Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 14: Problem 52

Write the expression for \(K_{\text {eq }}\) for the reaction \(4 \mathrm{NH}_{3}(g)+5 \mathrm{O}_{2}(g) \rightleftarrows 4 \mathrm{NO}(g)+6 \mathrm{H}_{2} \mathrm{O}(g)\)

Short Answer

Expert verified
The expression for the equilibrium constant, \(K_{eq}\), for the given reaction is: \[K_{eq} = \frac{[NO]^4[H_2O]^6}{[NH_3]^4[O_2]^5}\]

Step by step solution

01

Identify the reactants and products

In the given reaction, the reactants are: - Ammonia (NH3) with a coefficient of 4 - Oxygen (O2) with a coefficient of 5 The products are: - Nitric oxide (NO) with a coefficient of 4 - Water vapor (H2O) with a coefficient of 6
02

Write the expression for the equilibrium constant \(K_{eq}\)

Using the general formula for the equilibrium constant, we have \[K_{eq} = \frac{[NO]^4[H_2O]^6}{[NH_3]^4[O_2]^5}\] This gives us the expression for the equilibrium constant for the given reaction.

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

Will \(K_{\text {eq }}\) for an endothermic reaction increase or decrease when the reaction mixture is (a) heated and (b) cooled? Explain your answer.

Write the equilibrium constant expression for: (a) \(\mathrm{SiCl}_{4}(l)+2 \mathrm{H}_{2} \mathrm{O}(g)\) \(\rightleftarrows \mathrm{SiO}_{2}(s)+4 \mathrm{HCl}(g)\) (b) \(\mathrm{H}_{2}(\mathrm{~g})+\mathrm{CO}_{2}(g) \rightleftarrows \mathrm{CO}(g)+\mathrm{H}_{2} \mathrm{O}(l)\) (c) \(\mathrm{MnO}_{2}(s)+4 \mathrm{H}^{+}(a q)+2 \mathrm{Cl}^{-}(a q)\) \(\rightleftarrows \mathrm{Mn}^{2+}(a q)+\mathrm{Cl}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(l)\) (d) \(\mathrm{I}_{2}(s) \rightleftarrows \mathrm{I}_{2}(g)\) (e) \(\mathrm{TiCl}_{4}(g)+2 \mathrm{Mg}(s) \rightleftarrows \mathrm{Ti}(s)+2 \mathrm{MgCl}_{2}(s)\) (f) \(\mathrm{Ni}(\mathrm{OH})_{2}(s) \rightleftarrows \mathrm{Ni}^{2+}(a q)+2 \mathrm{OH}^{-}(a q)\)

Phosphorus pentachloride gas decomposes to \(\mathrm{PCl}_{3}(\mathrm{~g})\) and \(\mathrm{Cl}_{2}(\mathrm{~g}) .\) At equilibrium, the concentrations of the decomposition products are \(5.50 \times 10^{-3} \mathrm{M}\) for \(\mathrm{PCl}_{3}(\mathrm{~g})\) and \(0.125 \mathrm{M}\) for \(\mathrm{Cl}_{2}(g)\). What is the equilibrium concentration of \(\mathrm{PCl}_{5}\) ? The equilibrium constant for this reaction is \(7.50 \times 10^{-2}\).

The saturation solubility of \(\mathrm{Ag}_{2} \mathrm{~S}\) at \(25^{\circ} \mathrm{C}\) is \(1.14 \times 10^{-17} \mathrm{M}\). What are the equilibrium concentrations of the cation and anion?

Would the value you obtain for \(K_{\text {eq }}\) for a reaction depend on the initial concentrations of reactants and products you use? Explain your answer.
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Reactions

Read Explanation

Physical Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation

Nuclear Chemistry

Read Explanation

Organic Chemistry

Read Explanation

Kinetics

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