Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 38: Problem 16

Assume that the system is at equilibrium as determined in CTQ \(13 .\) What will happen to the number of moles of \(\mathrm{PCl}_{3}\) present if some \(\mathrm{PCl}_{5}\) gas is suddenly injected into the box? Explain your reasoning.

Short Answer

Expert verified
The number of moles of \(\mathrm{PCl}_{3}\) will increase when additional \(\mathrm{PCl}_{5}\) gas is injected into the box as the system shifts its equilibrium to re-establish balance.

Step by step solution

01

Identify the system and disruption

The equilibrium in consideration here is the reaction \(\mathrm{PCl}_{5} \rightleftharpoons \mathrm{PCl}_{3} + \mathrm{Cl}_{2}\). The disturbance or change here is an increase in the concentration of \(\mathrm{PCl}_{5}\).
02

Le Chatelier's response

According to Le Chatelier's Principle, the system will respond in such a way to offset the change. This means that the equilibrium will shift in the direction that reduces the number of moles of \(\mathrm{PCl}_{5}\). In this case, the equilibrium will shift to the right, as this will consume the added \(\mathrm{PCl}_{5}\) to form more \(\mathrm{PCl}_{3}\) and \(\mathrm{Cl}_{2}\).
03

Determine the effect on PCl3

Because the equilibrium shifts to the right, more \(\mathrm{PCl}_{3}\) will be produced. Therefore, the number of moles of \(\mathrm{PCl}_{3}\) present will increase.

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

Assume that the system is at equilibrium as determined in CTQ \(13 .\) What will happen to the number of moles of \(\mathrm{PCl}_{3}\) present if some \(\mathrm{Cl}_{2}\) gas is suddenly injected into the box? Explain your reasoning.

Consider a situation in which the reaction quotient, \(Q_{\mathrm{c}}\), for a given reaction is larger than the equilibrium constant, \(K_{\mathrm{c}}\) a) How must the value of \(\mathrm{Q}_{\mathrm{c}}\) change to reach equilibrium? b) Describe how the concentrations of reactants and/or the concentration of products must change to reach equlibrium.

Explain why the reaction quotient is useful.

In general, how does the rate of the forward reaction \((\mathrm{Y} \rightarrow \mathrm{Z})\) at equilibrium compare to the rate of the reverse reaction \((\mathrm{Z} \rightarrow \mathrm{Y})\) at equilibrium?
See all solutions

Recommended explanations on Chemistry Textbooks

Organic Chemistry

Read Explanation

Inorganic Chemistry

Read Explanation

Nuclear Chemistry

Read Explanation

Chemical Reactions

Read Explanation

The Earths Atmosphere

Read Explanation

Chemistry Branches

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