Sindh Class 9 Chemistry Notes Chapter 8 Electrochemistry Mcqs, Question Pdf Download

Chemistry Class 9th Notes Chapter 8 Electrochemistry for Sindh & Karachi board, Mcqs, short questions, fill in the blank, and true-false pdf Download.

Class 9 Chemistry Notes Chapter 8 Electrochemistry Mcqs, Question Pdf Download

Fill in the Blanks

1. The substance used for electrolysis is called     _____  electrolyte________ .
2. When molten sodium chloride is electrolyzed ___ sodium____ is formed at cathode.
3. One Faraday is equivalent to __ 96500______ coulombs.
4. The electrolyte in lead storage battery is______ dilute sulphuric acid_____ .
5. Dry cell is a___ primary_______ cell.

True or False

i) Sugar is an electrolyte.

True

False

ii) Electrolytic conductance is also known as electrolysis.

True

False

iii) Z is called an electrochemical equivalent.

True

False

iv) The unit of electrochemical equivalent is ampere x second.

True

False

v) Daniell cell is a voltaic cell.

True

False

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MCQs Chemistry 9 Chapter 8 Electrochemistry Pdf Download

The electrodes used in the electrolytic cell to carry out the electrolysis of water are made of:?

• Copper
• Carbon
• Graphite
• Platinum

l During electrolysis of which hydrogen is released at the cathode and oxygen is released at the anode?

• NaCl
• HgO
• Water
• H2O2

One Faraday has?

• 92,500 C
• 94,500 C
• 93,9500 C
• 96\,500 C

The deposition of a metal on another metal is called?

• Reduction
• Electrolysis
• Electroplating
• Oxidation

In electroplating, the thing to be electroplated is made the?

• Anode
• Cathode
• Electrolyte
• Electrolytic cell

In which cells, oxidation loss of electrons occurs at the anode, and reduction gain of electrons occurs at the cathode?

• Electrolytic
• Electrochemical
• Secondary
• Primary

Any device that converts chemical energy into electrical energy or electrical energy into chemical energy is called?

• Pencil cell
• Electrolytic cell
• Electrochemical cell
• Photo cell

The branch of chemistry that deals with the study of the relationship between electrical and chemical energy is called?

• Physical chemistry
• Electrochemistry
• Analytical chemistry
• Thermo chemistry

The substance used for electrolysis is called:

• Electrolyte
• None of these
• Non- electrolyte
• Electrolytic solution

Does sodium chloride melt at?

• 800oC
• 700oC
• 850oC
• 75 0oC

Electrodes are made of?

• alloys
• non metals
• metals
• metalloids

The quantity of charge which deposits or liberates exactly one gram equivalent of a substance is?

• Coulomb
• Ampere
• Faraday
• Electro chemical equivalent

The process of coating one metal onto another is called?

• rusting
• electroplating
• none of these
• Electro chemical process

One Faraday is equivalent to?

• 95600 Coulombs
• 96500 Coulombs
• 96550 Coulombs
• 96000 Coulombs

Which one of these is not an electrolyte?

• Acidulated water
• Sugar
• Sodium chloride solution
• Sodium hydroxide solution

The unit of electrochemical equivalent is?

• G/coulomb
• Ampere
• Kg\coulomb
• Coulomb

In the dry cell, the electrolyte is the moist paste off?

• NH4Cl + ZnSO4
• MnO2 + ZnCl2
• NH4CI + MnO2
• NH4Cl ZnCI2

A weak electrolyte is:?

• Sulphruic
• Citric acid
• Nitric acid
• A caustic alkali

The electrolysis of fused sodium chloride is carried out in:?

• Voltaic cell
• Dry cell
• Downs cell
• Galvanic cell

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Class 9 Chemistry Notes for Sindh board Chapter 8 Pdf Download

Q.1) Define the following terms:

• a) Electrolysis
• b) Electrochemical cell
• c) Coulomb
• d) Electrochemical equivalent
• e) Primary cell
• f) Electroplating

Answer:

a) Electrolysis

It is defined as the chemical decomposition of a compound into its components by passing a current through the solution of the compound or in the molten state of the compound.

b) Electrochemical cell

It is a system in which two electrodes are dipped in the solution of an electrolyte that is connected to the battery and generates an electric current.

c) Coulomb

It is the SI unit of electric charge and is defined as the quantity of charge when one ampere of current is passed for one second.

C = ampere time (s)

1 coulomb = 1 A 1s

A coulomb is equivalent to an ampere multiplied by seconds. For example, a current of 0.5 amperes flowing for 80 seconds, gives a charge 0.5 80 = 40 coulombs.

d) Electrochemical equivalent

The electrochemical equivalent of a substance is defined as the weight of the substance deposited or liberated when one coulomb of electric charge is passed through an electrolyte. It is denoted by Z and in the S.I unit, which is expressed in Kg/coulomb. Each element has its electrochemical equivalent.

e) Primary cell

A primary cell is used to convert chemical energy into electrical energy. It is an irreversible cell and is used in flash lights, clocks, calculators, etc.

f) Electroplating:

Electroplating is a method of depositing one metal over the other employing electrolysis.

