The expected freezing point of L i F solution has to be determined. Concept introduction: Colligative properties: Properties of solutions which having influence on the concentration of the solute in it. Colligative properties are, Decrease in the vapor pressure Increase in the boiling point Decline in the freezing point Osmotic pressure Decline in the freezing point is huge when solute is an electrolyte than when solute is nonelectrolyte. Therefore, change in freezing point is calculated by using the equation, Δ T f p = K f p m s o l u t e i where, K f p is the molal freezing point depression constant. i is van’t Hoff factor van’t Hoff factor, i : it is the relation between change in in freezing point measured and change in in freezing point calculated. It indicates the total number of ions that are produced. Molality (m): Molality is the number of moles of solute present in one kilogram of solvent. Molality (m) = Number of moles of solute 1kg of solvent

Question

Part II. Given two isomers: 2-methylpentane (A) and 2,2-dimethyl butane (B) answer the following: (a) match structures of isomers given their mass spectra below (spectra A and spectra B) (b) Draw the fragments given the following prominent peaks from each spectrum: Spectra A m/2 =43 and 1/2-57 spectra B m/2 = 43 (c) why is 1/2=57 peak in spectrum A more intense compared to the same peak in spectrum B. Relative abundance Relative abundance 100 A 50 29 29 0 10 -0 -0 100 B 50 720 30 41 43 57 71 4-0 40 50 60 70 m/z 43 57 8-0 m/z = 86 M 90 100 71 m/z = 86 M -O 0 10 20 30 40 50 60 70 80 -88 m/z 90 100

Answer 1

Question

Chapter 13, Problem 47PS

Interpretation Introduction

Interpretation: The expected freezing point of LiFsolution has to be determined.

Concept introduction:

Colligative properties: Properties of solutions which having influence on the concentration of the solute in it. Colligative properties are,

Decrease in the vapor pressure

Increase in the boiling point

Decline in the freezing point

Osmotic pressure

Decline in the freezing point is huge when solute is an electrolyte than when solute is nonelectrolyte. Therefore, change in freezing point is calculated by using the equation,

ΔTfp = Kfp msolutei

where,

Kfp is the molal freezing point depression constant.

i is van’t Hoff factor

van’t Hoff factor, i: it is the relation between change in in freezing point measured and change in in freezing point calculated. It indicates the total number of ions that are produced.

Molality (m): Molality is the number of moles of solute present in one kilogram of solvent.

Molality (m) =Number of moles of solute1kg of solvent

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