Electrochemistry Test

Result

Electrochemistry Test - 18

Score
-
out of -
Rank
-
out of -

TIME Taken - -

SHARING IS CARING

If our Website helped you a little, then kindly spread our voice using Social Networks. Spread our word to your readers, friends, teachers, students & all those close ones who deserve to know what you know now.

Weekly Quiz Competition

Question 1
4 / -1

Given below are the half- cell reactions
Mn²⁺ + 2e^‒ → Mn; E^o = ‒ 1.18e V
2(Mn³⁺ + e^‒ → Mn²⁺) E^o = + 1.51e V
The E^o for 3 Mn²⁺ → Mn + 2Mn³⁺ will be

A
‒2.69V, the reaction will not occur

B
‒2.69 V, the reaction will occur

C
‒0.33 V, the reaction will not occur

D
‒0.33 V, the reaction will occur

Solution
Question 2
4 / -1

What is the cell potential (standard emf, E°) for the reaction below ?
[E°_{(Fe²/(aq)Fe)} = 0.44 V and E°_{(O₂(g)/H₂O/OH ^‒ )} = + 0.4V]
2Fe (s) + O₂ (g) + 2H₂O (l) ⇌ 2Fe²⁺ (aq) + 4OH ^‒ (aq)

A

B

C

D

Solution
Question 3
4 / -1

A
2

B
3

C
5

D
4

Solution
Question 4
4 / -1

Zinc is used to reduce iron because

A
E_red of Zn < E_red of Fe

B
E_oxi of Zn < E_oxide of Fe

C
E_oxi of Zn = E_oxide of Fe

D
Zinc is cheaper than iron
Question 5
4 / -1

A
Ag₂O

B
Al₂O₃

C
MgO

D
Na₂O
Question 6
4 / -1

A
Cl

B
Cr³⁺

C
Mn²⁺

D

Solution
Question 7
4 / -1

A
Weston cell

B
Daniell cell

C
Calomel cell

D
Faraday cell
Question 8
4 / -1

Aluminium displaces hydrogen from acids but copper does not. A galvanic cell prepared by combining Cu / Cu²⁺ and Al/ Al³⁺ has an emf of 2.0 V at 298 K. If the potential of copper electrode is +0.34 V, that of aluminimum electrode is

A
- 2.3 V

B
+ 2. 34 V

C
-1.66 V

D
+ 1.66 V

Solution
Question 9
4 / -1

The standard emf. of a cell Zn/Zn²⁺|| Fe²⁺/Fe, if electrode potentials for (Zn/Zn²⁺) and (Fe²⁺/Fe) are 0.763 V and - 0.44 V respectively is

A
+ 0.323 V

B
- 1.203 V

C
+ 1.203 V

D
- 0.323 V
Question 10
4 / -1

The electrochemical cell shown below is a concentration cell. M / M²⁺ (saturated solution of a sparingly soluble salt, MX₂) 11M²⁺ (0.00001 mol dm^-3/ M) . The emf of the cell depends on the difference in concentration of M²⁺ ions at the two electrodes. The emf of the cell at 298 is 0.059 V. The value of ∆G (kJ mol^-1 ) for the given cell is (take 1F = 96500C mol^-1 )

A
- 5.7

B
5.7

C
11.4

D
- 11.4