An aqueous solution of PdCl 2 is electrolyzed for 48.6 seconds, and during this time 0.1064 g of Pd is deposited on the cathode. What is the average current used in the electrolysis?

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Interpretation Introduction Interpretation: The average current used in the electrolysis of PdCl 2 is to be calculated. Concept introduction: The non-spontaneous reaction takes place in an electrolytic cell in which there occurs conversion of electrical energy into chemical energy and this is used for the electrolysis of a metal. The charge generated in the cell is calculated as, Q = I t When electricity is passed through an electrolytic cell, at that time the amount of the substance that is liberated at an electrode is given by, W = Z Q = Z I t The value of Z is given as, Z = Molar mass n × 96 , 485 To determine: The average current used in the electrolysis of PdCl 2 . Explanation Given, The time period is 48.6 s . The amount of metal deposited is 0.1046 g . The reaction of Pd 2 + during electrolysis is, Pd 2 + + 2 e − → Pd For the reduction of one Pd 2 + 2 electrons are required. Molar mass of Palladium is 106.42 g / mole The value of E is given as, E = Molar mass n Where, n is the number of electrons exchanged. E is the equivalent weight. Substitute the value of the molar mass of Palladium in the above equation as, E = Molar mass n = 106.42 g mole 2 e − The value of Z is given as, Z = Molar mass n × 96 , 485 = E 96 , 485 C mole e − Where, Z is the electrochemical equivalent. Substitute the value of E in the above equation as, Z = E 96 , 485 C mole e − = 106

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Chemistry: An Atoms First Approach

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Steven S. Zumdahl + 1 other

Publisher: Cengage Learning

ISBN: 9781305079243

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Interpretation Introduction

Interpretation:

The average current used in the electrolysis of PdCl2 is to be calculated.

Concept introduction:

The non-spontaneous reaction takes place in an electrolytic cell in which there occurs conversion of electrical energy into chemical energy and this is used for the electrolysis of a metal.

The charge generated in the cell is calculated as,

Q=It

When electricity is passed through an electrolytic cell, at that time the amount of the substance that is liberated at an electrode is given by,

W=ZQ=ZIt

The value of Z is given as,

Z=Molar massn×96,485

To determine: The average current used in the electrolysis of PdCl2 .

Explanation of Solution

Given,

The time period is 48.6 s .

The amount of metal deposited is 0.1046 g .

The reaction of Pd2+ during electrolysis is,

Pd2++2e−→Pd

For the reduction of one Pd2+ 2 electrons are required.

Molar mass of Palladium is 106.42 g/mole

The value of E is given as,

E=Molar massn

Where,

n is the number of electrons exchanged.

E is the equivalent weight.

Substitute the value of the molar mass of Palladium in the above equation as,

E=Molar massn=106.42 gmole2 e−

The value of Z is given as,

Z=Molar massn×96,485=E96,485 Cmole e−

Where,

Z is the electrochemical equivalent.

Substitute the value of E in the above equation as,

Z=E96,485 Cmole e−=106

An aqueous solution of PdCl 2 is electrolyzed for 48.6 seconds, and during this time 0.1064 g of Pd is deposited on the cathode. What is the average current used in the electrolysis?

Chemistry: An Atoms First Approach

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Chemistry: An Atoms First Approach

An aqueous solution of PdCl₂ is electrolyzed for 48.6 seconds, and during this time 0.1064 g of Pd is deposited on the cathode. What is the average current used in the electrolysis?

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An aqueous solution of PdCl 2 is electrolyzed for 48.6 seconds, and during this time 0.1064 g of Pd is deposited on the cathode. What is the average current used in the electrolysis?

Chemistry: An Atoms First Approach

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Chemistry: An Atoms First Approach