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For a miscible system and and PT = PA + PB PA = XAPO XA= molA mola + molB This means that the total vapor pressure is dependent on the mole fraction (X) of each component. Po is the vapor pressure of a pure liquid at a given temperature. This is something you would look up or be given in a table of values. The moles of each component can be calculated based on the volume used, density, and molar mass. a. Calculate the total vapor pressure of a system made of 10 mL water and 5 mL methyl salicylate at 108°C. Pwater = 1.0512 atm and Pms = 0.0238 atm at this temperature. Assume the system is miscible. Is this system boiling (assuming it is miscible?) at 108°C? b.

For a miscible system and and PT = PA + PB PA = XAPO XA= molA mola + molB This means that the total vapor pressure is dependent on the mole fraction (X) of each component. Po is the vapor pressure of a pure liquid at a given temperature. This is something you would look up or be given in a table of values. The moles of each component can be calculated based on the volume used, density, and molar mass. a. Calculate the total vapor pressure of a system made of 10 mL water and 5 mL methyl salicylate at 108°C. Pwater = 1.0512 atm and Pms = 0.0238 atm at this temperature. Assume the system is miscible. Is this system boiling (assuming it is miscible?) at 108°C? b.

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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Answer question 3 part A and B please!!

Conceptual Questions: 1. Explain what the reading on the thermometer will do (change, stay the same, etc.) while the liquid is boiling and collecting in the receiving flask at a steady rate. Include why this happens. the heat thats being applied to the liquid is used to convert from liquid-gas instead of increasing the temp of liquid Data: 1. What was the temperature at which you first started collecting liquid? 96.9°C (ours didn't distill) 2. What was your experimental boiling point for your mixture? 30°C Distillation Post Lab Analysis: 1. Look at the boiling points for methyl salicylate and water. A miscible system would have a boiling point between those two temperatures based on the ratio of components. a. are water and methyl salicylate miscible? Yes (a little/slightly) b. was the boiling point below, between, or above the two literature boiling points? Below 2. Raoult's Law states that a liquid will boil when the vapor pressure of the liquid is equal to (or greater than) the external pressure. In an open system, this is atmospheric pressure; in a closed system, it is the applied pressure a. was your simple distillation an open or a closed system? Open 3. For a miscible system SYCHIOL PT = PA + PB PA = XAPO and and XA = mola mola + molB This means that the total vapor pressure is dependent on the mole fraction (X) of each component. Pº is the vapor pressure of a pure liquid at a given temperature. This is something you would look up or be given in a table of values. The moles of each component can be calculated based on the volume used, density, and molar mass. a. Calculate the total vapor pressure of a system made of 10 mL water and 5 mL methyl salicylate at 108°C. Pwater = 1.0512 atm and Pms = 0.0238 atm at this temperature. Assume the system is miscible. b. Is this system boiling (assuming it is miscible?) at 108°C? 4. In an immiscible system, the two liquids in the mixture behave as if they are pure liquids, as if they don't "see" each other. X becomes 1 for both components and the equation becomes PT = P + PO This means that for a system of two immiscible liquids, the boiling point will always occur below either of the two pure boiling points. a. Did you observe this behavior with your own results? Reflection: 1. Based on this experience, what are the practical considerations when using a simple distillation for purification? What do you feel are the significant limitations on this technique? What are the potential benefits of a distillation? not able to greatly purify if boiling points are too close Pro: removing inorganic compounds
Transcribed Image Text:Conceptual Questions: 1. Explain what the reading on the thermometer will do (change, stay the same, etc.) while the liquid is boiling and collecting in the receiving flask at a steady rate. Include why this happens. the heat thats being applied to the liquid is used to convert from liquid-gas instead of increasing the temp of liquid Data: 1. What was the temperature at which you first started collecting liquid? 96.9°C (ours didn't distill) 2. What was your experimental boiling point for your mixture? 30°C Distillation Post Lab Analysis: 1. Look at the boiling points for methyl salicylate and water. A miscible system would have a boiling point between those two temperatures based on the ratio of components. a. are water and methyl salicylate miscible? Yes (a little/slightly) b. was the boiling point below, between, or above the two literature boiling points? Below 2. Raoult's Law states that a liquid will boil when the vapor pressure of the liquid is equal to (or greater than) the external pressure. In an open system, this is atmospheric pressure; in a closed system, it is the applied pressure a. was your simple distillation an open or a closed system? Open 3. For a miscible system SYCHIOL PT = PA + PB PA = XAPO and and XA = mola mola + molB This means that the total vapor pressure is dependent on the mole fraction (X) of each component. Pº is the vapor pressure of a pure liquid at a given temperature. This is something you would look up or be given in a table of values. The moles of each component can be calculated based on the volume used, density, and molar mass. a. Calculate the total vapor pressure of a system made of 10 mL water and 5 mL methyl salicylate at 108°C. Pwater = 1.0512 atm and Pms = 0.0238 atm at this temperature. Assume the system is miscible. b. Is this system boiling (assuming it is miscible?) at 108°C? 4. In an immiscible system, the two liquids in the mixture behave as if they are pure liquids, as if they don't "see" each other. X becomes 1 for both components and the equation becomes PT = P + PO This means that for a system of two immiscible liquids, the boiling point will always occur below either of the two pure boiling points. a. Did you observe this behavior with your own results? Reflection: 1. Based on this experience, what are the practical considerations when using a simple distillation for purification? What do you feel are the significant limitations on this technique? What are the potential benefits of a distillation? not able to greatly purify if boiling points are too close Pro: removing inorganic compounds
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