Electrode where reduction takes place and electrons are gained.

Electrode where oxidation takes place and electrons are lost.

Electrode where reduction takes place and electrons are lost.

A fluid that conducts electricity.

Electrode where oxidation takes place and electrons are gained.

When metal is created through chemical reactions

When metal is gradually destroyed through chemical reactions

When a metal is destroyed after exposure to a gas

When a solid is destroyed through chemical reactions

MCQ Questions for Class 12 Engineering Chemistry Electrochemistry Quiz 1

Select among the following statements that characterize a galvanic cell?
I: Oxidation occurs at the anode, which is negative.
II: Oxidation occurs at the anode, which is positive.
III. Reduction occurs at the cathode, which is positive.

0%
II only
0%
III only
0%
I and III
0%
I, II and III
0%
II and III

Assertion: The anions migrate to the cathode in an electrolytic cell.
Reason: Positively charged ions are attracted to the negatively charged cathode.

0%
Both Assertion and Reason are true and Reason is the correct explanation of Assertion
0%
Both Assertion and Reason are true but Reason is not the correct explanation of Assertion
0%

Assertion is true but Reason is false
0%

Assertion is false but Reason is true
0%

Both Assertion and Reason are false

In electrochemical corrosion. the metal undergoing corrosion :

0%
acts as anode
0%
acts as cathode
0%
undergoes reduction
0%
liquifies

Zn(s)|ZnCl

$_2$ (aq)|Cl

$^-$ (aq)|Cl

$_2$ (g)|C(s)
According to the above cell diagram the electrochemical cell described, the reaction at anode is :

0%
Zn $\rightarrow$ Zn $^{2+}$ + 2e $^-$
0%
Zn $^{2+}$ + 2e $^-$ $\rightarrow$ Zn
0%
Cl $_2$ + 2e $^-$ $\rightarrow$ 2Cl $^-$
0%
2Cl $^-$ $\rightarrow$ Cl $_2$ + 2e $^-$
0%
Zn + Cl $_2$ $\rightarrow$ ZnCl $_2$

Explanation

At anode, zinc is oxidized to Zn(II) ions.

$\displaystyle Zn \rightarrow Zn^{2+} + 2e^-$
In the cell diagram, the electrode on left hand side is anode and the electrode on right hand side is cathode. Oxidation occurs at anode and reduction occurs at cathode.

$Zn\left( s \right) \left| Zn{ Cl }_{ 2 }\left( aq \right) \right| \left| { Cl }^{ - }\left( aq \right) \right| \left| { Cl }_{ 2 }\left( g \right) \right| C\left( s \right)$
The reaction at anode in the electrochemical cell is:

0%
$Zn\rightarrow { Zn }^{ 2+ }+2e$
0%
${ Zn }^{ 2+ }+2e\rightarrow Zn$
0%
${ Cl }_{ 2 }+2e\rightarrow 2{ Cl }^{ - }$
0%
$2{ Cl }^{ - }\rightarrow { Cl }_{ 2 }+2e$
0%
$Zn+{ Cl }_{ 2 }\rightarrow Zn{ Cl }_{ 2 }$

Explanation

The reaction at anode in the electrochemical cell is

$\displaystyle Zn\rightarrow { Zn }^{ 2+ }+2e$
It is an oxidation reaction
The reaction at cathode in the electrochemical cell is

$\displaystyle { Cl }_{ 2 }+2e\rightarrow 2{ Cl }^{ - }$
It is a reduction reaction.
In the cell notation, the left hand electrode is anode where oxidation half reaction occurs.
The right hand electrode is cathode where reduction half reaction occurs.

What is a cathode?

0%
Electrode where reduction takes place and electrons are gained.
0%
Electrode where oxidation takes place and electrons are lost.
0%
Electrode where reduction takes place and electrons are lost.
0%
A fluid that conducts electricity.
0%
Electrode where oxidation takes place and electrons are gained.

Which half-cell reactions describes what is going on at the anode, from the diagram ?

0%
$Zn\rightarrow Zn^{2+} + 2e^{-}$
0%
$H_{2} \rightarrow 2H^{+} + 2e^{-}$
0%
$2Cl^{-} \rightarrow Cl_{2} + 2e^{-}$
0%
$SO^{4-} \rightarrow S + 2O2 + 6e^{-}$
0%
$2H^{+} + 2e^{-} \rightarrow H_{2}$

Explanation

At anode, zinc is oxidized to Zn(II) ions. Loss of electrons is oxidation.

