The experimental procedure to test the hypothesis that solute blocking of solvent vaporization is not the reason that solutions have lower vapor pressures than the pure solvents is to be determined. Concept introduction: According to Raoult’s law, the vapor pressure of a solution is equal to the product of the mole fraction and the vapor pressure of the pure solvent. The expression of Raoult’s law is, P solution = x solvent P ∘ solvent

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Answer 1

Question

Chapter 13, Problem 1DE

Interpretation Introduction

Interpretation: The experimental procedure to test the hypothesis that solute blocking of solvent vaporization is not the reason that solutions have lower vapor pressures than the pure solvents is to be determined.

Concept introduction: According to Raoult’s law, the vapor pressure of a solution is equal to the product of the mole fraction and the vapor pressure of the pure solvent.
The expression of Raoult’s law is,
Psolution=xsolvent P∘solvent

Expert Solution & Answer

Answer to Problem 1DE

Solution: The interaction between solute and solvent and the number of solute particles are responsible for the lower vapor pressures of the solution than the pure solvents.

Explanation of Solution

According to Raoult’s law, the vapor pressure of a solution is equal to the product of the mole fraction and the vapor pressure of the pure solvent.
The expression of Raoult’s law is,

Psolution=xsolvent P∘solvent

When a solute is added to a solution, the vapor pressure of the solution decreases because on addition of solute, the gap between the solvent molecules gets filled. Hence, on the surface of solution, the number of solvent molecule is less as compared to the pure solvent. This indicates that the number of solvent molecule enter into the gas phase is less and due to this there is a decrease in vapor pressure.
Using the Raoult’s law, the lowering of vapor pressure can be explained.
Assume two sealed containers, one is for pure solvent and other is for solution. The equilibrium stage arises when the number of molecules striking on the surface of the molecule becomes equal to the number of molecules going to the gas phase. On addition of solute, half of the surface of the solution is occupied by the solute and half of the surface is occupied by solvent molecules.

Study Guide for Chemistry: The Central Science, Chapter 13, Problem 1DE

Figure 1

The vapor pressure of the solution depends upon the number of solvent molecule present on the surface of the solution. As the number of solute molecule increases, the number of solvent molecule present on the surface of solution decreases, now lesser number of solvent molecules is present to go in gas phase. Hence, the vapor pressure of the solution decreases.

The attraction between molecules of solvent with solute also plays an important role in lowering the vapor pressure. If there is a strong attraction between the solute and solvent, than the solvent molecule try to remain in the solution rather than escaping from it. Due to this, lowering of vapor pressure occurs because now there are less number of solvent molecule in vapor phase.

Another important factor is that, number of molecules present in the solution is not important rather than this number of solute particles present in the solution is important.
More the number of solute particles, low will be the vapor pressure.

Conclusion

The interaction between solute and solvent and the number of solute particles are responsible for the lower vapor pressures of the solution than the pure solvents.

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eks.com/aleksogi/x/sl.exe/1o_u-IgNslkr7j8P3jH-IQs_pBanHhvTCeeBZbufuBYTI0Hz7m7D3ZS17Hd6m-HIl6n52njJN-TXdQA2X9yID-1SWQJTgnjARg30 111 States of Matter Understanding conceptual components of the enthalpy of solution 0/5 Ge A small amount of acetonitrile (CH, CN) is dissolved in a large amount of water. Imagine separating this process into the four stages sketched below. (These sketches show only a portion of the substances, so you can see the density and distribution of atoms and molecules in them.) CH,CN H₂O B 88 C Use these sketches to answer the questions in the table below. The enthalpy of solution AH is negative soln when CH3CN dissolves in water. Use this information to list the stages in order of increasing enthalpy. Would heat be absorbed or released if the system moved from Stage C to D? What force would oppose or favor the system moving from Stage C to D? Check all that apply. 1 absorbed O released neither absorbed nor released. none O ionic bonding force covalent bonding force…

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Answer 2

Question

Chapter 13, Problem 1DE

Interpretation Introduction

Interpretation: The experimental procedure to test the hypothesis that solute blocking of solvent vaporization is not the reason that solutions have lower vapor pressures than the pure solvents is to be determined.

