Electrochemistry Test

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Electrochemistry Test - 3

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Weekly Quiz Competition

Question 1
1 / -0

Standard electrode potential is measured taking the concentrations of all the species involved in a half-cell is

A
4 M

B
1 M

C
2M

D
3M

Solution

Under standard condition that is at 298K, the molar concentration of every species taken in each half cell is 1 M and if gases are involved the partial pressure of the gas is taken as 1 atm..
Question 2
1 / -0

The Nernst equation at 25°C involving the reaction Fe³+ + e^– →Fe²⁺ is

A
E = E° + (RT/nF) In ([Fe²⁺]/[Fe³⁺])

B
E = E^o – (RT/nF) log ([Fe²⁺]/[Fe³⁺])

C
E = E^o – (0.0595 V) In ([Fe²⁺]/[Fe³⁺])

D
E = E^o – (0.0595 V) log ([Fe²⁺]/[Fe³⁺])
Question 3
1 / -0

Given: E°(Ag⁺|Ag) = 0.799 V and E^o(Zn²⁺|Zn) = – 0.763 V. Which of the following facts is correct?

A
Ag⁺ can be reduced by H₂(g).

B
Ag can oxidise H₂(g) to H⁺.

C
Zn²⁺ can be reduced by H₂(g).

D
Ag can reduce Zn²⁺.
Question 4
1 / -0

Molar conductivity has the unit of

A
Ω^-1

B
Ω^-1 cm^-1

C
Ω^-1 cm² eq^-1

D
Ω^-1 cm² mol^-1
Question 5
1 / -0

A sample of 1.08 g of pure silver was converted into silver nitrate and its solution was taken in a beaker. It was electrolysed using platinum cathode and silver anode. 0.01 faraday of electric current was passed using 0.15 volt above the decomposition potential of silver. The silver content of the beaker after the above process must be

A
zero

B
0.108 g

C
10.8 g

D
1.08 g
Question 6
1 / -0

Conductivity always decreases with decrease in concentration both, for weak and strong electrolytes because of the fact that

A
mobility of ions that carry the current in a solution increases on dilution

B
the number of ions per unit volume that carry the current in a solution decreases on dilution

C
the number of collisions of ions per unit volume that carry the current in a solution increases on dilution

D
the number of ions per unit volume that carry the current in a solution increases on dilution

Solution

Conductivity is conductance of one centimetercube of the solution. so on dilution the number of ions per cm3 decreases.
Question 7
1 / -0

During the measurement of EMF of a half cell using a reference electrode and a salt bridge, if the salt bridge is removed, then the voltage

A
remains unchanged

B
decreases to half the previous value

C
increases to its maximum value

D
drops to zero or becomes negative
Question 8
1 / -0

Molar conductivity denoted by the symbol Λm is related to the conductivity of the solution by the equation (κ is the conductivity and c the concentration)

A
Λm=2/kc

B
Λm=k/c

C
Λm=c/k

D
Λm=k/c

Solution

Molar conductivity is conducting power of all the ions produced by dissolving 1 mole of electrolyte in solution.
Question 9
1 / -0

The following question consists of Assertion (A) and Reason (R). Mark the appropriate answer.

(A): Equivalent conductance of all electrolytes decreases with increasing concentration.
(R): Lesser ions are available per gram equivalent at higher concentration.

A
Both (A) and (R) are correct and (R) is the right explanation of (A).

B
Both (A) and (R) are correct, but (R) is not the right explanation of (A).

C
(A) is correct, but (R) is incorrect.

D
(A) is incorrect, but (R) is correct.

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Electrochemistry Test - 3

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Question 1

4 M

1 M

2M

3M

Solution

Question 2

E = E° + (RT/nF) In ([Fe2+]/[Fe3+])

E = Eo – (RT/nF) log ([Fe2+]/[Fe3+])

E = Eo – (0.0595 V) In ([Fe2+]/[Fe3+])

E = Eo – (0.0595 V) log ([Fe2+]/[Fe3+])

Question 3

Ag+ can be reduced by H2 (g).

Ag can oxidise H2(g) to H+.

Zn2+ can be reduced by H2 (g).

Ag can reduce Zn2+.

Question 4

Ω-1

Ω-1 cm-1

Ω-1 cm2 eq-1

Ω-1 cm2 mol-1

Question 5

zero

0.108 g

10.8 g

1.08 g

Question 6

mobility of ions that carry the current in a solution increases on dilution

the number of ions per unit volume that carry the current in a solution decreases on dilution

the number of collisions of ions per unit volume that carry the current in a solution increases on dilution

the number of ions per unit volume that carry the current in a solution increases on dilution

Solution

Question 7

remains unchanged

decreases to half the previous value

increases to its maximum value

drops to zero or becomes negative

Question 8

Λm=2/kc

Λm=k/c

Λm=c/k

Λm=k/c

Solution

Question 9

Both (A) and (R) are correct and (R) is the right explanation of (A).

Both (A) and (R) are correct, but (R) is not the right explanation of (A).

(A) is correct, but (R) is incorrect.

(A) is incorrect, but (R) is correct.

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E = E° + (RT/nF) In ([Fe²⁺]/[Fe³⁺])

E = E^o – (RT/nF) log ([Fe²⁺]/[Fe³⁺])

E = E^o – (0.0595 V) In ([Fe²⁺]/[Fe³⁺])

E = E^o – (0.0595 V) log ([Fe²⁺]/[Fe³⁺])

Ag⁺ can be reduced by H₂(g).

Ag can oxidise H₂(g) to H⁺.

Zn²⁺ can be reduced by H₂(g).

Ag can reduce Zn²⁺.

Ω^-1

Ω^-1 cm^-1

Ω^-1 cm² eq^-1

Ω^-1 cm² mol^-1