How long will it take to plate out each of the following with a current of 100.0 A? a. 1.0 kg AI from aqueous Al 3+ b. 1.0 g Ni from aqueous Ni 2+ c. 5.0 moles of Ag from aqueous Ag +

Interpretation:

The time taken to plate out each of each of given metal with a current of 100.0 A 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=Atomic massn×96,485

The mass of metal is calculated by multiplying the moles of metal with its atomic molar mass. This gives the mass of the metal to be plated out in the electrolytic cell.

To determine: The time taken to plate out 1.0 kg Al from aqueous Al3+ with a current of 100 A .

Given

The mass of aluminum to be plated out is 1.0 kg .

The current passed to plate out the metal is 100 A .

The reaction involved is,

Al3++3e−→Al

The conversion of each Al3+ to convert to Al requires 3 electrons.

The number of moles of Al atoms present in 27 g of Al is 1 mol .

The number of moles of Bi atoms present in 1000 g of Al is,

1000 g Al×1 mol Al27 g Al=37.04 mol Al

The number of electrons required to convert to 37.04 mol Al is,

37.04×3=111.12 mol e−

The quantity of charge that is carried by these electrons is,

111.12 mol e−×96,485mol e−=10.72×106 C

The charge generated in the cell is calculated as,

Q=It

Where,

• Q is the charge carried in the cell.
• I is the current in amperes

Interpretation:

The time taken to plate out each of each of given metal with a current of 100.0 A 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=Atomic massn×96,485

The mass of metal is calculated by multiplying the moles of metal with its atomic molar mass. This gives the mass of the metal to be plated out in the electrolytic cell.

To determine: The time taken to plate out 1.0 g Ni from aqueous Ni2+ with a current of 100 A .

Interpretation:

The time taken to plate out each of each of given metal with a current of 100.0 A 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=Atomic massn×96,485

The mass of metal is calculated by multiplying the moles of metal with its atomic molar mass. This gives the mass of the metal to be plated out in the electrolytic cell.

To determine: The time taken to plate out 5.0 moles of Ag from aqueous Ag+ with a current of 100 A .