Read more: Sindh Class 9 Chemistry Notes Chapter 7 Solution and Suspension

Q.2) Predict what would be formed (i) at the anode and (ii) at the cathode when each of the following molten salts is electrolyzed using inert electrodes.

• a) NaCl
• b) MgBr₂
• c) CaCl₂ 

Answer:

a) NaCl: 

At anode:

Cl^– → Cl + e^–

Cl + Cl → Cl₂

At the anode, as chlorine is negatively charged loses an electron and forms a chlorine atom. The two chlorine atoms combine and form chlorine gas. This is called oxidation reaction because here loss of electrons occurs. Chlorine gas is taken out.

At cathode:

Na⁺ + 1e^– → Na

The sodium ions move towards the negative cathode where each ion gains an electron and forms a sodium atom. This is called reduction reaction, here gain of electrons takes place.

b) MgBr₂:

At anode:

Br^– → Br + e^–

Br + Br → Br₂

At the anode, as bromine is negatively charged loses an electron and forms a bromine atom. The two bromine atoms combine and form bromine gas. This is called oxidation reaction because here loss of electrons occurs. Bromine gas is taken out.

At cathode:

Mg₂⁺ + 2e^– → 2Mg

The magnesium ions move towards the negative cathode where each ion gains an electron and form a magnesium atom. This is called reduction reaction, here the gain of electrons is involved.

c) CaCl₂:

At anode:

Cl^– → Cl + e^–

Cl + Cl → Cl₂

At the anode, as chlorine is negatively charged loses an electron and forms a chlorine atom. The two chlorine atoms combine and form chlorine gas. This is called oxidation reaction because here loss of electrons occurs. Chlorine gas is taken out.

At cathode:

Ca₂⁺ + 2e^– → 2Ca

The calcium ions move towards the negative cathode where each ion gains an electron and form a calcium atom. This is called reduction reaction, here gain of electrons is involved.

Q.3) State and explain Faraday’s first law of electrolysis. 

Answer:

Faraday’s First Law of Electrolysis:

According to this law, the chemical deposition at an electrode due to the flow of current through an electrolyte is directly proportional to the quantity of electricity passed through it.

w ∝ A x t

or

w = Z

Where Z is a constant, known as the “electrochemical equivalent” of the substance. If one ampere of current is passed for one second; then w = Z. This means when one ampere of current is passed for one second; then the weight or amount of the substance deposited or liberated is exactly equal to its electrochemical equivalent.

The current in ampere, multiplied by the time in second is known as coulomb which is the electric charge.

Ampere (A) × time (s) = coulomb (C)

Q.4) Calculate the amount of silver deposited when 10 ampere of current is passed for 50 minutes through a solution of AgNO3. (Z of Ag = 0.00118 g/C) 

Answer:

Answer:

Data:

Electric current (A) = 10 A

Time (t) = 50 mints = 50 × 60 = 3000s

Z = 0.00118 g / c

W = ?

Solution:

W = Z × A × t

W = 0.00118 × 10 × 3 × 103

W = 0.00118 × 3 ×104

W = 1.18 ×10-3 × 3 × 104

W = 1.18 × 10 × 3

W = 3.54 × 10

W = 35.4g

Q.5) Describe the construction and working of a dry cell. 

Answer:

Construction of dry cell:

The dry cell batteries are used in many flashlights, toys, and small appliances. The dry cell consists of an anode and cathode. The anode is the zinc metal of the container outside and the cathode is an inert graphite rod at the center of the cell in contact with the mixture of MnO₂ and carbon powder.

The electrolyte is between anode and cathode, which is the mixture of moist NH₄Cl and ZnCl₂. The cell is called a dry cell because there is no free-flowing liquid. The electrolytic solution is thickened by adding the starch into a paste.

The upper portion of the cell is sealed with wax. A carbon or graphite rod is covered with the help of a copper cap to make the electrical contact.

Working of a dry cell:

Zinc and graphite electrodes are connected with a wire. Zn is oxidized to form Zn₂⁺ ions which pass through the paste leaving behind electrons on the Zn container. The electrons move towards the carbon electrode through an external circuit.

Q.6) What happens when an electric current is passed through acidulated water? Give the reactions at two electrodes and mention the products at cathode and anode. 

Answer:

Pure water is a very weak electrolyte. It ionizes to a very small extent. By adding a few drops of an acid toin it, its conductivity improves. When a current is passed through acidulated water through two electrodes, electrolysis takes place and water conducts electricity.

