Electrochemistry Test

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Electrochemistry Test - 20

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Weekly Quiz Competition

Question 1
4 / -1

The standard reduction potential E^o for half reactions are
Zn = Zn⁺ + Ze, E^o = + 0.76 V
Fe = Fe²⁺ + Ze, E^o = + 0.41 V
The emf of the cell reaction
Fe²⁺ + Zn = Zn²⁺ + Fe is

A
- 0.35 V

B
+0.35 V

C
+1.17 V

D
- 1.17 V
Question 2
4 / -1

Which of the following reactions is correct for a given electrochemical cell at 25°C?
Pt | Br₂(g) | Br^- (g) || Cl^- (aq) | Cl₂(g) | Pt

A
2Br^- (aq) + Cl₂ (g) → 2Cl^- (aq) + Br₂ (g)

B
Br₂ (g) + 2Cl^- (aq) → 2 Br^- (aq) + Cl₂ (g)

C
Br₂ (g) + Cl₂(g) → 2Br^- (aq) + 2Cl^- (aq)

D
2Br^- (aq) + 2Cl^- (aq) → Br₂ (g) + Cl₂ (g)
Question 3
4 / -1

What will be the electrode potential of that hydrogen electrode is filled with HCl solution of pH value 1.0?

A
- 59.15 V

B
+ 59.15 V

C
+ 59.15 mV

D
- 59.15 mV
Question 4
4 / -1

A
II

B
I

C
III

D
All of these
Question 5
4 / -1

At 25^oC temperature the cell potential of a given electrochemical cell is 1.92 V. Find the value of x.
Mg (s) | Mg²⁺ (aq) x M ||Fe²⁺ (aq) 0.01M| Fe (s)
E^o Mg / Mg²⁺ (aq) = 2.37 V; E^o Fe/ F_e²⁺ (aq) = 0.45 V

A
x = 0.01 M

B
x < 0.01 M

C
x > 0.01 M

D
x cannot be predicted
Question 6
4 / -1

The emf of the cell Ni|Ni²⁺ (1.0M)|| Au³⁺ (1.0M)| Au is [E^o(Ni²⁺/Ni) = -0.25 V and E^o (Au³⁺/Au) = + 1.5V]

A
2.00 V

B
1.25 V

C
- 1.25 V

D
1.75 V
Question 7
4 / -1

A
-0.072 V

B
0.385 V

C
0.770 V

D
-0.270 V

Solution
Question 8
4 / -1

Daniel cell, anode and cathode are, respectively

A
Zn|Zn²⁺ and Cu²⁺| Cu

B
Cu|Cu²⁺ and Zn²⁺| Zn

C
Fe|Fe²⁺ and Cu²⁺|Cu

D
Cu|Cu²⁺ and Fe²⁺|Fe
Question 9
4 / -1

The potential of the following cell is 0.34V at 25°C. Calculate the standard reduction potential of the copper half-cell.
Pt | H₂ (1 atm) | H⁺ (1 M) || Cu²⁺ (1 M) | Cu

A
-3.4 V

B
+3.4 V

C
-0.34 V

D
+ 0.34 V

Solution
Question 10
4 / -1

The potential of the cell for the reaction,
M (s) + 2 H⁺ (1M) → H₂ (g) (1 atm) + M²⁺ (0.1M) is 1.500 V. The standard reduction potential for M²⁺/ M (s) couple is

A
0.1470 V

B
1.470 V

C
14.70 V

D
None of these

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Electrochemistry Test - 20

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Electrochemistry Test - 20

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Question 1

- 0.35 V

+0.35 V

+1.17 V

- 1.17 V

Question 2

2Br- (aq) + Cl2 (g) → 2Cl- (aq) + Br2 (g)

Br2 (g) + 2Cl- (aq) → 2 Br- (aq) + Cl2 (g)

Br2 (g) + Cl2(g) → 2Br- (aq) + 2Cl- (aq)

2Br- (aq) + 2Cl- (aq) → Br2 (g) + Cl2 (g)

Question 3

- 59.15 V

+ 59.15 V

+ 59.15 mV

- 59.15 mV

Question 4

II

I

III

All of these

Question 5

x = 0.01 M

x < 0.01 M

x > 0.01 M

x cannot be predicted

Question 6

2.00 V

1.25 V

- 1.25 V

1.75 V

Question 7

-0.072 V

0.385 V

0.770 V

-0.270 V

Solution

Question 8

Zn|Zn2+ and Cu2+| Cu

Cu|Cu2+ and Zn2+| Zn

Fe|Fe2+ and Cu2+|Cu

Cu|Cu2+ and Fe2+|Fe

Question 9

-3.4 V

+3.4 V

-0.34 V

+ 0.34 V

Solution

Question 10

0.1470 V

1.470 V

14.70 V

None of these

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2Br^- (aq) + Cl₂ (g) → 2Cl^- (aq) + Br₂ (g)

Br₂ (g) + 2Cl^- (aq) → 2 Br^- (aq) + Cl₂ (g)

Br₂ (g) + Cl₂(g) → 2Br^- (aq) + 2Cl^- (aq)

2Br^- (aq) + 2Cl^- (aq) → Br₂ (g) + Cl₂ (g)

Zn|Zn²⁺ and Cu²⁺| Cu

Cu|Cu²⁺ and Zn²⁺| Zn

Fe|Fe²⁺ and Cu²⁺|Cu

Cu|Cu²⁺ and Fe²⁺|Fe