Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 18: Problem 27

Which of the following reactions is (are) spontaneous at standard conditions? (a) \(2 \mathrm{NO}_{3}^{-}(a q)+8 \mathrm{H}^{+}(a q)+6 \mathrm{Cl}^{-}(a q) \longrightarrow\) \(2 \mathrm{NO}(g)+4 \mathrm{H}_{2} \mathrm{O}+3 \mathrm{Cl}_{2}(g)\) (b) \(\mathrm{O}_{2}(g)+4 \mathrm{H}^{+}(a q)+4 \mathrm{Cl}^{-}(a q) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}+2 \mathrm{Cl}_{2}(g)\) (c) \(3 \mathrm{Fe}(s)+2 \mathrm{AuCl}_{4}^{-}(a q) \longrightarrow 2 \mathrm{Au}(s)+8 \mathrm{Cl}^{-}(a q)+3 \mathrm{Fe}^{2+}(a q)\)

Short Answer

Expert verified
Provide the calculated ∆G° values for each reaction to support your answer.

Step by step solution

01

(a) Calculate ∆G° for reaction (a)

Using the standard Gibbs free energy values from a table, find the ∆G° values for the reactants and products of reaction (a). Subtract the sum of the reactant ∆G° values from the sum of the product ∆G° values to find the ∆G° for the reaction.
02

(b) Calculate ∆G° for reaction (b)

Repeat step (a) for the reactants and products of reaction (b).
03

(c) Calculate ∆G° for reaction (c)

Repeat step (a) for the reactants and products of reaction (c). Step 2: Determine if each reaction is spontaneous
04

(a) Determine spontaneity for reaction (a)

If the calculated ∆G° for reaction (a) is negative, then the reaction is spontaneous. If the ∆G° is positive or zero, the reaction is non-spontaneous or reaches equilibrium, respectively.
05

(b) Determine spontaneity for reaction (b)

Repeat step (a) for the calculated ∆G° of reaction (b).
06

(c) Determine spontaneity for reaction (c)

Repeat step (a) for the calculated ∆G° of reaction (c). Step 3: Conclusion
07

Conclusion

Based on the calculated ∆G° values and the spontaneity determinations, list which of the reactions (a), (b), and (c) are spontaneous at standard conditions.

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

Calculate \(E^{\circ}\) for the following cells: (a) \(\mathrm{Pb}\left|\mathrm{PbSO}_{4} \| \mathrm{Pb}^{2+}\right| \mathrm{Pb}\) (b) \(\mathrm{Pt}\left|\mathrm{Cl}_{2}\right| \mathrm{ClO}_{3}^{-} \| \mathrm{O}_{2}\left|\mathrm{H}_{2} \mathrm{O}\right| \mathrm{Pt}\) (c) \(\mathrm{Pt}\left|\mathrm{OH}^{-}\right| \mathrm{O}_{2} \| \mathrm{ClO}_{3}^{-}, \mathrm{Cl}^{-} \mid \mathrm{Pt} \quad\) (basic medium)

A solution containing a metal ion \(\left(M^{2+}(a q)\right)\) is electrolyzed by a current of \(7.8\) A. After \(15.5\) minutes, \(2.39 \mathrm{~g}\) of the metal is plated out. (a) How many coulombs are supplied by the battery? (b) What is the metal? (Assume \(100 \%\) efficiency.)

A hydrogen-oxygen fuel cell operates on the reaction: $$ \mathrm{H}_{2}(g)+\frac{1}{2} \mathrm{O}_{2}(g) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l) $$ If the cell is designed to produce \(1.5\) amp of current and if the hydrogen is contained in a 1.0-L tank at 200 atm pressure and \(25^{\circ} \mathrm{C}\), how long can the fuel cell operate before the hydrogen runs out? Assume that oxygen gas is in excess.

The electrolysis of an aqueous solution of \(\mathrm{NaCl}\) has the overall equation $$ 2 \mathrm{H}_{2} \mathrm{O}+2 \mathrm{Cl}^{-}(a q) \longrightarrow \mathrm{H}_{2}(g)+\mathrm{Cl}_{2}(g)+2 \mathrm{OH}^{-}(a q) $$ During the electrolysis, \(0.228\) mol of electrons passes through the cell. (a) How many electrons does this represent? (b) How many coulombs does this represent? (c) Assuming \(100 \%\) yield, what masses of \(\mathrm{H}_{2}\) and \(\mathrm{Cl}_{2}\) are produced?

Calculate voltages of the following cells at \(25^{\circ} \mathrm{C}\) and under the following conditions. (a) \(\mathrm{Fe}\left|\mathrm{Fe}^{2+}(0.010 \mathrm{M}) \| \mathrm{Cu}^{2+}(0.10 \mathrm{M})\right| \mathrm{Cu}\) (b) \(\mathrm{Pt}\left|\mathrm{Sn}^{2+}(0.10 \mathrm{M}), \mathrm{Sn}^{4+}(0.010 \mathrm{M}) \| \mathrm{Co}^{2+}(0.10 \mathrm{M})\right| \mathrm{Co}\)
See all solutions

Recommended explanations on Chemistry Textbooks

Organic Chemistry

Read Explanation

Kinetics

Read Explanation

Chemical Reactions

Read Explanation

Inorganic Chemistry

Read Explanation

Making Measurements

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