A solution of methanol and water has a mole fraction of water of 0.312 and a total vapor pressure of 211 torr at 39.9 ∘C. The vapor pressures of pure methan ol and pure water at this temperature are 256 torr and 55.3 torr, respectively. ls the solution ideal? If not, what can you say about the relative strengths of the solute-solvent interactions compared to the solute-solute and solvent-solvent interactions?
Answers
Answer:
Weaker
Explanation:
The strategy here is to use Raoult´s law to calculate the theoretical vapor pressure for the concentrations given and compare it with the experimental value of 211 torr.
Raoult´s law tell us that for a binary solution
P total = partial pressure A + partial pressure B = Xa PºA + Xb PºB
where Xa and Xb are the mol fractions, and PºA and PºB are the vapor pressures of pure A and pure B, respectively
For the solution in question we have
Ptotal = 0.312 x 55.3 torr + ( 1- 0.312 ) x 256 torr ( XA + XB = 1 )
Ptotal = 193 torr
Since experimentally, the total vapor pressure is 211 and our theoretical value is smaller ( 193 torr ), we can conclude the interactions solute-solvent are weaker compared to the solute-solute and solvent-solvent interactions.
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Answers
Explanation:
The given data is as follows.
V = 250.0 ml, T = 58^{o}C = 58 + 273 = 331 K
n = 2.48 moles, P = ? , R = 0.082 atm L /K mol
Therefore, calculate the pressure using ideal gas equation as follows.
PV = nRT
P =
=
= 0.269 atm
Thus, we can conclude that pressure of the given gas is 0.269 atm.
R = 0.082 atm
V = 250.0 mL / 1000 = 0.25 L
P = n x R x T / V
P = 2.48 x 0.082 x 331.15 / 0.25
P = 67.342 / 0.25
P = 269.368 atm
hope this helps!
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Answer:
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Answers
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Answers
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Learn more about electron configuration here: brainly.com/question/11316046
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Answers
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Explanation:
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