Concept introduction: According to Raoult’s law, the vapor pressure of a solution is equal to the product of the mole fraction and the vapor pressure of the pure solvent.
The expression of Raoult’s law is,
Psolution=xsolvent P∘solvent

Expert Solution & Answer

Answer to Problem 1DE

Solution: The interaction between solute and solvent and the number of solute particles are responsible for the lower vapor pressures of the solution than the pure solvents.

Explanation of Solution

According to Raoult’s law, the vapor pressure of a solution is equal to the product of the mole fraction and the vapor pressure of the pure solvent.
The expression of Raoult’s law is,

Psolution=xsolvent P∘solvent

When a solute is added to a solution, the vapor pressure of the solution decreases because on addition of solute, the gap between the solvent molecules gets filled. Hence, on the surface of solution, the number of solvent molecule is less as compared to the pure solvent. This indicates that the number of solvent molecule enter into the gas phase is less and due to this there is a decrease in vapor pressure.
Using the Raoult’s law, the lowering of vapor pressure can be explained.
Assume two sealed containers, one is for pure solvent and other is for solution. The equilibrium stage arises when the number of molecules striking on the surface of the molecule becomes equal to the number of molecules going to the gas phase. On addition of solute, half of the surface of the solution is occupied by the solute and half of the surface is occupied by solvent molecules.

Study Guide for Chemistry: The Central Science, Chapter 13, Problem 1DE

Figure 1

The vapor pressure of the solution depends upon the number of solvent molecule present on the surface of the solution. As the number of solute molecule increases, the number of solvent molecule present on the surface of solution decreases, now lesser number of solvent molecules is present to go in gas phase. Hence, the vapor pressure of the solution decreases.

The attraction between molecules of solvent with solute also plays an important role in lowering the vapor pressure. If there is a strong attraction between the solute and solvent, than the solvent molecule try to remain in the solution rather than escaping from it. Due to this, lowering of vapor pressure occurs because now there are less number of solvent molecule in vapor phase.

Another important factor is that, number of molecules present in the solution is not important rather than this number of solute particles present in the solution is important.
More the number of solute particles, low will be the vapor pressure.

Conclusion

The interaction between solute and solvent and the number of solute particles are responsible for the lower vapor pressures of the solution than the pure solvents.

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Answer 3

Question

Chapter 13, Problem 1DE

Interpretation Introduction

Interpretation: The experimental procedure to test the hypothesis that solute blocking of solvent vaporization is not the reason that solutions have lower vapor pressures than the pure solvents is to be determined.

Concept introduction: According to Raoult’s law, the vapor pressure of a solution is equal to the product of the mole fraction and the vapor pressure of the pure solvent.
The expression of Raoult’s law is,
Psolution=xsolvent P∘solvent

Expert Solution & Answer

Answer to Problem 1DE

Solution: The interaction between solute and solvent and the number of solute particles are responsible for the lower vapor pressures of the solution than the pure solvents.

Explanation of Solution

According to Raoult’s law, the vapor pressure of a solution is equal to the product of the mole fraction and the vapor pressure of the pure solvent.
The expression of Raoult’s law is,

Psolution=xsolvent P∘solvent

When a solute is added to a solution, the vapor pressure of the solution decreases because on addition of solute, the gap between the solvent molecules gets filled. Hence, on the surface of solution, the number of solvent molecule is less as compared to the pure solvent. This indicates that the number of solvent molecule enter into the gas phase is less and due to this there is a decrease in vapor pressure.
Using the Raoult’s law, the lowering of vapor pressure can be explained.
Assume two sealed containers, one is for pure solvent and other is for solution. The equilibrium stage arises when the number of molecules striking on the surface of the molecule becomes equal to the number of molecules going to the gas phase. On addition of solute, half of the surface of the solution is occupied by the solute and half of the surface is occupied by solvent molecules.

