacing:

5,6K = i×3,41 K·kg/mol×0,475 mol/kg

i = 3,5

I hope it helps!

a polar bond is formed when electrons are shared unevenly between atoms

a). in this case, dh> 0 and sd> 0. if t becomes larger, the term "-tds" will become more negative. at some point, it is possible that -dts will be more negative than the dh is positive, and the reaction will become spontaneous. this is probably the correct answer, but you should look at all of the other possibilities and make sure of that.