2 Questions: 29 & 31
29. Above which beaker is the vapor pressure of methanol the greatest?
A. Beaker I
B. Beaker II
C. Beaker III
D. The vapor pressure of methanol is the same above all 3 beakers
Correct answer: B (highlight to show correct answer)
Passage Info.
All beakers are sealed.
Beaker 1 contains: 50g methanol and 50g ethanol
Beaker 2 contains: 50ml methanol and 50 ml ethanol
Beaker 3 contains: 1 mole methanol and 1 mole ethanol
Density of methanol: .7914g/ml (mw = 32; bp = 56 degrees C)
Density of ethanol: .7893g/ml (mw = 46; bp = 79 degrees C)
Answer Key: The solution with the greatest mole fraction of methanol has the highest vapor pressure of methanol. Methanol has the lower molecular mass between ethanol and methanol, so beaker 1 has more moles of methanol than ethanol. This means that beaker 1 will exhibit a higher vapor pressure due to methanol than beaker 3. Because the density of methanol is greater than the density of ethanol, beaker 2 with equal volume quantities of methanol and ethanol has more methanol by mass than ethanol by mass. The mole fraction of methanol in beaker 2 is even greater than the mole fraction of ethanol in beaker 1. The highest vapor pressure of methanol is therefore above beaker 2.
Can anyone calculate step by step?
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Question # 31 below
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31. During the first minute of evaporation, before equilibrium is established and the temperature changes to any significant degree, what is observed for the solution in beaker 3?
C. ...rate of vaporization increases
D. ...rate of vaporization decreases
Highlight for answer: D - now my question is why doesn't rate increase before decreasing
Please explain. I had this one backwards.
29. Above which beaker is the vapor pressure of methanol the greatest?
A. Beaker I
B. Beaker II
C. Beaker III
D. The vapor pressure of methanol is the same above all 3 beakers
Correct answer: B (highlight to show correct answer)
Passage Info.
All beakers are sealed.
Beaker 1 contains: 50g methanol and 50g ethanol
Beaker 2 contains: 50ml methanol and 50 ml ethanol
Beaker 3 contains: 1 mole methanol and 1 mole ethanol
Density of methanol: .7914g/ml (mw = 32; bp = 56 degrees C)
Density of ethanol: .7893g/ml (mw = 46; bp = 79 degrees C)
Answer Key: The solution with the greatest mole fraction of methanol has the highest vapor pressure of methanol. Methanol has the lower molecular mass between ethanol and methanol, so beaker 1 has more moles of methanol than ethanol. This means that beaker 1 will exhibit a higher vapor pressure due to methanol than beaker 3. Because the density of methanol is greater than the density of ethanol, beaker 2 with equal volume quantities of methanol and ethanol has more methanol by mass than ethanol by mass. The mole fraction of methanol in beaker 2 is even greater than the mole fraction of ethanol in beaker 1. The highest vapor pressure of methanol is therefore above beaker 2.
Can anyone calculate step by step?
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Question # 31 below
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31. During the first minute of evaporation, before equilibrium is established and the temperature changes to any significant degree, what is observed for the solution in beaker 3?
C. ...rate of vaporization increases
D. ...rate of vaporization decreases
Highlight for answer: D - now my question is why doesn't rate increase before decreasing
Please explain. I had this one backwards.
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