/*! 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 10 Which of the following processes... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 19: Problem 10

Which of the following processes are spontaneous: (a) the melting of ice cubes at \(10^{\circ} \mathrm{C}\) and 1 atm pressure; (b) separating a mixture of \(\mathrm{N}_{2}\) and \(\mathrm{O}_{2}\) into two separate samples, one that is pure \(\mathrm{N}_{2}\) and one that is pure \(\mathrm{O}_{2}\); (c) alignment of iron filings in a magnetic field; (d) the reaction of sodium metal with chlorine gas to form sodium chloride; (e) the dissolution of \(\mathrm{HCl}(g)\) in water to form concentrated hydrochloric acid?

Short Answer

Expert verified
The spontaneous processes are: (a) the melting of ice cubes at \(10^{\circ} \mathrm{C}\) and 1 atm pressure, (c) alignment of iron filings in a magnetic field, (d) the reaction of sodium metal with chlorine gas to form sodium chloride, and (e) the dissolution of \(\mathrm{HCl}(g)\) in water to form concentrated hydrochloric acid.

Step by step solution

01

Process (a) - Melting of ice cubes at 10掳C and 1 atm

: Ice cube melting means a phase transition going from solid ice to liquid water. The given condition is that the temperature is above its freezing/melting point, which is 0掳C at 1 atm atmospheric pressure. Since the temperature is higher than its melting point, it means the ice would absorb heat and start to melt. Therefore, melting is a spontaneous process under these conditions.
02

Process (b) - Separating a mixture of N2 and O2

: In this process, we need to evaluate if separating a mixture of N2 and O2 into two pure samples of N2 and O2 occurs spontaneously. In general, gases tend to mix and naturally spread out, as they have natural tendency towards higher entropy. To separate the gases, it is required to apply a specific method or external influence. Hence, this process of separating N2 and O2 does not occur spontaneously.
03

Process (c) - Alignment of iron filings in a magnetic field

: Iron filings are made up of small particles of iron which are attracted to a magnetic field. When a magnetic field is introduced, the iron filings will align themselves along the magnetic field lines. In this case, the external influence is the magnetic field itself, and the alignment of iron filings will occur spontaneously under its influence.
04

Process (d) - Reaction of sodium metal with chlorine gas

: The reaction between sodium (Na) and chlorine (Cl2) is given as follows: \[ 2 \mathrm{Na}(s) + \mathrm{Cl}_{2}(g) \longrightarrow 2 \mathrm{NaCl}(s) \] This reaction is known to be highly exothermic, which means it releases a large amount of energy. Exothermic reactions typically occur spontaneously because they result in a decrease in the system's internal energy. Therefore, the reaction of sodium metal with chlorine gas to form sodium chloride is spontaneous.
05

Process (e) - Dissolution of HCl(g) in water

: The dissolution of HCl gas in water to form concentrated hydrochloric acid is an exothermic reaction that releases heat. It results in the formation of solvated hydrogen ions and chloride ions in solution: \[ \mathrm{HCl}(g) + \mathrm{H}_{2}\mathrm{O}(l) \longrightarrow \mathrm{H}_{3}\mathrm{O}^{+}(aq) + \mathrm{Cl}^{-}(aq) \] As the process is exothermic and results in an increase in the system's entropy (the gas dissolves into an aqueous solution), the dissolution of HCl(g) in water is a spontaneous process.

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!

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

Ammonium nitrate dissolves spontaneously and endothermally in water at room temperature. What can you deduce about the sign of \(\Delta S\) for this solution process?

(a) The energy of a gas is increased by heating it. Using \(\mathrm{CO}_{2}\) as an example, illustrate the different ways in which additional energy can be distributed among the molecules of the gas. (b) You are told that the number of microstates for a system increases. What does this tell you about the entropy of the system?

For each of the following pairs, choose the substance with the higher entropy per mole at a given temperature: (a) \(\operatorname{Ar}(l)\) or \(\operatorname{Ar}(g)\), (b) \(\mathrm{He}(g)\) at 3 atm pressure or \(\mathrm{He}(\mathrm{g})\) at \(1.5\) atm pressure, (c) \(1 \mathrm{~mol}\) of \(\mathrm{Ne}(g)\) in \(15.0 \mathrm{~L}\) or mol of \(\mathrm{Ne}(\mathrm{g})\) in \(1.50 \mathrm{~L}_{,}(\mathrm{d}) \mathrm{CO}_{2}(g)\) or \(\mathrm{CO}_{2}(\mathrm{~s})\)

(a) Express the second law of thermodynamics in words. (b) If the entropy of the system increases during a reversible process, what can you say about the entropy change of the surroundings? (c) In a certain spontaneous process the system undergoes an entropy change, \(\Delta S=42 \mathrm{~J} / \mathrm{K}\). What can you conclude about \(\Delta S_{\text {surr }} ?\)

Consider a process in which an ideal gas changes from state 1 to state 2 in such a way that its temperature changes from \(300 \mathrm{~K}\) to \(200 \mathrm{~K}\). (a) Describe how this change might be carried out while keeping the volume of the gas constant. (b) Describe how it might be carried out while keeping the pressure of the gas constant. (c) Does the change in \(\Delta E\) depend on the particular pathway taken to carry out this change of state? Explain.
See all solutions

Recommended explanations on Chemistry Textbooks

Chemistry Branches

Read Explanation

Chemical Reactions

Read Explanation

Kinetics

Read Explanation

Nuclear Chemistry

Read Explanation

Physical Chemistry

Read Explanation

Making Measurements

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.