   # A zinc-copper battery is constructed at follows at 25°C: Zn | Zn 2 + ( 0.10 M ) | | Cu 2 + ( 2.50 M ) | Cu The mass of each electrode is 200. g. a. Calculate the cell potential when this battery is first connected. b. Calculate the cell potential after 10.0 A of current has flowed for 10.0 h. (Assume each half-cell contains 1.00 L of solution.) c. Calculate the mass of each electrode after 10.0 h. d. How long can this battery deliver a current of 10.0 A before it goes dead? ### Chemistry: An Atoms First Approach

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

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 17, Problem 144CP
Textbook Problem
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## A zinc-copper battery is constructed at follows at 25°C: Zn | Zn 2 + ( 0.10 M ) |   | Cu 2 + ( 2.50   M ) |   Cu The mass of each electrode is 200. g.a. Calculate the cell potential when this battery is first connected.b. Calculate the cell potential after 10.0 A of current has flowed for 10.0 h. (Assume each half-cell contains 1.00 L of solution.)c. Calculate the mass of each electrode after 10.0 h.d. How long can this battery deliver a current of 10.0 A before it goes dead?

(a)

Interpretation Introduction

Interpretation: The cell potential Ecell of the given cell, the mass of each electrode after 10.0 h and the time of the given battery to deliver a current of 10.0 A before it goes dead is to be calculated.

Concept introduction: Cell potential is defined as the measure of energy per unit charge available from the redox reaction to carry out the reaction. The electrochemical equivalent is defined as the mass of the element transported when electricity of one coulomb charge is passed.

To determine: The cell potential of the given cell when the battery is connected.

### Explanation of Solution

Explanation

Given

The molar concentration of Zn2+ is (0.10 M) .

The molar concentration of Cu2+ is (2.50 M) .

The half cell reactions for the cell are,

Zn+2+2eZn                      E1ο=0.76 V (1)

Cu+2+2eCu                          E2ο=0.34 V (2)

Where,

• E1ο is the standard electrode potential of equation (1).
• E2ο is the standard electrode potential of equation (2).

The overall cell reaction is,

Zn+Cu+2Zn2++Cu (3)

The standard electrode potential of equation (3) is calculated by the formula,

Ecellο=E2οE1ο

Where,

• Ecellο is the standard electrode potential of equation (3).

Substitute the values of E1ο and E2ο in the above formula

(b)

Interpretation Introduction

Interpretation: The cell potential Ecell of the given cell, the mass of each electrode after 10.0 h and the time of the given battery to deliver a current of 10.0 A before it goes dead is to be calculated.

Concept introduction: Cell potential is defined as the measure of energy per unit charge available from the redox reaction to carry out the reaction. The electrochemical equivalent is defined as the mass of the element transported when electricity of one coulomb charge is passed.

To determine: The cell potential after 10.0 A of current has flowed for 10.0 h .

(c)

Interpretation Introduction

Interpretation: The cell potential Ecell of the given cell, the mass of each electrode after 10.0 h and the time of the given battery to deliver a current of 10.0 A before it goes dead is to be calculated.

Concept introduction: Cell potential is defined as the measure of energy per unit charge available from the redox reaction to carry out the reaction. The electrochemical equivalent is defined as the mass of the element transported when electricity of one coulomb charge is passed.

To determine: The mass of each electrode after 10.0 h .

(d)

Interpretation Introduction

Interpretation: The cell potential Ecell of the given cell, the mass of each electrode after 10.0 h and the time of the given battery to deliver a current of 10.0 A before it goes dead is to be calculated.

Concept introduction: Cell potential is defined as the measure of energy per unit charge available from the redox reaction to carry out the reaction. The electrochemical equivalent is defined as the mass of the element transported when electricity of one coulomb charge is passed.

To determine: The time of the given battery to deliver a current of 10.0 A before it goes dead.

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