   Chapter 18, Problem 133AE

Chapter
Section
Textbook Problem

# An aqueous solution of an unknown salt of ruthenium is electrolyzed by a current of 2.50 A passing for 50.0 min. If 2.618 g Ru is produced at the cathode, what is the charge on the ruthenium ions in solution?

Interpretation Introduction

Interpretation:

The electrolysis of the unknown salt of Ruthenium is given. The charge on Ruthenium ions in solution for a given amount of metal produced at the electrode 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=Molarmassn×96,485

To determine: The charge on Ruthenium ions in solution for a given amount of metal produced at the electrode is to be calculated.

Explanation

Given,

The amount of current passed is 2.50A .

The time period is 50.0min .

The amount of gas produced is 2.618g .

The conversion of min to s is done as,

1min=60s

Conversion of 50.0min to s is done as,

50.0min=50×60s=3000s

The value of E is given as,

E=Molarmassn

Where,

• n is the number of electrons exchanged.
• E is the equivalent weight.

Molar mass of Ruthenium is 101.07g/mole .

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

E=Molarmassn=101.07gmolen

The value of Z is given as,

Z=Molarmassn×96,485Cmolee=E96,485Cmolee

Where,

• Z is the electrochemical equivalent.

Substitute the value of E in the above equation as,

Z=E96,485Cmolee=101

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