Answered: Solve for the following with the given…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

Solve for the following with the given information:

Al3⁺+3e⁻⟶Al E^o= - 1.66 V

Ag⁺+e⁻⟶Ag E^o= +0.80 V

a) Write a balanced full reaction for the oxidation of solid aluminum by silver chloride (Cl^- is the spectator ion).

b) Compute the standard cell potential for this reaction.

c) Compute the standard Gibbs energy for this reaction. Interpret your answer in terms of whether this redox couple will generate electricity under standard conditions

Expert Solution

Step 1

The standard cell potential can be calculated by the following equation.

$\begin{array}{rcl} {E^{0}}_{cell} & = & {E^{0}}_{cathode} - {E^{0}}_{anode} \\ {E^{0}}_{cell} & = & standard cell potential \\ {E^{0}}_{cathode} & = & reduction potential of cathode \\ {E^{0}}_{anode} & = & reduction potential of anode \end{array}$

At cathode reduction occurs and at anode oxidation occurs.

The standard Gibbs energy for this reaction can be calculated as follows.

$\begin{array}{rcl} ∆ {G^{0}}_{cell} & = & - {nFE}^{0}_{cell} \\ ∆ {G^{0}}_{cell} & = & standard Gibbs energy \\ n & = & no of electrons \\ F & = & Faraday' s constant \end{array}$

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