$\displaystyle Zn\rightarrow Zn^{2+} + 2e^{-}$

What is the correct formula for determining the voltage of an electrochemical cell?

0%
$E^{0}_{cell}$ = $E^{0}_{cathode}$ - $E^{0}_{anode}$
0%
$E^{0}_{cell}$ = $E^{0}_{cathode}$ + $E^{0}_{anode}$
0%
$E^{0}_{constant}$ = $E^{0}_{cathode}$ - $E^{0}_{anode}$
0%
$E^{0}_{constant}$ = $E^{0}_{cathode}$ + $E^{0}_{anode}$
0%
$E^{0}_{cell}$ = - $E^{0}_{cathode}$ + $E^{0}_{anode}$

What two metals are often used in electrochemical cells?

0%
Zinc and copper
0%
Zinc and sulfur
0%
Carbon and copper
0%
Zinc and carbon
0%
Sulfur and copper

At anode of an electrochemical cell, which of the following change may occur?

0%
$\displaystyle { Cu }^{ 2+ }$ to $\displaystyle Cu$
0%
$\displaystyle Cl{ O }_{ 3 }^{ - }$ to $\displaystyle Cl{ O }^{ - }$
0%
$\displaystyle { Cl }^{ - }$ to $\displaystyle { Cl }_{ 2 }$
0%
$\displaystyle { H }^{ + }$ to $\displaystyle { H }_{ 2 }$
0%
$\displaystyle { O }_{ 2 }$ to $\displaystyle { H }_{ 2 }O$

Explanation

At anode of an electrochemical cell, the following change may occur.

$\displaystyle \displaystyle { Cl }^{ - }$ may be oxidized to

$\displaystyle Cl_2$ .

$\displaystyle \displaystyle { Cl }^{ - } \rightarrow \dfrac {1}{2} Cl_2 + e^-$

$\displaystyle \displaystyle { Cl }^{ - }$ iond have lower discharge potential than hydroxide ions. Hence,

$\displaystyle \displaystyle { Cl }^{ - }$ ions are preferentially liberated at anode.

Which of the following will not occur in a voltaic cell while a chemical reaction is on a spontaneous process?

0%
The electrons will migrate through the wire
0%
The cations in the salt bridge will migrate to the anode half-cell
0%
The cathode will gain mass
0%
The anode will lose mass
0%
Reduction will occur at the cathode

Explanation

The anions in the salt bridge will migrate to the anode half-cell not cations so option

$B$ is not true.

What is corrosion?

0%
When metal is gradually destroyed through chemical reactions
0%
When metal is created through chemical reactions
0%
When a redox reaction takes place
0%
When a metal is destroyed after exposure to a gas
0%
When a solid is destroyed through chemical reactions

Explanation

Corrosion occurs when a redox reaction takes place.

Corrosion is a natural process, which converts a refined metal to a more chemically-stable form, such as its oxide, hydroxide, or sulfide. It is the gradual destruction of materials by chemical and/or electrochemical reaction with their environment.

It also gradually destroys the element through chemical reactions

Hence, the correct options are

$A$ and

$C$

Assertion: Input of energy is required by electrolytic cells.

Reason: Electrolytic cells have just one container, while voltaic cells have two.

0%
Both Assertion and Reason are true and Reason is the correct explanation of Assertion
0%
Both Assertion and Reason are true but Reason is not the correct explanation of Assertion
0%
Assertion is true but Reason is false
0%
Assertion is false but Reason is true
0%
Both Assertion and Reason are false

For the following reactions:

$Zn \rightarrow Zn^{2+} + 2e^-; E=+0.76 V$

$Au \rightarrow Au^{3+} + 3e^-; E=-1.42 V$
If gold foil is placed in a solution containing

$Zn^{2+}$ , the reaction potential would be:

0%
$-1.34 V$
0%
$-2.18 V$
0%
$-0.66 V$
0%
$+2.18 V$
0%
$+1.34 V$

Explanation

If gold foil is placed in a solution containing

$Zn^{2+}$ , Gold will be reduced and Zinc will be oxidised and the following reaction will take place:

$3Zn+2Au^{3+}\rightarrow 3Zn^{2+}+2Au$

The reaction potential for the above reaction is given by :

$E=E_{cathode}-E_{anode}=-1.42-0.76=-2.18 \ V$

Which of these statements best describes a galvanic cell?

