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Calculate values for the following cells. Which reactions are spontaneous as written (under standard conditions)? Balance the equations that are not already balanced. Standard reduction potentials are found in Table 17-1. a. H 2 ( g ) → H + ( a q ) + H − ( a q ) b. Au 3 + ( a q ) + Ag ( s ) → Ag + ( a q ) + Au ( s )

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Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

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BuyFindarrow_forward

Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 17, Problem 48E
Textbook Problem
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Calculate Chapter 17, Problem 48E, Calculate values for the following cells. Which reactions are spontaneous as written (under standard values for the following cells. Which reactions are spontaneous as written (under standard conditions)? Balance the equations that are not already balanced. Standard reduction potentials are found in Table 17-1.

a. H 2 ( g ) H + ( a q ) + H ( a q )

b. Au 3 + ( a q ) + Ag ( s ) Ag + ( a q ) + Au ( s )

(a)

Interpretation Introduction

Interpretation:

The reactions taking place in two different galvanic cells are given. The E° of the given galvanic cells, the spontaneity of the reactions and balanced chemical equation for each cell is to be stated.

Concept introduction:

The galvanic cell converts chemical energy into electrical energy while the electrolytic cell converts electrical energy into chemical energy.

The species at anode undergoes oxidation while the species at cathode undergoes reduction and the electrons generated at the anode are transferred through wire to the cathode.

To determine: The set up of the cell given in the chemical equation and the direction of electron flow, identification of the cathode and anode and balanced chemical equation.

Explanation of Solution

The value of E°cell is calculated as -2.23V_ .

The reaction taking place at cathode is,

H2(g)+2e2H(aq)E°red=2.23V

The reaction taking place at anode is,

H2(g)2H+(aq)+2eE°ox=0.00V

Add both the oxidation and reduction half-reaction,

H2(g)+2e2H(aq)H2(g)2H+(aq)+2e

The final equation is,

H2(g)H(aq)+H+(aq)

The overall cell potential is calculated as,

E°cell=E°ox+E°red=0

(b)

Interpretation Introduction

Interpretation:

The reactions taking place in two different galvanic cells are given. The E° of the given galvanic cells, the spontaneity of the reactions and balanced chemical equation for each cell is to be stated.

Concept introduction:

The galvanic cell converts chemical energy into electrical energy while the electrolytic cell converts electrical energy into chemical energy.

The species at anode undergoes oxidation while the species at cathode undergoes reduction and the electrons generated at the anode are transferred through wire to the cathode.

To determine: The set up of the cell given in the chemical equation and the direction of electron flow, identification of the cathode and anode and the balanced chemical equation.

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Chapter 17 Solutions

Chemistry: An Atoms First Approach
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