Study Guide for Chemistry: The Central Science, Chapter 13, Problem 1DE

Figure 1

The vapor pressure of the solution depends upon the number of solvent molecule present on the surface of the solution. As the number of solute molecule increases, the number of solvent molecule present on the surface of solution decreases, now lesser number of solvent molecules is present to go in gas phase. Hence, the vapor pressure of the solution decreases.

The attraction between molecules of solvent with solute also plays an important role in lowering the vapor pressure. If there is a strong attraction between the solute and solvent, than the solvent molecule try to remain in the solution rather than escaping from it. Due to this, lowering of vapor pressure occurs because now there are less number of solvent molecule in vapor phase.

Another important factor is that, number of molecules present in the solution is not important rather than this number of solute particles present in the solution is important.
More the number of solute particles, low will be the vapor pressure.

Conclusion

The interaction between solute and solvent and the number of solute particles are responsible for the lower vapor pressures of the solution than the pure solvents.

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 4

Question

Chapter 13, Problem 1DE

Interpretation Introduction

Interpretation: The experimental procedure to test the hypothesis that solute blocking of solvent vaporization is not the reason that solutions have lower vapor pressures than the pure solvents is to be determined.

Concept introduction: According to Raoult’s law, the vapor pressure of a solution is equal to the product of the mole fraction and the vapor pressure of the pure solvent.
The expression of Raoult’s law is,
Psolution=xsolvent P∘solvent

Expert Solution & Answer

Answer to Problem 1DE

Solution: The interaction between solute and solvent and the number of solute particles are responsible for the lower vapor pressures of the solution than the pure solvents.

Explanation of Solution

According to Raoult’s law, the vapor pressure of a solution is equal to the product of the mole fraction and the vapor pressure of the pure solvent.
The expression of Raoult’s law is,

Psolution=xsolvent P∘solvent

When a solute is added to a solution, the vapor pressure of the solution decreases because on addition of solute, the gap between the solvent molecules gets filled. Hence, on the surface of solution, the number of solvent molecule is less as compared to the pure solvent. This indicates that the number of solvent molecule enter into the gas phase is less and due to this there is a decrease in vapor pressure.
Using the Raoult’s law, the lowering of vapor pressure can be explained.
Assume two sealed containers, one is for pure solvent and other is for solution. The equilibrium stage arises when the number of molecules striking on the surface of the molecule becomes equal to the number of molecules going to the gas phase. On addition of solute, half of the surface of the solution is occupied by the solute and half of the surface is occupied by solvent molecules.

Study Guide for Chemistry: The Central Science, Chapter 13, Problem 1DE

Figure 1

The vapor pressure of the solution depends upon the number of solvent molecule present on the surface of the solution. As the number of solute molecule increases, the number of solvent molecule present on the surface of solution decreases, now lesser number of solvent molecules is present to go in gas phase. Hence, the vapor pressure of the solution decreases.

The attraction between molecules of solvent with solute also plays an important role in lowering the vapor pressure. If there is a strong attraction between the solute and solvent, than the solvent molecule try to remain in the solution rather than escaping from it. Due to this, lowering of vapor pressure occurs because now there are less number of solvent molecule in vapor phase.

Another important factor is that, number of molecules present in the solution is not important rather than this number of solute particles present in the solution is important.
More the number of solute particles, low will be the vapor pressure.

Conclusion

The interaction between solute and solvent and the number of solute particles are responsible for the lower vapor pressures of the solution than the pure solvents.

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 5

Chapter 13, Problem 1DE

Interpretation Introduction

Interpretation: The experimental procedure to test the hypothesis that solute blocking of solvent vaporization is not the reason that solutions have lower vapor pressures than the pure solvents is to be determined.