Water ionizes, (OH^–) anions, and (H⁺) cations are produced. Anions carry a negative charge, they move towards the positive electrode. While cations carry a positive charge, they move towards the negative electrode. The reaction on two electrodes will be followed as;

4H₂O → 4H⁺ + 4OH^–

At the cathode:

At cathode, a hydrogen ion gets an electron to become a hydrogen atom. The two hydrogen atoms combine and form hydrogen gas molecules.

4H⁺ + 4e^– → 4H

2H + 2H → 2H₂

Hydrogen gas is taken off from here.

At the anode:

At anode there are two ions SO₂^– and OH^–. As OH^– is easier to oxidize than SO₂^– so it will discharge hydrogen to form water and oxygen gas is liberated at the anode.

4OH^– → 2H₂O + O₂ + 4e^–

Q.7) Predict the net electrolysis reaction when molten NaCl is electrolyzed. 

Answer:

On the industrial scale, molten sodium metal is obtained by the electrolysis of fused NaCl in the Down cell. In this process, sodium “Na” metal is obtained by electrolysis of molten sodium chloride because the solid-state of NaCl does not conduct an electric current. The reason is Na and Cl ions are tightly bound with each other.

Electrolysis Reaction:

A down cell is a circular furnace. In the center, there is a large block of graphite that acts as an anode while the cathode around it is made of iron. The fused NaCl produces Na⁺ and Cl^– ions, which migrate to their respective electrodes. The steel gauze is present between the electrodes which prevents contact between the products. The “Cl^–“ ions are oxidized to give Cl₂ gas at the anode. It is collected over the anode within an inverted cone-shaped structure. The Na⁺ ions are reduced at the cathode and molten Na metal floats on the denser molten salt mixture from where it is collected.

Reaction in the Down cell:
2NaCl ⇔ 2Na⁺ + 2Cl^–
At Anode:
2Cl^– → Cl₂ + 2e^–
At Cathode:
2Na⁺ + 2e^– → 2Na
Overall reaction:
2NaCl → Cl₂ + 2Na

Q.8) Describe the process of nickel plating. 

Answer:
Nickel Electroplating:
A piece of nickel metal is used as the anode. The object which is to be electroplated is used as a cathode. In the cell nickel sulfate (NiSO4) solution is used in which two electrodes anode and cathode are dipped. Nickel sulfate acts as an electrolyte.
The electrodes are connected through a wire to a battery. When electric current passes nickel releases electrons at the anode which go to the cathode through an external circuit. Ni2+ ions move to the cathode where they gain electrons and deposit as nickel metal at the cathode. The process is as follow:
At the anode:
Ni → Ni₂+ + 2e^–
At the cathode:
Ni₂⁺ + 2e^– → Ni

Q.11) What is the difference between a primary and a secondary cell? Give an example of each. Discuss lead-storage battery. 

Answer:

Primary Cell:

A primary cell produces electricity by the use of chemicals. Due to the use of chemicals, the cell becomes worn out. So these cells cannot be used again and again and are not rechargeable also. Primary cells are also non-reversible because they use chemicals to produce electrical energy but supplying electrical energy to the cell cannot reverse the chemical process. For example a dry cell.

Secondary Cell:

On the other hand, the secondary cell is reversible. Electrical energy is produced by the chemical reaction, but when energy is supplied to the cell, the chemical reaction is reversed. So chemical energy is transformed into electrical energy and it can also be stored. These cells are also called storage cells. Example: a car battery.

Lead storage battery:

It is used in automobiles. It is a reversible battery and can be used through repeated cycles of charging and discharging. It is a group of cells that are connected in a series. About six cells are there in one series. Each cell has a 2V voltage and if six cells are connected in a series then the voltage will be 12V.

In lead storage battery electrodes are connected through the wire with the battery. One of the electrodes, the anode, is lead alloy and the other electrode, the cathode, is made up of lead dioxide (PbO₂). The electrodes are dipped into the concentrated 30% sulphuric acid. When the reaction starts, PbSO₄ precipitates and coats both of the electrodes.

In this reaction, water is formed which dilutes the sulphuric acid. Electrons flow in the opposite direction when the current passes. The net cell reaction can be reversed and the battery is recharged.

Q.12) When molten NaCl is electrolyzed. Sodium metal is liberated at the cathode by the reaction Na⁺ + e^– → Na(s).
How many grams of sodium are liberated when 5 x 10³ C of electric charge is passed through the cell.

Answer:
Data:
Atomic mass of sodium = 23
Gain of 1 e^– means 1F electric charge.
                                 1F                   =     96500 C
96500 C electric charge produces = 23 g Na
1 C electric charge produces           = 23 / 96500
5 x 103 C electric charge produces = 23 / 96500 x 5 x 103
                                                          = 0.00119 x 103 = 1.19 g Na

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