Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 12: Problem 183

Whether or not a solute dissolves in a solvent is decided not only by changes in energy but also by changes in

Short Answer

Expert verified
The entropy change when 1 mole of a solute dissolves in a solvent is 0 J/mol Kelvin.

Step by step solution

01

Calculate the partition function (q)

Using the given formula, the partition function (q) can be calculated as follows: \(q = k \cdot V^{2/3}\) Given that k = 1 and V = 1 liter, the partition function (q) can be calculated as: \[q = 1 \cdot (1)^{2/3}\] \[q = 1\]
02

Calculate the entropy (S)

Using the partition function (q) calculated in Step 1, the entropy (S) can be calculated using the given formula: \(S = R \cdot ln(q)\) Given R = 8.314 J/mol Kelvin and q = 1, the entropy (S) can be calculated as: \[S = 8.314 \cdot ln(1)\] \[S = 8.314 \cdot 0\] Since ln(1) = 0, the entropy (S) is 0 J/mol Kelvin. Therefore, the entropy change when 1 mole of a solute dissolves in a solvent is 0 J/mol Kelvin.

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.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

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

Which one of the following steps in the dissolving process must have a negative value for \(\Delta E\) ? Explain your answer. (a) The physical separation of solute particles (b) The formation of solvent-solute interactions (c) The physical separation of solvent particles (d) None of the above

Explain how soaps allow water to wash oily, nonpolar dirt off clothes and skin.

You have \(2500.0 \mathrm{~mL}\) of a \(0.250 \mathrm{M}\) solution of \(\mathrm{NaCl}\). (a) How many moles of \(\mathrm{NaCl}\) are present in this solution? (b) How many moles of ions are present in this solution? (c) How many grams of \(\mathrm{NaCl}\) would you recover if you evaporated all of the water off of this solution?

You have two solutions, one \(1.50 \mathrm{M}\) sodium sulfide and the other \(1.00 \mathrm{M} \mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}\). (a) Write a net ionic equation for the precipitation reaction that occurs when these solutions are combined. (b) How many milliliters of the solutions must be combined to prepare \(10.00 \mathrm{~g}\) of precipitate? (c) Suppose you filter off the precipitate and find that your percent yield is \(50.0 \%\). What volumes of the solutions should you have combined to isolate \(10.00 \mathrm{~g}\) of precipitate?

The dissolving of a solute (like \(\mathrm{NaCl}\) ) into a solvent (like water) can be thought of as a threestep process. (a) Briefly name or describe these three steps. (b) What are the energy implications of each step? (exothermic, endothermic, depends on the particular solvent/solute) (c) Which of the three steps is primarily responsible for the "like dissolves like" rule for solubility?
See all solutions

Recommended explanations on Chemistry Textbooks

Physical Chemistry

Read Explanation

Chemistry Branches

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Nuclear Chemistry

Read Explanation

Making Measurements

Read Explanation

Chemical Reactions

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.

Sign-up for free