Chemistry High School

A certain liquid X has a normal boiling point of 121.70 "C and a boiling point elovation constant K i
​
=131 "C kg mol 1 a solution is prepared by. dissolving some olycine (C 2
​
H 3
​
NO 2
​
) in 800 . g of X. This solution boils at 123.7 C. Calculate the mass of C 2
​
H 5
​
NO that was dissolved. Round your answer to 2 significant digits.

Answers

Answer 1

The Mass of glycine = Molality × Molar mass × Mass of solvent=0.0153 × 75 × 800=91.35 g ≈ 91 g Mass of C2H5NO2 that was dissolved is approximately 91 g.

Hence, the correct option is 91.

Given,Normal boiling point of liquid X, T1

= 121.7°C Boiling point elevation constant, Kb

= 131°C kg mol-1 Mass of solvent, w2

= 800 g Boiling point of solution, T2

= 123.7°C

Now, Boiling point elevation is given by, ΔTb

= T2 - T1ΔTb

= 123.7 - 121.7ΔTb

= 2°C The boiling point elevation is given by,ΔTb

= Kb × bΔTb/Kb

= b Molality (b) of solution, b

= ΔTb/Kb

=2/131

=0.0153 mol/kg

The molality of the solution is 0.0153 mol/kg.Molar mass of glycine, C2H3NO2

= 75 g/mol

We need to calculate the mass of glycine dissolved in the solution.

The Mass of glycine

= Molality × Molar mass × Mass of solvent

=0.0153 × 75 × 800

=91.35 g ≈ 91 g Mass of C2H5NO2 that was dissolved is approximately 91 g.

Hence, the correct option is 91.

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