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Trava [24]
3 years ago
13

When two volatile liquids (X and Y) are mixed, the solution process involves 1. breaking the intermolecular X---X and Y---Y attr

actions, and 2. forming new X---Y attractions.
Complete this table describing how the relative strengths of these attractive forces affect vapor pressure and enthalpy of solution.
1. X---X, Y---Y, and X---Y are equal
2. X---Y is strongest
3. X---Y is weakest
Raoult's law deviations & deltaHsoln

Chemistry
2 answers:
Misha Larkins [42]3 years ago
6 0

1. X --- X, Y --- Y, and X --- Y are equal

delta H = 0 and Raoult's Deviation = 0

2. X --- Y is the strongest

delta H = - and Raoult's Deviation = negative

3. X --- Y is the weakest

delta H = + and Raoult's Deviation = positive

<h3>Further explanation</h3>

In mixing the two solutions, it will require energy to break the attraction of each solution and create a new attraction that produces energy.

If both are equal then there will be no heat released or received so that the delta H solution is 0, which indicates that the solution is ideal

Raoult's Law states that the magnitude of the vapor pressure of a solution is proportional to the mole fraction of the solvent and the vapor pressure of the pure solvent

So the vapor pressure of a component depends on the mole fraction of that component in the solution

Can be formulated:

\large{\boxed{\bold{P~=~Po.X_{solvent}}}}

P = solution vapor pressure

X = mole fraction

Po = vapor pressure of the pure solvent

This solution that can fulfill Raoult's law is said to be the ideal solution

So the ideal solution occurs if the  attractive  force between the molecules is the same as the attractive  force of each solute and solvent

But not all solutions have ideal properties, so this solution has a deviation or deviation from Raoult's law

There are 2 kinds of deviations from Raoult's Law,

  • 1. Positive deviation

Occurs if the attractive strength between each mixture forming agent is stronger than the  attractive in the mixture

(X-X, Y-Y> X-Y)

This deviation produces a positive enthalpy of solution (ΔH +) which is endothermic so that there is an increase in the volume of the mixture

  • 2. Negative deviation

Occurs if the attractive force in the mixture is stronger than the attractive force of each substance

(X-Y> X-X, Y-Y)

This deviation produces an enthalpy of a negative value solution (ΔH -) which is exothermic so that there is a reduction in the volume of the mixture

So that at a positive deviation, for example, the vapor pressure of the mixed solution will be greater than the initial vapor pressure value

So if

1. X --- X, Y --- Y, and X --- Y are equal

then the value ΔH = 0 and Raoult's Deviation = 0, indicating that the solution is ideal / there is no deviation from Raoult's Law

2. X --- Y is the strongest

then the value ΔH = - and the deviation of Raoult = negative

3. X --- Y is the weakest

then the value ΔH = + and Raoult's Deviation = positive

<h3>Learn more</h3>

Raoult's law

brainly.com/question/10165688

Deviation from Raoult's Law

brainly.com/question/13004684

The vapor pressure of benzene

brainly.com/question/11102916

Keywords: Raoult's Law, Deviation, Delta H solution, vapor pressure

leonid [27]3 years ago
3 0
Forming the table:

(1)
X---X, Y---Y &<span>X---Y are equal
</span><span>Raoult's Law Deviation: ZERO
</span>DeltaHsoln: ZERO

(2) 
<span>X---Y is strongest
</span><span>Raoult's Law Deviation: NEGATIVE
</span><span>DeltaHsoln: NEGATIVE
</span>
(3)
X---Y is weakest
<span>Raoult's Law Deviation: POSITIVE
</span><span>DeltaHsoln: POSITIVE</span>

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Mass of O = Mass of compound - Mass of C - Mass of H = (1.500 – 0.5568 – 0.077 81) g = 0.8654 g O

=====

2. Convert these masses to moles.

Moles  C = 0.5568  × 1/12.01  = 0.046 36

Moles H = 0.077 81 × 1/1.008 = 0.077 19

Moles O = 0.8654   × 1/16.00 = 0.054 09

=====

3. Find the molar ratios.

Moles  C = 0.046 36/0.046 36 = 1

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======

4. Multiply the ratios by a number to make them close to integers

C  = 1        × 6 = 6

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=====

5. Round the ratios to integers

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=====

6. Write the empirical formula

The empirical formula is C₆H₁₀O₇.

=======

7. Calculate the empirical formula mass

C₆H₁₀O₇ = 6×12.01 + 10×1.008 + 7×16.00

C₆H₁₀O₇ = 72.01 + 10.08+ 112.0

C₆H₁₀O₇ = 194.09

=====

8. Divide the molecular mass by the empirical formula mass.  

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=====

9. Determine the molecular formula

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