1st Year Chemistry Electrochemistry MCQs

You can get 1st Year Chemistry Electrochemistry MCQs here if you are searching for the MCQs of Entry Test. This chapter is very important for Entry Test. When we talk about Electrochemistry, we first study oxidation and reduction. Then the most important term which comes is Ionization. There are many electrolytic cells e.g. Down’s cell etc. Electrolysis is a specific phenomenon used in the cells. The electrodes have their own Electrode Potential. There is a complete Electrochemical series for elements. They have numerous applications. When we say about batteries, there are two types of batteries. One is Rechargeable and the other is Non-Rechargeable. Both have their own importance and products. So, this is the brief introduction of this chapter. Check the important MCQs below.

1st Year Chemistry Electrochemistry MCQs

KEY POINTS

 

Question#1. Magnesium metal is extracted by the electrolysis of its:

A concentrated aqueous solution of its chloride
Dilute aqueous solution on of its chloride
Its fused chloride
Any solution

Question#2. Iron can be prevented from rusting by:

Connecting iron to more electropositive metal, a case of cathodic protection
Connecting iron to more electropositive metal, a case of anodic protection
Connecting iron to less electropositive metal, a case of anodic protection
Connecting iron to less electropositive metal, a case of cathodic protection

Question#3. Standard hydrogen electrode has an arbitrarily fixed potential of:

0 V
0.1 V
1.0 V
0.001 V

Question#4. The correct order of equivalent conductance at infinite dilution among LiCl, NaCl, and KCl is:

LiCl > NaCl > KCl
NaCl > KCl > LiCl
KCl > NaCl > LiCl
LiCl > KCl > NaCl

Question#5. Electrochemical series is useful in:

Prediction of the feasibility of a chemical reaction
Calculation of voltage
Comparison of the relative tendencies of the metals and non-metals to get oxidized or reduced
All of the above

Question#6. A normal aluminum electrode coupled with a normal hydrogen electrode gives an emf of 1.66 volts and deflection of the needle towards Hydrogen. The standard electrode potential of aluminum is:

-1.66 V
-0.83 V
+1.66 V
+0.83 V

Question#7. If the sum of E^o values of the two half cells is negative, then:

The reaction will be feasible
The reaction may or may not be feasible
The reaction will not be feasible
No prediction can be made

Question#8. Which of the following cell can convert chemical energy directly into electrical energy:

Mercury cell
Lead storage battery
Daniel cell
Fuel cell

Question#9. In a galvanic cell, the electrode occupying a lower position in the electrochemical series:

Will act as a cathode
The reduction will take place on it
Oxidation will take place on it
Both a and b

Question#10. Which of the following statement is true about galvanic cell:

The anode is positively charged
The cathode is positively charged
Reduction occurs at the anode
Reduction occurs at the cathode

Question#11. Greater the value of the standard reduction potential of the given species:

Greater is its tendency to accept electrons to undergo reduction
Greater is its tendency to accept electrons to undergo oxidation
Greater is its tendency to lose electrons to undergo reduction
Greater is its tendency to lose electrons to undergo oxidation

Question#12. Coinage metals have the least reactivity because they have:

Positive oxidation potentials
Zero oxidation potentials
Positive reduction potentials
Zero reduction potentials

Question#13. Which of the following is a secondary cell:

Dry cell
Ni-Cd cell
Mercury cell
Alkali cell

Question#14. Four metals A, B, C, and D are having standard electrode potential as -3.05, -1.66, -0.4, and 0.8V respectively. Which one will be the best reducing agent:

A
B
C
D

Question#15. The oxidation potential of Mg and Al are +2.37 and 1.66V, respectively. The Mg is a chemical reaction:

Will be replaced by Al
Won’t be able to replace Al
Will replace Al
None of the above

Question#16. Which can replace hydrogen from dilute acids?

Au
Zn
Pt
None of these

Question#17. The oxidation state of carbon-atom in glucose is:

+4
+6
-4
None of these

Question#18. The cell in which electrical energy is converted into chemical energy is:

Galvanic cell
Electrolytic cell
Voltaic cell
All of these

Question#19. The ability of elements to act as reducing agent _________ down to electrochemical series.

Increases
Remain constant
Decreases
Depends upon the reaction conditions

Question#20. If a strip of Cu-metals is placed in a solution of FeSO₄ then:

Cu will be deposited
Cu and Fe both dissolve
Fe is precipitated
No reaction occur

Question#21. “Al” metal is extracted from its ________ during electrolysis.

Chlorides
Cryolite
Oxides
All of these

Question#22. Halogens are placed at the lower level of electrochemical series, this indicates that:

Halogens are good reducing agents
Halogens are an oxidizing agent but bad reducing agents
Halogens are good oxidizing agent as well as good reducing agents
All the above statements are correct

Question#23. The electrolysis product of molten NaCl at electrodes:

Na and Cl₂
Na and NaOH
H₂ and Cl₂
H₂, Cl₂, and NaOH

Question#24. SHE acts as an anode when connected with Cu electrode but cathode with Zn electrode because:

Zn has less reduction potential than hydrogen and Cu more
Zn has less oxidizing potential than hydrogen and Cu more
Zn is above in electrochemical series than hydrogen and Cu below
All the above are possible reasons

Question#25. When an element is in contact with 1M aqueous solution of its own ions, at 298K then the potential is called?

Standard reduction potential
Reduction potential
Standard electrode potential
Both a and c

Question#26. Gold and silver are the least reactive due to:

Positive oxidation potential
Zero oxidation potential
Positive reduction potential
Having a large negative electrode potential

Question#27. During the electrolysis of aqueous KNO₃, H₂ is produced at cathode instead of potassium due to:

The reduction potential of K is greater than hydrogen
Hydrogen is more reactive than potassium
The reduction potential of potassium is less than hydrogen
All of the above are possible reasons

Question#28. Which of the following statement is correct?

Zn can replace Cu²⁺ in CuSO₄
Cu can replace H⁺ in H₂SO₄
Cu can replace Zn²⁺ in ZnSO₄
None of these

Question#29. In a reaction Zn + HNO₃ → Zn(NO₃)₂ + NO + H₂O:

Zn is reduced
N is oxidized
N is reduced
Hydrogen is reduced

Question#30. Which one metal shows the maximum oxidation state?

Mn
Ag
Cr
Hg