Electrochemistry is an important topic in the Chemistry section in MHT CET exam. Practising this topic will increase your score overall and make your conceptual grip on MHT CET exam stronger.
This article gives you a full set of MHT CET PYQs for Electrochemistry with explanations for effective preparation. Practice of MHT CET Chemistry PYQs including Electrochemistry questions regularly will improve accuracy, speed, and confidence in the MHT CET 2026 exam.
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MHT CET PYQs for Electrochemistry with Solutions
1.
What is standard reduction potential of Cu2+ | Cu(s) if E° of following cell is 0.46V ? Cu(s) | Cu2+(aqs) || Ag+(aq) | Ag(s) ( Eo = 0.80V)
- 1.56 V
- 1.44 V
- 1.26 V
- 0.34 V
2.
What is the percentage composition of nitrogen in ammonium nitrate (\( \text{NH}_4\text{NO}_3 \))?- 18.5%
- 28.0%
- 35.0%
- 42.5%
3.
Alkyl halide and aryl halide react in the presence of sodium metal and dry ether. The name of the reaction is?- Wurtz Reaction
- Wurtz-Fittig Reaction
- Fittig Reaction
- Williamson Ether Synthesis
4.
$ 1\, C $ electricity deposits- $ 10.8\, g $ of $ Ag $
- $ 96500\, g $ of $ Ag $
- electrochemical equivalent of $ Ag $
- half of electrochemical equivalent of $ Ag $
5.
In an electrochemical cell, the standard electrode potential of \( \text{Zn}^{2+}/\text{Zn} \) is \( -0.76 \, \text{V} \) and that of \( \text{Cu}^{2+}/\text{Cu} \) is \( +0.34 \, \text{V} \). What is the standard EMF of the cell formed by these electrodes?- \( 0.42 \, \text{V} \)
- \( 1.10 \, \text{V} \)
- \( -1.10 \, \text{V} \)
- \( -0.42 \, \text{V} \)
6.
Copper is a divalent metal. The value of its electrochemical equivalent is $ 3.29 \times 10^{-4}\, g $ . Its atomic mass is- $ 31.74\,g $
- $ 63.5 \,g $
- $ 126.9\, g $
- $ 15.87 \,g $
7.
What is the standard electrode potential of the half-reaction: \[ \text{Cu}^{2+} + 2e^- \rightarrow \text{Cu} \, (\text{solid})? \] Given that the standard electrode potential for the half-reaction: \[ \text{Ag}^+ + e^- \rightarrow \text{Ag} \, (\text{solid}) \quad \text{is} \, +0.80 \, \text{V}. \] Also, the cell potential for the following reaction is: \[ \text{Cu}^{2+} + 2\text{Ag} \rightarrow \text{Cu} + 2\text{Ag}^+ \] is \( 0.46 \, \text{V} \).\( 1.26 \, \text{V} \)
- \( 0.50 \, \text{V} \)
- \( 0.46 \, \text{V} \)
- \( 1.0 \, \text{V} \)
8.
During galvanization of iron, which metal is used for coating iron surface ?- Copper
- Zinc
- Nickel
- Tin
9.
The metal that cannot be obtained by electrolysis of an aqueous solution of its salts is:- \( \text{Ag} \)
- \( \text{Ca} \)
- \( \text{Cu} \)
- \( \text{Cr} \)
10.
What is the $SI$ unit of conductivity ?- $Sm$
- $Sm^{-1}$
- $Sm^{2}$
- $Sm^{-2}$
11.
What is the standard electrode potential for the reduction half-reaction \( \text{Cu}^{2+} + 2e^- \rightarrow \text{Cu} \)?- +0.34 V
- -0.34 V
- +0.72 V
- -0.72 V
12.
What is the standard electrode potential for the half-reaction \( \text{Cu}^{2+} + 2e^- \rightarrow \text{Cu} \)?- +0.34 V
- -0.34 V
- +1.10 V
- 0 V
13.
Which from following equations is correct for relation between standard cell potential and equilibrium constant?
Ecell =\(\frac {0.0592}{n}\) log10 K
Ecell = log10 K\(\frac {n}{(0.0592)}\)
E0cell = \(\frac {0.0592}{n}\) log10 K
Ecell = log10 K\(\frac {n}{0.0592}\)
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