How many faradays are required for each of the following processes? How many coulombs arc required?
- a Reduction of 5.0 mol Na+ to Na
- b Reduction of 5.0 mol Cu2+ to Cu
- c Oxidation of 6.0 g H2O to O2
- d Oxidation of 6.0 g Cl− to Cl2
(a)
Interpretation:
The amount of Faraday currents and coulombs charges are required to reduction of given mole of species should be calculated.
Concept introduction:
Faraday:
Faraday is a unit for electric charge, which is equal to the Faraday’s constant and it is given by
Faraday’s constant:
One mole (Avogadro's number) of electrons containing electrical charge is given by the ratio of number of electrons per mole with number of electrons per coulomb and it is,
In the redox reaction, a species gains electron from its reaction mixture to get reduced while during the reaction is known as reduction.
In the redox reaction, a specie loss it’s of electron to get oxidized while during the reaction is known as reduction.
The charge of the species where decreases, while reduction occurs.
In the electro reduction process, the coulombs is given by the amount of charge required to reduction of given mole of species.
In the electro oxidation process, the coulombs is given by the amount of charge required to oxidation of given mole of species.
Answer to Problem 19.113QP
Reduction of
Reduction of
Explanation of Solution
Given:
Reduction of
In above reduction 1 mole of electron required to reduce
The amount of faradays required is,
The mole of electron required reducing
Reduction of
The amount of coulombs required is,
The calculated Faraday is plugged in above equation to give a coulombs charge reduction of
Reduction of
(b)
Interpretation:
The amount of Faraday currents and coulombs charges are required to reduction of given mole of species should be calculated.
Concept introduction:
Faraday:
Faraday is a unit for electric charge, which is equal to the Faraday’s constant and it is given by
Faraday’s constant:
One mole (Avogadro's number) of electrons containing electrical charge is given by the ratio of number of electrons per mole with number of electrons per coulomb and it is,
In the redox reaction, a species gains electron from its reaction mixture to get reduced while during the reaction is known as reduction.
In the redox reaction, a specie loss it’s of electron to get oxidized while during the reaction is known as reduction.
The charge of the species where decreases, while reduction occurs.
In the electro reduction process, the coulombs is given by the amount of charge required to reduction of given mole of species.
In the electro oxidation process, the coulombs is given by the amount of charge required to oxidation of given mole of species.
Answer to Problem 19.113QP
Reduction of
Reduction of
Explanation of Solution
Given:
Reduction of
In above reduction 2 moles of electrons required to reduce
The amount of faradays required is,
The moles of electrons required to reduce
Reduction of
The amount of coulombs required is,
The calculated Faraday is plugged in above equation to give a coulombs charge reduction of
Reduction of
(c)
Interpretation:
The amount of Faraday currents and coulombs charges are required to reduction of given mole of species should be calculated.
Concept introduction:
Faraday:
Faraday is a unit for electric charge, which is equal to the Faraday’s constant and it is given by
Faraday’s constant:
One mole (Avogadro's number) of electrons containing electrical charge is given by the ratio of number of electrons per mole with number of electrons per coulomb and it is,
In the redox reaction, a species gains electron from its reaction mixture to get reduced while during the reaction is known as reduction.
In the redox reaction, a specie loss it’s of electron to get oxidized while during the reaction is known as reduction.
The charge of the species where decreases, while reduction occurs.
In the electro reduction process, the coulombs is given by the amount of charge required to reduction of given mole of species.
In the electro oxidation process, the coulombs is given by the amount of charge required to oxidation of given mole of species.
Answer to Problem 19.113QP
Oxidation of
Oxidation of
Explanation of Solution
Given:
Oxidation of
In above Oxidation 4 moles of electrons required to reduce
The amount of faradays required is,
The molar mass of water is
The molar mass, mole of electron required oxidizing
Oxidation of
The amount of coulombs required is,
The calculated Faraday is plugged in above equation to give a coulombs charge Oxidation of
Oxidation of
(d)
Interpretation:
The amount of Faraday currents and coulombs charges are required to reduction of given mole of species should be calculated.
Concept introduction:
Faraday:
Faraday is a unit for electric charge, which is equal to the Faraday’s constant and it is given by
Faraday’s constant:
One mole (Avogadro's number) of electrons containing electrical charge is given by the ratio of number of electrons per mole with number of electrons per coulomb and it is,
In the redox reaction, a species gains electron from its reaction mixture to get reduced while during the reaction is known as reduction.
In the redox reaction, a specie loss it’s of electron to get oxidized while during the reaction is known as reduction.
The charge of the species where decreases, while reduction occurs.
In the electro reduction process, the coulombs is given by the amount of charge required to reduction of given mole of species.
In the electro oxidation process, the coulombs is given by the amount of charge required to oxidation of given mole of species.
Answer to Problem 19.113QP
Oxidation of
Oxidation of
Explanation of Solution
Given:
Oxidation of
In above Oxidation 2 moles of electrons required to oxidizing
The amount of faradays required is,
The molar mass of Chlorine is
The molar mass, mole of electron required oxidizing
Oxidation of
The amount of coulombs required is,
The calculated Faraday is plugged in above equation to give a coulombs charge oxidation of
Oxidation of
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Chapter 19 Solutions
General Chemistry (Instructor's)
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