Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 13: Problem 66

What will happen to the number of moles of \(\mathrm{SO}_{3}\) in equilibrium with \(\mathrm{SO}_{2}\) and \(\mathrm{O}_{2}\) in the reaction $$ 2 \mathrm{SO}_{3}(g) \rightleftharpoons 2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) $$ in each of the following cases? a. Oxygen gas is added. b. The pressure is increased by decreasing the volume of the reaction container. c. In a rigid reaction container, the pressure is increased by adding argon gas. d. The temperature is decreased (the reaction is endothermic). e. Gaseous sulfur dioxide is removed.

Short Answer

Expert verified
a. The number of moles of \(\mathrm{SO}_{3}\) will increase. b. The number of moles of \(\mathrm{SO}_{3}\) will increase. c. There will be no change in the number of moles of \(\mathrm{SO}_{3}\). d. The number of moles of \(\mathrm{SO}_{3}\) will decrease. e. The number of moles of \(\mathrm{SO}_{3}\) will decrease.

Step by step solution

01

a. Oxygen gas is added.

Adding more oxygen gas to the system will increase the concentration of \(\mathrm{O}_{2}\). To counteract this, the reaction will shift to the left to consume the excess \(\mathrm{O}_{2}\). This results in an increase in the concentration of \(\mathrm{SO}_{3}\).
02

b. The pressure is increased by decreasing the volume.

When the volume of the container is decreased, the pressure inside increases. According to Le Chatelier's Principle, the system will respond by shifting towards the side with fewer moles of gas. In this case, the left side of the reaction (2 moles of \(\mathrm{SO}_{3}\)) has fewer moles than the right side (3 moles - 2 moles of \(\mathrm{SO}_{2}\) and 1 mole of \(\mathrm{O}_{2}\)). Therefore, the reaction will shift to the left, and the concentration of \(\mathrm{SO}_{3}\) will increase.
03

c. In a rigid container, the pressure is increased by adding argon gas.

Since argon is an inert gas and does not participate in the reaction, adding it does not affect the equilibrium directly. However, when the pressure is increased due to the addition of argon, the partial pressures of the components will not change. Therefore, there will be no change in the number of moles of \(\mathrm{SO}_{3}\).
04

d. The temperature is decreased (the reaction is endothermic).

In an endothermic reaction, heat can be considered a reactant. Decreasing the temperature is equivalent to removing heat from the system. According to Le Chatelier's Principle, the reaction will shift towards the side that absorbs the heat, in this case, the right side. The shift to the right will result in a decrease in the concentration of \(\mathrm{SO}_{3}\).
05

e. Gaseous sulfur dioxide is removed.

When \(\mathrm{SO}_{2}\) is removed, its concentration decreases. To counteract the change, the reaction will shift towards the right side to produce more \(\mathrm{SO}_{2}\). This means that more \(\mathrm{SO}_{3}\) will be consumed, and its concentration will decrease.

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

For the reaction below, \(K_{\mathrm{p}}=1.16\) at \(800 .{ }^{\circ} \mathrm{C}\). $$ \mathrm{CaCO}_{3}(s) \rightleftharpoons \mathrm{CaO}(s)+\mathrm{CO}_{2}(g) $$ If a 20.0-g sample of \(\mathrm{CaCO}_{3}\) is put into a \(10.0\) - \(\mathrm{L}\) container and heated to \(800 .{ }^{\circ} \mathrm{C}\), what percentage by mass of the \(\mathrm{CaCO}_{3}\) will react to reach equilibrium?

For a typical equilibrium problem, the value of \(K\) and the initial reaction conditions are given for a specific reaction, and you are asked to calculate the equilibrium concentrations. Many of these calculations involve solving a quadratic or cubic equation. What can you do to avoid solving a quadratic or cubic equation and still come up with reasonable equilibrium concentrations?

At \(327^{\circ} \mathrm{C}\), the equilibrium concentrations are \(\left[\mathrm{CH}_{3} \mathrm{OH}\right]=0.15 \mathrm{M}\), \([\mathrm{CO}]=0.24 M\), and \(\left[\mathrm{H}_{2}\right]=1.1 M\) for the reaction $$ \mathrm{CH}_{3} \mathrm{OH}(g) \rightleftharpoons \mathrm{CO}(g)+2 \mathrm{H}_{2}(g) $$ Calculate \(K_{\mathrm{p}}\) at this temperature.

The equilibrium constant \(K_{\mathrm{p}}\) for the reaction $$ \mathrm{CCl}_{4}(g) \rightleftharpoons \mathrm{C}(s)+2 \mathrm{Cl}_{2}(g) $$ at \(700^{\circ} \mathrm{C}\) is \(0.76\) atm. Determine the initial pressure of carbon tetrachloride that will produce a total equilibrium pressure of \(1.20 \mathrm{~atm}\) at \(700^{\circ} \mathrm{C}\).

Consider the reaction \(\mathrm{A}(g)+2 \mathrm{~B}(g) \rightleftharpoons \mathrm{C}(g)+\mathrm{D}(g)\) in a 1.0-L rigid flask. Answer the following questions for each situation \((\mathrm{a}-\mathrm{d})\) : i. Estimate a range (as small as possible) for the requested substance. For example, [A] could be between \(95 M\) and \(100 M\) ii. Explain how you decided on the limits for the estimated range. iii. Indicate what other information would enable you to narrow your estimated range. iv. Compare the estimated concentrations for a through d, and explain any differences. a. If at equilibrium \([\mathrm{A}]=1 M\), and then \(1 \mathrm{~mol} \mathrm{C}\) is added, estimate the value for \([\mathrm{A}]\) once equilibrium is reestablished. b. If at equilibrium \([\mathrm{B}]=1 M\), and then \(1 \mathrm{~mol} \mathrm{C}\) is added, estimate the value for [B] once equilibrium is reestablished. c. If at equilibrium \([\mathrm{C}]=1 M\), and then \(1 \mathrm{~mol} \mathrm{C}\) is added, estimate the value for \([\mathrm{C}]\) once equilibrium is reestablished. d. If at equilibrium \([\mathrm{D}]=1 M\), and then \(1 \mathrm{~mol} \mathrm{C}\) is added, estimate the value for [D] once equilibrium is reestablished.
See all solutions

Recommended explanations on Chemistry Textbooks

Ionic and Molecular Compounds

Read Explanation

Organic Chemistry

Read Explanation

Physical Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation

Chemical Analysis

Read Explanation

Nuclear Chemistry

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