Concept introduction: According to Raoult’s law, the vapor pressure of a solution is equal to the product of the mole fraction and the vapor pressure of the pure solvent.
The expression of Raoult’s law is,
Psolution=xsolvent P∘solvent

Expert Solution & Answer

Answer to Problem 1DE

Solution: The interaction between solute and solvent and the number of solute particles are responsible for the lower vapor pressures of the solution than the pure solvents.

Explanation of Solution

According to Raoult’s law, the vapor pressure of a solution is equal to the product of the mole fraction and the vapor pressure of the pure solvent.
The expression of Raoult’s law is,

Psolution=xsolvent P∘solvent

When a solute is added to a solution, the vapor pressure of the solution decreases because on addition of solute, the gap between the solvent molecules gets filled. Hence, on the surface of solution, the number of solvent molecule is less as compared to the pure solvent. This indicates that the number of solvent molecule enter into the gas phase is less and due to this there is a decrease in vapor pressure.
Using the Raoult’s law, the lowering of vapor pressure can be explained.
Assume two sealed containers, one is for pure solvent and other is for solution. The equilibrium stage arises when the number of molecules striking on the surface of the molecule becomes equal to the number of molecules going to the gas phase. On addition of solute, half of the surface of the solution is occupied by the solute and half of the surface is occupied by solvent molecules.

Study Guide for Chemistry: The Central Science, Chapter 13, Problem 1DE

Figure 1

The vapor pressure of the solution depends upon the number of solvent molecule present on the surface of the solution. As the number of solute molecule increases, the number of solvent molecule present on the surface of solution decreases, now lesser number of solvent molecules is present to go in gas phase. Hence, the vapor pressure of the solution decreases.

The attraction between molecules of solvent with solute also plays an important role in lowering the vapor pressure. If there is a strong attraction between the solute and solvent, than the solvent molecule try to remain in the solution rather than escaping from it. Due to this, lowering of vapor pressure occurs because now there are less number of solvent molecule in vapor phase.

Another important factor is that, number of molecules present in the solution is not important rather than this number of solute particles present in the solution is important.
More the number of solute particles, low will be the vapor pressure.

Conclusion

The interaction between solute and solvent and the number of solute particles are responsible for the lower vapor pressures of the solution than the pure solvents.

Answer 6

Chapter 13, Problem 1DE

Interpretation Introduction

Interpretation: The experimental procedure to test the hypothesis that solute blocking of solvent vaporization is not the reason that solutions have lower vapor pressures than the pure solvents is to be determined.

Concept introduction: According to Raoult’s law, the vapor pressure of a solution is equal to the product of the mole fraction and the vapor pressure of the pure solvent.
The expression of Raoult’s law is,
Psolution=xsolvent P∘solvent

Expert Solution & Answer

Answer to Problem 1DE

Solution: The interaction between solute and solvent and the number of solute particles are responsible for the lower vapor pressures of the solution than the pure solvents.

Explanation of Solution

According to Raoult’s law, the vapor pressure of a solution is equal to the product of the mole fraction and the vapor pressure of the pure solvent.
The expression of Raoult’s law is,

Psolution=xsolvent P∘solvent

When a solute is added to a solution, the vapor pressure of the solution decreases because on addition of solute, the gap between the solvent molecules gets filled. Hence, on the surface of solution, the number of solvent molecule is less as compared to the pure solvent. This indicates that the number of solvent molecule enter into the gas phase is less and due to this there is a decrease in vapor pressure.
Using the Raoult’s law, the lowering of vapor pressure can be explained.
Assume two sealed containers, one is for pure solvent and other is for solution. The equilibrium stage arises when the number of molecules striking on the surface of the molecule becomes equal to the number of molecules going to the gas phase. On addition of solute, half of the surface of the solution is occupied by the solute and half of the surface is occupied by solvent molecules.

Study Guide for Chemistry: The Central Science, Chapter 13, Problem 1DE

Figure 1

The vapor pressure of the solution depends upon the number of solvent molecule present on the surface of the solution. As the number of solute molecule increases, the number of solvent molecule present on the surface of solution decreases, now lesser number of solvent molecules is present to go in gas phase. Hence, the vapor pressure of the solution decreases.

