/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 13 Indicate whether each statement ... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 13: Problem 13

Indicate whether each statement is true or false: (a) A solute will dissolve in a solvent if solute-solute interactions are stronger than solute-solvent interactions. (b) In making a solution, the enthalpy of mixing is always a positive number. (c) An increase in entropy favors mixing.

Short Answer

Expert verified
(a) False, (b) False, (c) True.

Step by step solution

01

Understanding Solute and Solvent Interactions

Statement (a) states that a solute will dissolve in a solvent if solute-solute interactions are stronger than solute-solvent interactions. In reality, dissolution occurs more readily when solute-solvent interactions are strong, allowing the solute particles to disperse into the solvent. Therefore, when solute-solvent interactions are stronger, not solute-solute, the solute is more likely to dissolve. Thus, this statement is False.
02

Examining Enthalpy of Mixing

Statement (b) claims that the enthalpy of mixing is always a positive number. The enthalpy of mixing could be either positive or negative depending on the balance of energy absorbed or released during the dissolution. If more energy is required to break solute-solute and solvent-solvent bonds compared to the energy released upon forming solute-solvent bonds, the enthalpy will be positive, otherwise it will be negative. Thus, this statement is False.
03

Analyzing Entropy's Influence on Mixing

Statement (c) explores the role of entropy in mixing. Entropy reflects the degree of disorder or randomness in a system. An increase in entropy typically favors spontaneous processes, including mixing, because systems tend to move towards higher disorder. Therefore, an increase in entropy does favor mixing. Hence, this statement is True.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91影视!

Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Solute-Solvent Interactions
In solution chemistry, understanding how solutes and solvents interact is vital. When a solute dissolves in a solvent, the solute-solvent interactions come into play in a big way. Generally, solute particles are surrounded by solvent molecules, which allows them to disperse uniformly throughout the solvent. This dispersion is possible because the solute and solvent molecules attract each other.
  • For a successful dissolution, solute-solvent interactions need to be stronger than solute-solute interactions.
  • This attraction helps overcome the forces holding the solute particles together, allowing them to become immersed in the solvent.
When solute-solute interactions are stronger, solute particles prefer to remain bonded to each other, which makes mixing much more difficult. Thus, strong solute-solvent interactions are key to the solubility of a substance.
Enthalpy of Mixing
The enthalpy of mixing is a concept from thermodynamics that helps explain energy changes during dissolution. It represents the heat absorbed or released when solute and solvent combine. The enthalpy of mixing can be either positive or negative:
  • If the energy required to separate solute and solvent molecules is greater than the energy released when they create new bonds, the enthalpy is positive, suggesting that the reaction is endothermic.
  • Conversely, if less energy is needed to disrupt the original interactions than is released during forming new interactions, the enthalpy is negative, indicating an exothermic process.
Thus, the enthalpy of mixing isn't always positive; it is entirely dependent on the specific interaction dynamics between the solute and solvent.
Entropy and Mixing
Entropy reflects the level of disorder in a system, and it plays a crucial role in the mixing process. It is a measure of how much energy in a system is unavailable to do work, often described as a system's tendency towards chaos.
  • A higher entropy state is more probable because nature tends to favor disorder and randomness over order.
  • Thus, an increase in entropy generally encourages the mixing of substances.
This is because mixing increases the number of possible configurations for the dissolved particles, leading to a higher entropy state. Therefore, in most cases, an increase in entropy favors the mixing process, making it a driving force for spontaneous dissolution.

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

At \(63.5^{\circ} \mathrm{C},\) the vapor pressure of \(\mathrm{H}_{2} \mathrm{O}\) is \(23.3 \mathrm{kPa},\) and that of ethanol \(\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\right)\) is \(53.3 \mathrm{kPa}\). A solution is made by mixing equal masses of \(\mathrm{H}_{2} \mathrm{O}\) and \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\). (a) What is the mole fraction of ethanol in the solution? (b) Assuming idealsolution behavior, what is the vapor pressure of the solution at \(63.5^{\circ} \mathrm{C} ?(\mathbf{c})\) What is the mole fraction of ethanol in the vapor above the solution?

A dilute aqueous solution of fructose in water is formed by dissolving \(1.25 \mathrm{~g}\) of the compound in water to form \(0.150 \mathrm{~L}\) of solution. The resulting solution has an osmotic pressure of \(112.8 \mathrm{kPa}\) at \(20^{\circ} \mathrm{C}\). Assuming that the organic compound is a nonelectrolyte, what is its molar mass?

A sulfuric acid solution containing \(697.6 \mathrm{~g}\) of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) per liter of solution has a density of \(1.395 \mathrm{~g} / \mathrm{cm}^{3} .\) Calculate (a) the mass percentage, (b) the mole fraction, (c) the molality, \((\mathbf{d})\) the molarity of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) in this solution.

Indicate whether each statement is true or false: \((\mathbf{a}) \mathrm{NaCl}\) dissolves in water but not in benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)\) because benzene is denser than water. (b) \(\mathrm{NaCl}\) dissolves in water but not in benzene because water has a large dipole moment and benzene has zero dipole moment. (c) NaCl dissolves in water but not in benzene because the water-ion interactions are stronger than benzene-ion interactions.

Ascorbic acid (vitamin C, \(\mathrm{C}_{6} \mathrm{H}_{8} \mathrm{O}_{6}\) ) is a water-soluble vitamin. A solution containing \(80.5 \mathrm{~g}\) of ascorbic acid dissolved in \(210 \mathrm{~g}\) of water has a density of \(1.22 \mathrm{~g} / \mathrm{mL}\) at \(55^{\circ} \mathrm{C}\). Calculate (a) the mass percentage, \((\mathbf{b})\) the mole fraction, \((\mathbf{c})\) the molality, \((\mathbf{d})\) the molarity of ascorbic acid in this solution.
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Reactions

Read Explanation

Nuclear Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation

Making Measurements

Read Explanation

Chemistry Branches

Read Explanation

Chemical Analysis

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.