Electrochemistry Test

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Electrochemistry Test - 34

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Question 1
1 / -0

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

A
Both Assertion and Reason are true and Reason is the correct explanation of Assertion

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

C
Assertion is true but Reason is false

D
Assertion is false but Reason is true

E
Both Assertion and Reason are false

Solution

In an electrolytic reaction, negatively charged anions move towards positively charged anode whereas positively charged cations move towards negatively charged cathode.
Question 2
1 / -0

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

A
$$\displaystyle { Cu }^{ 2+ }$$ to $$\displaystyle Cu$$

B
$$\displaystyle Cl{ O }_{ 3 }^{ - }$$ to $$\displaystyle Cl{ O }^{ - }$$

C
$$\displaystyle { Cl }^{ - }$$ to $$\displaystyle { Cl }_{ 2 }$$

D
$$\displaystyle { H }^{ + }$$ to $$\displaystyle { H }_{ 2 }$$

E
$$\displaystyle { O }_{ 2 }$$ to $$\displaystyle { H }_{ 2 }O$$

Solution

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.
Question 3
1 / -0

In electrochemical corrosion. the metal undergoing corrosion :

A
acts as anode

B
acts as cathode

C
undergoes reduction

D
liquifies

Solution

In electrochemical corrosion. the metal undergoing corrosion acts as an anode.

In anode region, the metal is oxidized to metal cation and in cathode region, oxygen is reduced to water.

Hence option A is correct.
Question 4
1 / -0

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 :

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

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

C
Cl$$_2$$ + 2e$$^-$$ $$\rightarrow$$ 2Cl$$^-$$

D
2Cl$$^-$$ $$\rightarrow$$ Cl$$_2$$ + 2e$$^-$$

E
Zn + Cl$$_2$$ $$\rightarrow$$ ZnCl$$_2$$

Solution

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.
Question 5
1 / -0

Assertion: Input of energy is required by electrolytic cells.
Reason: Electrolytic cells have just one container, while voltaic cells have two.

A
Both Assertion and Reason are true and Reason is the correct explanation of Assertion

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

C
Assertion is true but Reason is false

D
Assertion is false but Reason is true

E
Both Assertion and Reason are false

Solution

Assertion: Input of energy is required by electrolytic cells.
By passage of electric current, a non spontaneous chemical reaction is carried out.
Reason: Electrolytic cells have just one container in which two electrodes dip in the solution to be electrolyzed, while voltaic cells have two, one is anode compartment and other is cathode compartment. These two containers are joined by salt bridge.
Question 6
1 / -0

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

A
$$Zn\rightarrow { Zn }^{ 2+ }+2e$$

B
$${ Zn }^{ 2+ }+2e\rightarrow Zn$$

C
$${ Cl }_{ 2 }+2e\rightarrow 2{ Cl }^{ - }$$

D
$$2{ Cl }^{ - }\rightarrow { Cl }_{ 2 }+2e$$

E
$$Zn+{ Cl }_{ 2 }\rightarrow Zn{ Cl }_{ 2 }$$

Solution

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.
Question 7
1 / -0

What is a cathode?

A
Electrode where reduction takes place and electrons are gained.

B
Electrode where oxidation takes place and electrons are lost.

C
Electrode where reduction takes place and electrons are lost.

D
A fluid that conducts electricity.

E
Electrode where oxidation takes place and electrons are gained.

Solution

Cathode is an electrode where reduction takes place and electrons are gained.
Anode electrode where oxidation takes place and electrons are lost.
Question 8
1 / -0

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

A
$$E^{0}_{cell}$$ = $$E^{0}_{cathode}$$ - $$E^{0}_{anode}$$

B
$$E^{0}_{cell}$$ = $$E^{0}_{cathode}$$ + $$E^{0}_{anode}$$

C
$$E^{0}_{constant}$$ = $$E^{0}_{cathode}$$ - $$E^{0}_{anode}$$

D
$$E^{0}_{constant}$$ = $$E^{0}_{cathode}$$ + $$E^{0}_{anode}$$

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

Solution

The correct formula for determining the voltage of an electrochemical cell is
Eo cell = Eo cathode - Eo anode
Here, the electrode potentials corresponds to the standard reduction potentials.
Cathode is the right hand electrode and anode is left hand electrode.
Question 9
1 / -0

What two metals are often used in electrochemical cells?

A
Zinc and copper

B
Zinc and sulfur

C
Carbon and copper

D
Zinc and carbon

E
Sulfur and copper

Solution

Zinc and copper are often used in electrochemical cells.
An electrochemical cell is a device used to study chemical reactions electrically.
Question 10
1 / -0

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

A
The electrons will migrate through the wire

B
The cations in the salt bridge will migrate to the anode half-cell

C
The cathode will gain mass

D
The anode will lose mass

E
Reduction will occur at the cathode

Solution

The anions in the salt bridge will migrate to the anode half-cell not cations so option $$B$$ is not true.

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Electrochemistry Test - 34

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Question 1

Both Assertion and Reason are true and Reason is the correct explanation of Assertion

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

Assertion is true but Reason is false

Assertion is false but Reason is true

Both Assertion and Reason are false

Solution

Question 2

$$\displaystyle { Cu }^{ 2+ }$$ to $$\displaystyle Cu$$

$$\displaystyle Cl{ O }_{ 3 }^{ - }$$ to $$\displaystyle Cl{ O }^{ - }$$

$$\displaystyle { Cl }^{ - }$$ to $$\displaystyle { Cl }_{ 2 }$$

$$\displaystyle { H }^{ + }$$ to $$\displaystyle { H }_{ 2 }$$

$$\displaystyle { O }_{ 2 }$$ to $$\displaystyle { H }_{ 2 }O$$

Solution

Question 3

acts as anode

acts as cathode

undergoes reduction

liquifies

Solution

Question 4

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

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

Cl$$_2$$ + 2e$$^-$$ $$\rightarrow$$ 2Cl$$^-$$

2Cl$$^-$$ $$\rightarrow$$ Cl$$_2$$ + 2e$$^-$$

Zn + Cl$$_2$$ $$\rightarrow$$ ZnCl$$_2$$

Solution

Question 5

Both Assertion and Reason are true and Reason is the correct explanation of Assertion

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

Assertion is true but Reason is false

Assertion is false but Reason is true

Both Assertion and Reason are false

Solution

Question 6

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

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

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

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

$$Zn+{ Cl }_{ 2 }\rightarrow Zn{ Cl }_{ 2 }$$

Solution

Question 7

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.

Solution

Question 8

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

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

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

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

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

Solution

Question 9

Zinc and copper

Zinc and sulfur

Carbon and copper

Zinc and carbon

Sulfur and copper

Solution

Question 10

The electrons will migrate through the wire

The cations in the salt bridge will migrate to the anode half-cell

The cathode will gain mass

The anode will lose mass

Reduction will occur at the cathode

Solution

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