The attraction between molecules of solvent with solute also plays an important role in lowering the vapor pressure. If there is a strong attraction between the solute and solvent, than the solvent molecule try to remain in the solution rather than escaping from it. Due to this, lowering of vapor pressure occurs because now there are less number of solvent molecule in vapor phase.

Another important factor is that, number of molecules present in the solution is not important rather than this number of solute particles present in the solution is important.
More the number of solute particles, low will be the vapor pressure.

Conclusion

The interaction between solute and solvent and the number of solute particles are responsible for the lower vapor pressures of the solution than the pure solvents.

Answer 7

Chapter 13, Problem 1DE

Interpretation Introduction

Interpretation: The experimental procedure to test the hypothesis that solute blocking of solvent vaporization is not the reason that solutions have lower vapor pressures than the pure solvents is to be determined.

Concept introduction: According to Raoult’s law, the vapor pressure of a solution is equal to the product of the mole fraction and the vapor pressure of the pure solvent.
The expression of Raoult’s law is,
Psolution=xsolvent P∘solvent

Answer 8

Expert Solution & Answer

Answer to Problem 1DE

Solution: The interaction between solute and solvent and the number of solute particles are responsible for the lower vapor pressures of the solution than the pure solvents.

Answer 9

Expert Solution & Answer

Answer 10

Expert Solution & Answer

Answer 11

Explanation of Solution

According to Raoult’s law, the vapor pressure of a solution is equal to the product of the mole fraction and the vapor pressure of the pure solvent.
The expression of Raoult’s law is,

Psolution=xsolvent P∘solvent

When a solute is added to a solution, the vapor pressure of the solution decreases because on addition of solute, the gap between the solvent molecules gets filled. Hence, on the surface of solution, the number of solvent molecule is less as compared to the pure solvent. This indicates that the number of solvent molecule enter into the gas phase is less and due to this there is a decrease in vapor pressure.
Using the Raoult’s law, the lowering of vapor pressure can be explained.
Assume two sealed containers, one is for pure solvent and other is for solution. The equilibrium stage arises when the number of molecules striking on the surface of the molecule becomes equal to the number of molecules going to the gas phase. On addition of solute, half of the surface of the solution is occupied by the solute and half of the surface is occupied by solvent molecules.

Study Guide for Chemistry: The Central Science, Chapter 13, Problem 1DE

Figure 1

The vapor pressure of the solution depends upon the number of solvent molecule present on the surface of the solution. As the number of solute molecule increases, the number of solvent molecule present on the surface of solution decreases, now lesser number of solvent molecules is present to go in gas phase. Hence, the vapor pressure of the solution decreases.

The attraction between molecules of solvent with solute also plays an important role in lowering the vapor pressure. If there is a strong attraction between the solute and solvent, than the solvent molecule try to remain in the solution rather than escaping from it. Due to this, lowering of vapor pressure occurs because now there are less number of solvent molecule in vapor phase.

Another important factor is that, number of molecules present in the solution is not important rather than this number of solute particles present in the solution is important.
More the number of solute particles, low will be the vapor pressure.

Answer 12

Conclusion

The interaction between solute and solvent and the number of solute particles are responsible for the lower vapor pressures of the solution than the pure solvents.

Answer 13

Ch. 13.3 - Prob. 13.1.1PE Ch. 13.3 - Prob. 13.1.2PE Ch. 13.3 - Prob. 13.2.1PE Ch. 13.3 - Prob. 13.2.2PE Ch. 13.4 - Prob. 13.3.1PE Ch. 13.4 - Prob. 13.3.2PE Ch. 13.4 - Prob. 13.4.1PE Ch. 13.4 - Prob. 13.4.2PE Ch. 13.4 - Prob. 13.5.1PE Ch. 13.4 - Prob. 13.5.2PE

Answer to Problem 1DE

Explanation of Solution

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Chapter 13 Solutions