0%
Reduction occurs at the anode.
0%
Oxidation occurs at the anode.
0%
Energy is required from an external source.
0%
The thode is negative.
0%
$E^o_{cell}$ is negative.

Electrolysis of water to form hydrogen and oxygen gas is called __________.

0%
precipitation
0%
oxidation-reduction
0%
distillation
0%
hydration
0%
condensation

Explanation

Electrolysis of water to form hydrogen and oxygen gas is called oxidation-reduction.

$\displaystyle 2H_2O \rightarrow 2H_2 + O_2$
Hydrogen ions (protons) are reduced.

$\displaystyle 2H^+ + 2e^- \rightarrow H_2$
Hydroxide ions are oxidised.

$\displaystyle 4OH^- \rightarrow 2H_2O + O_2 + 4e^-$

Which of the following is true for an electrolytic cell?

0%
An electric current causes an otherwise nonspontanteous chemical reaction to occur.
0%
Reduction occurs at the anode.
0%
A spontaneous electrochemical reaction produces an electric current.
0%
The electrode to which electrons flow is where oxidation occurs.
0%
None of the above

Explanation

For electrolytic cell following are true statements:

(a) Nonspontaneous Reduction.

(b) electrical energy

$\rightarrow$ chemical energy

$+ve$ charged electrode)

Reduction at cathode (

$-ve$ charged electrode)

A battery jar contained a solution of copper sulfate. Two electrodes. one made of copper the other a metal object to be copper plated, were placed in the jar and connected to a source of direct current. Which of the following statements concerning this system is correct?

0%
The object to be placed is the anode
0%
Oxidation occurs at the anode
0%
The sulfate ions migrate toward the cathode
0%
The concentration of the copper sulfate solution increases as electrolysis proceeds
0%
The copper electrode increases in mass.

Explanation

In electrolytic cell, for

$Cu^{2+}$ ions to get deposited at metal, metal sould have negative charge, i.e. it should act as cathode. Oxidation always occurs at anode. Sulphate ions will migrate towards anode as anode will have positive charge. Concentration of

$CuSO_4$ decreases as electrolysis proceeds and the copper electrode decreases in mass.

In the electrolysis of molten copper chloride, the substance liberated at the anode is __________ .

0%
copper
0%
chlorine
0%
hydrogen
0%
copper chloride
0%
none of the above

Explanation

In the electrolysis of molten copper chloride, the substance liberated at the anode is chlorine and the substance deposited at cathode is copper.
Oxidation at anode:

$\displaystyle 2Cl^-(aq) \rightarrow Cl_2(g) + 2e^-$
Reduction at cathode:

$\displaystyle Cu^{2+}(aq) + 2e^- \rightarrow Cu(s)$

Choose the correct statement from the following:

0%
Cations move towards cathode during the process of electrolysis
0%
Electrolysis is the process of decomposition of a electrolyte by the action of electric currrent
0%
SI unit of chemical equivalent is kg
0%
One faraday = 96500 coulombs

Explanation

Cations are positive charge and cathode are negative charge, so cation moves toward anode.

The process of decomposition of electrolyte by electric field (current ) is called electrolysis.

$F=\dfrac{E}{Z}$ ,E=chemical equivalent, Z=electro chemical equivalent

$1F=96500 C$ .

Si unit of chemical equivalent is

$E=\dfrac{M}{V}$ , V= valence electron and M =mass, V is dimensionless ,So unit of E is equivalent to kg

In the electrochemical cell shown above, which of the following half-reactions occurs at the anode?

0%
$\displaystyle { Cu }^{ 2+ }+e\rightarrow { Cu }^{ - }$
0%
$\displaystyle Zn\left( s \right) \rightarrow { Zn }^{ 2+ }+2e$
0%
$\displaystyle { Zn }^{ 2+ }+2e\rightarrow Zn\left( s \right)$
0%
$\displaystyle Cu\left( s \right) \rightarrow { Cu }^{ 2+ }+2e$
0%
$\displaystyle { Cu }^{ 2+ }+2e\rightarrow Cu\left( s \right)$
$\displaystyle$

Explanation

At anode, oxidation will take place and

$Zn(s)$ will get oxidised to

$Zn^{2+}$ leaving negatively charged electrons, making anode negatively charged, repelling negatively charged

$NO_3^-$ .

Which of these half-reactions represents an oxidation?
I.

