Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 15: Problem 2

Explain the difference between physical equilibrium and chemical equilibrium. Give two examples of each.

Short Answer

Expert verified
Physical equilibrium involves a balance of physical processes, like melting or evaporation, with no chemical reactions. Chemical equilibrium, on the other hand, involves a balance of forward and backward chemical reactions. Examples of physical equilibrium include the melting and freezing of ice at a consistent temperature, and the evaporation and condensation of water in a closed container. Examples of chemical equilibrium include the Haber Process for producing ammonia, and the formation and decomposition of hydrogen iodide.

Step by step solution

01

Define Physical Equilibrium

Physical equilibrium refers to the state where the physical processes (like melting, boiling, evaporation etc.) in the system are occurring at the same rate forward and backward. In physical equilibrium, no chemical reaction happens; it is only the physical state changes. Some of the system's properties, such as pressure, volume or temperature, may exhibit steady-state behavior.
02

Examples of Physical Equilibrium

1. When ice melts, it becomes liquid water. In a closed system at a stable temperature, the rate of ice melting will be equal to the rate of water freezing, maintaining equilibrium.\n2. In a closed container partially filled with water, the rate of evaporation of water will be equal to the rate of condensation of the water vapor. This is another example of physical equilibrium.
03

Define Chemical Equilibrium

Chemical equilibrium is the state in which both reactants and products are present in concentrations which have no further tendency to change with time. It typically involves visible chemical changes, such as the decomposition of a chemical compound in a reaction. Even though the concentration of the substances doesn't change over time in chemical equilibrium, the chemical reaction still proceeds but at an equal rate in both directions (forward and reverse).
04

Examples of Chemical Equilibrium

1. The Haber Process for the production of Ammonia is an example. In this process, Nitrogen and Hydrogen react to form Ammonia gas. The reaction proceeds equally in both directions - formation and decomposition of Ammonia, achieving a chemical equilibrium.\n2. The reaction between Hydrogen and Iodide ions to form Hydrogen iodide is another example. Here too, the forward and backward reactions proceed at an equal rate, achieving chemical equilibrium.

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

At \(1130^{\circ} \mathrm{C}\) the equilibrium constant \(\left(K_{\mathrm{c}}\right)\) for the reaction $$ 2 \mathrm{H}_{2} \mathrm{~S}(g) \rightleftharpoons 2 \mathrm{H}_{2}(g)+\mathrm{S}_{2}(g) $$ is \(2.25 \times 10^{-4}\). If \(\left[\mathrm{H}_{2} \mathrm{~S}\right]=4.84 \times 10^{-3} \mathrm{M}\) and \(\left[\mathrm{H}_{2}\right]=\) \(1.50 \times 10^{-3} M,\) calculate \(\left[\mathrm{S}_{2}\right].\)

Consider this reaction: $$ \mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{NO}(g) $$ The equilibrium constant \(K_{P}\) for the reaction is \(1.0 \times\) \(10^{-15}\) at \(25^{\circ} \mathrm{C}\) and 0.050 at \(2200^{\circ} \mathrm{C}\). Is the formation of nitric oxide endothermic or exothermic? Explain your answer.

Consider the reaction $$ \begin{aligned} 2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{SO}_{3}(g) & \\ \Delta H^{\circ}=&-198.2 \mathrm{~kJ} / \mathrm{mol} \end{aligned} $$ Comment on the changes in the concentrations of \(\mathrm{SO}_{2}, \mathrm{O}_{2},\) and \(\mathrm{SO}_{3}\) at equilibrium if we were to \((\mathrm{a})\) increase the temperature, (b) increase the pressure, (c) increase \(\mathrm{SO}_{2},\) (d) add a catalyst, (e) add helium at constant volume.

(a) Use the van't Hoff equation in Problem 15.97 to derive the following expression, which relates the equilibrium constants at two different temperatures $$ \ln \frac{K_{1}}{K_{2}}=\frac{\Delta H^{\circ}}{R}\left(\frac{1}{T_{2}}-\frac{1}{T_{1}}\right) $$ How does this equation support the prediction based on Le Châtelier's principle about the shift in equilibrium with temperature? (b) The vapor pressures of water are \(31.82 \mathrm{mmHg}\) at \(30^{\circ} \mathrm{C}\) and \(92.51 \mathrm{mmHg}\) at \(50^{\circ} \mathrm{C} .\) Calculate the molar heat of vaporization of water.

In 1899 the German chemist Ludwig Mond developed a process for purifying nickel by converting it to the volatile nickel tetracarbonyl \(\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]\) (b.p. \(=\) \(\left.42.2^{\circ} \mathrm{C}\right)\) $$ \mathrm{Ni}(s)+4 \mathrm{CO}(g) \rightleftharpoons \mathrm{Ni}(\mathrm{CO})_{4}(g) $$ (a) Describe how you can separate nickel and its solid impurities. (b) How would you recover nickel? \(\left[\Delta H_{\mathrm{f}}^{\circ}\right.\) for \(\mathrm{Ni}(\mathrm{CO})_{4}\) is \(\left.-602.9 \mathrm{kj} / \mathrm{mol} .\right]\)
See all solutions

Recommended explanations on Chemistry Textbooks

Physical Chemistry

Read Explanation

Making Measurements

Read Explanation

The Earths Atmosphere

Read Explanation

Kinetics

Read Explanation

Ionic and Molecular Compounds

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