Electrochemistry Test

Result

Electrochemistry Test - 35

Score
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Weekly Quiz Competition

Question 1
4 / -1

A
(2 × 0.0771) ‒ 0.536) = 1.006 volt

B
(0.771 ‒ 0.5 × 0.536) = 0.503 volt

C
0.771 ‒ 0.536 = 0.235 volt

D
0.536 ‒ 0.771 = ‒ 0.235 volt

Solution
Question 2
4 / -1

A
+ 1.25 V

B
+1.75 V

C
‒1.25 V

D
‒1.75 V

Solution
Question 3
4 / -1

The EMF of the cell Ni|Ni²⁺ || Cu²⁺ |Cu is 0.59 volt. The standard electrode potential (reduction potential) of copper electrode is 0.34 volt. The standard electrode potential of nickel electrode will be

A
0.25 Volt

B
‒ 0.25 Volt

C
0.93 Volt

D
‒ 0.93 Volt

Solution
Question 4
4 / -1

A
1.56 V

B
0.64 V

C
‒ 1.56 V

D
2.02 V

Solution
Question 5
4 / -1

The standard EMF for the cell reaction. Zn + Cu²⁺ → Cu + Zn²⁺ is 1.1 volt at 25^oC. The EMF for the cell reaction, when 0.1 M Cu²⁺ and 0.1 M Zn²⁺ solutions are used , at 25^oC is.

A
1.10 V

B
0.10 V

C
‒ 1.10V

D
‒ 0.110 V

Solution
Question 6
4 / -1

The potential of the cell containing two hydrogen electrodes as represented below

A
‒ 0.118 V

B
‒ 0.0591V

C
0.118 V

D
0.0591 V

Solution
Question 7
4 / -1

A
E = ‒ 0.36 + (0.059/2) log (0.004/2)

B
E = + 0.36 + (0.059/2) log (0.004/2)

C
E = ‒ 0.36 + (0.059/2) log (0.2/0.004)

D
E = + 0.36 + (0.059/2) log (0.2/0.004)

Solution
Question 8
4 / -1

What is the potential of half –cell consisting of zinc electrode in 0.01 m ZnSO₄ solution at 25^oC (E⁰_0x = 0.763 V)

A
0.8221 V

B
8.221 V

C
0.5282 V

D
9.282 V

Solution
Question 9
4 / -1

The e.m.f of the following Daniell cell at 298 K is E₁ Zn|ZnSO₄ (0.01M)||CuSO₄ (1.0M)|Cu. When the concentration of ZnSO₄ is 1.0 M and that of CuSO₄ is 0.01 M, the e.m.f changed to E₂. What is the relationship between E₁ and E₂ ?

A
E₁ > E₂

B
E₁ < E₂

C
E₁ = E₂

D
E₂ = 0 ≠ E₁

Solution
Question 10
4 / -1

A
1.80 volt

B
1.07 volt

C
0.82 volt

D
2.14 volt

Solution