$Sn^{4+} \rightarrow Sn^{2+}$
II.

$MnO_4^-\rightarrow Mn^{2+}$
III.

$Cl_2\rightarrow ClO_3^-$

0%
I only
0%
II only
0%
III only
0%
I and II only
0%
II and III only

Explanation

Oxidation state of

$Sn$ changes from

$+4$ to

$+2$

Oxidation state of

$Mn$ changes from

$+7$ to

$+2$

Oxidation state of

$Cl$ changes from

$0$ to

$+7$

Therefore reaction

$III$ represents oxidation.

An iron nail, solid iron metal, rusts. What type of reaction is it?

0%
Decomposition
0%
Synthesis
0%
Combustion
0%
Single replacement

Explanation

$2Fe+O_2\rightarrow FeO$ (rust)

Two compounds produce a single compound by reacting with each other. This is called as a synthesis reaction by the definition of synthesis reaction.

A secondary cell is one that :

0%
can be recharged
0%
can be recharged by passing current through it in the same direction
0%
can be recharged by passing current through it in the opposite direction
0%
can not be recharged

In the galvanic cell :

$Zn/Zn^{2+} (C_1)||Cu^{2+} (C_2)/Cu$

$E_{cell} - E_{cell}^o = +0.0591 V$ . The value of

$\dfrac{C_1}{C_2}$ at

$298\ K$ is:

0%
$10^{-1}$
0%
$10^{2}$
0%
$10^{-2}$
0%
$10$

Explanation

$\displaystyle E_{cell} - E_{cell}^o = +0.0591 V$

$\displaystyle E_{cell} = E_{cell}^o +0.0591 V$
But

$\displaystyle E_{cell} = E_{cell}^o - \dfrac {0.0591}{n} log \dfrac {C_1}{C_2}$
Hence,

$\displaystyle +0.0591 = - \dfrac {0.0591}{2} log \dfrac {C_1}{C_2}$

$\displaystyle log \dfrac {C_1}{C_2} =-2$

$\displaystyle \dfrac {C_1}{C_2} = 10^{-2}$
Hence, option (C) is the correct answer.

Which expression gives the correct value for the standard potential for a gold-rhodium voltaic cell?

Half-reaction	$E^{\circ}(V)$
$Rh_{(aq)}^{+3} + 3e^{-} \rightarrow Rh_{(s)}$	$0.76\ V$
$Au_{(aq)}^{+} + e^{-} \rightarrow Au_{(s)}$	$1.69\ V$

0%
$1.69\ V + 0.76\ V$
0%
$1.69\ V - 0.76\ V$
0%
$3(1.69)\ V + 0.76\ V$
0%
$3(1.69)\ V - 0.76\ V$

Explanation

We know that, metal having higher reduction potential undergoes reduction;

so, Au will undergo reduction and Rh will undergo oxidation.

$E^0_{cell}$ = 1.69 V - 0.76 V

_________ is an application of electrolysis.

0%
Oxidation
0%
Electrotyping
0%
Electric shielding
0%
Electric polishing.

During electrolysis negative terminal used is called anode.

0%
True
0%
False

Explanation

In electrolysis, the two wires or plates dipping into the electrolyte are called electrodes. The electrode which is connected to the positive terminal of the cell or battery is called the anode. The electrode which is connected to the negative terminal of the battery is called the cathode.

Hence, option

$B$ is correct.

State True or False.

In an electrochemical cell, in the inner circuit current is carried by ions and in the external circuit, current of electrons flows through the metal conductors.

0%
True
0%
False

Splitting a compound using electricity is called:

0%
electrolysis
0%
electrolyte
0%
electrokinesis
0%
none of the above

In electrolysis, mass of the substance liberated at cathode is proportional to

0%
strength of the current passed.
0%
time of passage of current.
0%
quantity of electricity passed.
0%
none of these

Explanation

According to the first law of electrolysis the mass of of substance liberated at cathode is proportional to the quantity of electric charge passed through it or indirectly it's proportional to the quantity of electricity passed.

$\because$

$m= k \times q$

Examine the drawing of an electrolytic cell shown:

Determine the time it would take to plate

$10.0\ g\ Ag$ with a current of

$0.452A$ .

