7. A student did a distillation experiment using 40 % aqueous ethanol and presented his result of distillation curve in his lab report as shown below: 100 90 80 70 60 50 40 30 10 20 30 40 Volume Collected (mL) What would be his possible conclusion about his experiment? 1). a good separation of ethanol from water was achieved. 2). the initial distillation temperature was set a little high. 3). the distillation temperature was not well controlled. 4). the concentration of ethanol was too high in the initial solution. 8. What is the main purpose of a fractional column in fractional distillation? 1). to heat the liquid being distilled efficiently 2). to provide more surface area for vapor to condense. 3). to speed up the distillation of the liquid 4). to completely condense the vapor to form a liquid 9. Why is it preferable to allow cold water to enter at the bottom of a water condenser and exit at the top than vice versa? 1). to effectively condense the vapor to form a liquid 2). to allow the water to flow unrestrictedly 3). to separate the liquids being distilled 4). to predict the boiling point of the liquid Temperature (°C)

7. A student did a distillation experiment using 40 % aqueous ethanol and presented his result of distillation curve in his lab report as shown below: 100 90 80 70 60 50 40 30 10 20 30 40 Volume Collected (mL) What would be his possible conclusion about his experiment? 1). a good separation of ethanol from water was achieved. 2). the initial distillation temperature was set a little high. 3). the distillation temperature was not well controlled. 4). the concentration of ethanol was too high in the initial solution. 8. What is the main purpose of a fractional column in fractional distillation? 1). to heat the liquid being distilled efficiently 2). to provide more surface area for vapor to condense. 3). to speed up the distillation of the liquid 4). to completely condense the vapor to form a liquid 9. Why is it preferable to allow cold water to enter at the bottom of a water condenser and exit at the top than vice versa? 1). to effectively condense the vapor to form a liquid 2). to allow the water to flow unrestrictedly 3). to separate the liquids being distilled 4). to predict the boiling point of the liquid Temperature (°C)

Organic Chemistry: A Guided Inquiry

2nd Edition

ISBN:9780618974122

Author:Andrei Straumanis

Publisher:Andrei Straumanis

Chapter4: Polar Bonds, Polar Reactions

Section: Chapter Questions

Problem 7E

See similar textbooks

Similar questions

DATA Note: Use the videos as references except when data is provided here. Table 1. Selection of Recrystallizing Solvent. Solvents Dissolution at room temperature? (+ or −) Dissolution at elevated temperature? (+ or −) Distilled water - - Acetone + n/a 95% ethanol - + Toluene + n/a Solid sample: Naphthalene Table 2. Mass Measurements. Mass, g Sample solid 0.5021 Empty watch glass 35.7602 Watch glass with recrystallized sample 36.2485 Table 3. Melting Point Determination. Temperature, oC Appearance of Sample in Capillary Tube … Solid 78.4 Solid 79.3 Solid with signs of liquid 79.9 Solid, liquid 80.6 Liquid, solid 81.3 Liquid with signs of solid … Liquid Theoretical Melting Point, oC: 80.2°C (176.4°F) QUESTIONS Which solvent should be used as the recrystallizing solvent? Check if your chosen solvent satisfies all characteristics of a good…
Suppose you have an organic sample X that is somewhat soluble in water, even though it issomewhat more soluble in dichloromethane or ether solvents. But if you do a singleextraction, you get only 60% of your material to transfer from the water to the organic layer.How many “washes” would it take to extract over 90% of your organic material extracted fromthe water layer?
3. If both water and your alkene products distill into your collection flask, why might you get two layers? because there is a temperature gradient in the graduated cyclinder because methylcyclohexenes and water are immiscible because methylcyclohexenes and water are miscible
A student in New York City carried ou1t a boiling point determination for cyclohexane {b.p. 81• C) according to the procedure in this laboratory manual. Will this student's observed boiling point be the same as the value obtained by another student in Denver, Co'lorado.{Nicknamed the "Mile-High City" due to its high elevation)? Will it be lower or higher? Ex plain your conclusion.
Naphthalene, C10H8 is insoluble in water but sublimes easily when heated. How could you separate a mixture of naphthalene and NaCl? Suggest two different methods. asap
Given the following statements, which would be the ideal solvent to use for recrystallization of this compound? Why? Compound X is soluble in both cold ethyl acetate and hot ethyl acetate. Compound X is insoluble in cold benzene but soluble in hot benzene. Compound X is insoluble in both cold hexanes and hot hexanes. Compound X is insoluble in cold ethanol but soluble in hot ethanol.
True or False. It is very important to regulate the temperature of the heating mantle so that the distillation occurs at a rate of about 1 drop per 2 seconds. Explain why?
If you use toluene as a solvent for recrystallization of biphenyl, what is the most likely reason it would be unsuccessful? a. The boiling point of toluene is too low. b. Biphenyl will not dissolve in the non-polar toluene. c. Biphenyl is too soluble in the similarly structured toluene solvent, and will be hard to recover after recrystallization. d. Toluene is a polar solvent.
Nitroethylene, HyC = CHNO, is a sensitive compound that must be prepared with great care. Attempted purification of nitroethylene by distillation often results in low recovery of product and a white coating on the inner walls of the distillation apparatus. Explain.
Which of the ff is not true about recrystallization? a. acetanalide recrystallized only at cold temp b. congo red stain is removed by using animal charcoal c. acetanalide can be dissolved in hot h20
The separation and purification processes given below and the method used against them are given. Which or which of these pairings are correct? I. Brewing of tea - ExtractionII. Purification of water impurities - ChromatographyIII. Separation of olive pomace from olive oil while producing olive oil-DecantationIV.Petroleum fractions obtaining - Ordinary distillationV. Obtaining essential oils and using them in perfume making - Water-steam distillation
What is done if the solid contains a colored impurity? Know the proper funnels and equipment to use. What is done if a solid impurity remains after your desired compound is dissolved in asolvent? When do you read the temperature to determine the boiling point of a liquid whendoing microscale boiling point determination