0%
$2.5\ hr$
0%
$3.5\ hr$
0%
$4.5\ hr$
0%
$5.5\ hr$

Explanation

we have,

$w = \dfrac{E * I*t}{96500}$

$w = \dfrac{Molecular weight * I*t}{1*96500}$

$10 = \dfrac{108 * 0.452 * t}{96500}$

$t = 19768.10\, sec\, or\, 5.49 hrs$

Which of the following represents the oxidation half-reaction for the unbalanced redox equation?

$Cu + HNO_{3} \rightarrow Cu (NO_{3})_{2} + NO_{2}$

0%
$Cu^{2+} + 2e^{-} \rightarrow Cu$
0%
$Cu \rightarrow Cu^{2+} + 2e^{-}$
0%
$NO_{3}^{-} \rightarrow NO_{2} + 1e^{-}$
0%
$2H^{+} + NO_{2}^{-} + 1e^{-} \rightarrow NO_{2} + H_{2}O$

Explanation

$Cu+HNO_3 \longrightarrow Cu(NO_3)_2+NO_2$

As Oxidation of

$Cu$ is taking place in the reaction.

Thus the oxidation half-cell reaction will be

$Cu \longrightarrow Cu^{+2}+2e^-$

If the

${ E }_{ cell }^{ o }$ for a given reaction has a negative value then which of the following gives the correct relationships for the values of

$\Delta { G }^{ o }$ and

${ K }_{ eq }$ ?

0%
$\Delta { G }^{ o } < 0; { K }_{ eq } > 1$
0%
$\Delta { G }^{ o } < 0; { K }_{ eq } < 1$
0%
$\Delta { G }^{ o } > 0; { K }_{ eq } < 1$
0%
$\Delta { G }^{ o } > 0; { K }_{ eq } > 1$

Explanation

$\displaystyle \Delta G^0 = - nF{ E }_{ cell }^{ o } = \displaystyle {-RTln K_{eq}}$

$\displaystyle { E }_{ cell }^{ o } \ is\ -ve$

$\Delta G=+ve$

Hence,

$\displaystyle \Delta { G }^{ o } > 0; { K }_{ eq } < 1$

The number of moles of electrons required to discharge one mole of

$Al^{3+}$ is:

0%
$3$
0%
$1$
0%
$2$
0%
$4$

Explanation

Here, Charge on one mole of ${ Al }^{ 3+ }$ is 3 moles. The discharge reaction is as follows:

${ Al }^{ 3+ }+3{ e }^{ - }\longrightarrow Al$

According to the reaction for every mole aluminium ion, 3 electrons are required to discharge it. Hence for one mole of aluminium ion 3 moles of electrons are required.

Hence, the correct option is $\text{A}$

Electrochemical equivalent is the amount of substance which gets deposited from its solution on passing electrical charge equal to :

0%
$96,500$ coulomb
0%
$1$ coulomb
0%
$60$ coulomb
0%
$965$ coulomb

Explanation

Electrochemical equivalent is the amount of substance which gets deposited from its solution on passing electrical charge equal to

$96,500$ coulomb. Note:

$96500$ coulomb corresponds to the charge on one mole of electrons. It is called electrochemical equivalent.

The breaking down of a compound by passing electricity through it is known as

0%
electromagnetism
0%
electrolysis
0%
electronics
0%
ultrasound

Explanation

Electrolysis is the process of breaking down of a compound into its constituent ions by passing electricity through it.

For example : When an electric current is passed through water

$(H_2O)$ , it decomposes into

$O^{-2}$ and

$H^+$ ions which get further converted into Oxygen

$(O_2)$ and Hydrogen

$H_2$ , respectively.

Who invented the first true battery ?

0%
Faraday
0%
Ohm
0%
Volta
0%
Alva Edison

What is used as anode in Volta's cell?

0%
Zinc plate
0%
Copper plate
0%
Carbon rod
0%
Iron plate

In three test tubes

$P, Q$ , and

$R$ iron nails, water, oil and anhydrous calcium chloride is taken. Among these test tubes, in which test tubes corrosion of nails will not take place?

0%
$P, Q$ and $R$
0%
$P$ and $R$
0%
$P$ and $Q$
0%
$Q$ and $R$

Explanation

Conditions necessary for the rusting of iron:

$\bullet$ Presence of air (or oxygen)

$\bullet$ Presence of water (or moisture).

How many faradays are required to reduce 1 mol of

$Cr_2O_7^{2-}$ to

$Cr^{3+}$ in acidic medium?

0%
2
0%
3
0%
5
0%
6

Explanation

$1 \ mol\ Cr_2O_7^{2-}$ requires 6 moles electron

$= 6F$ charge

$\therefore$ Number of Faraday's required

$= 6$ .

Hence, option D is correct.

The equilibrium constant of the reaction;

$Cu\left( s \right) +2{ Ag }^{ + }\left( aq \right) \longrightarrow { Cu }^{ 2+ }\left( aq \right) +2Ag\left( s \right)$

${ E }^{ o }=0.46V$ at

$298 K$

0%
$2.4\times { 10 }^{ 10 }$
0%
$2.0\times { 10 }^{ 10 }$
0%
$4.0\times { 10 }^{ 10 }$
0%
$4.0\times { 10 }^{ 15 }$

Explanation

$Cu\left( s \right) +2{ Ag }^{ 2+ }\left( aq \right) \longrightarrow { Cu }^{ 2+ }\left( aq \right) +2Ag\left( s \right)$

${ E }^{ o }=0.46 V$ at

$298 K$

$\log { { K }_{ C }= } \dfrac { nF{ E }^{ o } }{ RT }$

$=\dfrac { 2\times 0.46 }{ 0.059 }$

${ K }_{ C }=4\times { 10 }^{ 15 }$

Conductivity of a solution is affected by:

0%
addition of water
0%
process of heating
0%
addition of acetic acid
0%
all of the above

Explanation

Conductivity of a solution is affected by

$(A)$ Addition of water

$(B)$ Process of heating and

$(C)$ Addition of acetic acid.
The above changes affect the solute concentration which in turn affects the number of current-carrying ions present per unit volume of solution. This affects the conductivity of the solution.

When metals corrodes, it is being :

0%
dissolved into surrounding moisture
0%
weakened structurally
0%
chemically combined with another metal
0%
reacted with oxygen

Number of faradays' required to generate one gram atom of magnesium from molten

$MgCl_{2}$ is_________.

0%
$1$
0%
$2$
0%
$3$
0%
$4$

Explanation

$Mg^{2+} + 2e^{-} \rightarrow Mg$

$1\ mole$ of

$Mg$ atom requires

$2\ mole$ of electrons, i.e.,

$2$ faraday of charge.

$K, Ca$ and

$Li$ metals may be arranged in the decreasing order of their standard electrode potentials as____________.

0%
$K, Ca$ and $Li$
0%
$Li, K$ and $Ca$
0%
$Li, Ca$ and $K$
0%
$Ca, Li$ and $K$

A solution of sodium sulphate in water is electrolysed using platinum electrodes. The products at cathode and anode are respectively:

0%
$H_{2}, O_{2}$
0%
$O_{2}, H_{2}$
0%
$O_{2}, Na$
0%
$O_{2}, SO_{2}$

Explanation

At cathode (negative electrode) reduction occurs,

$2H^++2e^-\longrightarrow H_2\uparrow$

At anode (positive electrode) oxidation occurs.

$2O^{2-}\longrightarrow O_2+4e^-$

(Refer to Image)

Three faradays of electricity was passed through an aqueous solution of iron(II) bromide. The mass of iron metal (At. mass

$56$ ) deposited at the cathode is:

0%
$56\ g$
0%
$84\ g$
0%
$112\ g$
0%
$168\ g$

Explanation

${ Fe }^{ 2+ }+2{ e }^{ - }\rightarrow Fe$

n=2 as 2 electrons are exchanged in this reaction

3F charge is passed which implies 3 moles electrons are passed.

1 mole of Fe is formed when 2 moles of electrons are passed.

For 3 moles of electrons passed 1.5 moles of Fe will be formed.

mass of iron deposited

$=56\times 1.5=84g$

The half-cell reaction is the one that:

0%
takes place at one electrode
0%
consumes half a unit of electricity
0%
involves half a mole of electrolyte
0%
goes half way to completion

One Faraday is equal to:

0%
$9650\ coulomb$
0%
$10,000\ coulomb$
0%
$19640\ coulomb$
0%
$96500\ coulomb$

CBSE Questions for Class 12 Engineering Chemistry Electrochemistry Quiz 1 - MCQExams.com

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Practice Class 12 Engineering Chemistry Quiz Questions and Answers

CBSE Questions for Class 12 Engineering Chemistry Electrochemistry Quiz 1 - MCQExams.com

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Practice Class 12 Engineering Chemistry Quiz Questions and Answers

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