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Test: Nernst Equation - NEET MCQ


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Test: Nernst Equation - Question 1

 Cell reaction is spontaneous when

Detailed Solution for Test: Nernst Equation - Question 1

An electrochemical reaction takes place when the cations and the anions present in the electrolyte solution travel to the respective electrodes and either give up or take up electrons. As the ions travel, they carry a certain charge and in this process, electricity is produced.
But all these processes will only be possible or be spontaneous when the Gibbs Free energy of the medium is negative.

Test: Nernst Equation - Question 2

Three cell A, B and C has equilibrium constant in the ratio 1:4 : 9 respectively. Arrange the following cells in the order of increasing Gibbs free energy.

Detailed Solution for Test: Nernst Equation - Question 2

The correct answer is option A

 

The cells will be arranged as such 9 : 4: 1.

Explanation:

  • The equilibrium constant that is used here is represented with k.

  • The smaller the value of k the higher will be the value of energy according to Gibbs.

  • So, 1 has the highest Gibbs free energy while 9 has the least.

  • This is the energy of a chemical reaction.

  • It is represented by G.

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Test: Nernst Equation - Question 3

 Gibbs free energy change for a cell reaction is positive what does it indicates?

Detailed Solution for Test: Nernst Equation - Question 3

The correct answer is Option C.

Reactions with a negative ∆G release energy, which means that they can proceed without an energy input (are spontaneous). In contrast, reactions with a positive ∆G need an input of energy in order to take place (are non-spontaneous). Reactions with a positive ∆H and negative ∆S are non-spontaneous at all temperatures.

Test: Nernst Equation - Question 4

 At equilibrium:

Detailed Solution for Test: Nernst Equation - Question 4

The correct answer is option A

E cell is 0 in equilibrium, that is Ecathode becomes equal to E anode ……….
EZero cell becomes zero when both the electrodes are of the same metal but of different concentration i.e for concentration cell……
We know that EZero cell is - Ezerocathode -E zeroanode (since cathode and anode are same ) so EZero =0
 

Test: Nernst Equation - Question 5

In the equation, ΔG° = – nF E° cell ; F is:

Detailed Solution for Test: Nernst Equation - Question 5

The correct answer is Option B.
The relationship between ΔGo and Eo is given by the following equation: ΔGo=−nFEo. Here, n is the number of moles of electrons and F is the Faraday constant.

Test: Nernst Equation - Question 6

 Consider the cell reaction:
Cd(s) | Cd2+ (1.0 M) || Cu2+ (1.0 m) | Cu (s)
If we wish to make a cell with more positive voltage using the same substances, we should:

Detailed Solution for Test: Nernst Equation - Question 6

The correct answer is Option D.

Redox reaction:
Cd(s)→Cd2++2e
Cu2++2e→Cu(s)
Ecell = E°cell − (0.059/2) log ([Cd2+]/ [Cu2+])
Decreases [Cd2+] to 0.1M and increases [Cu2+] to 1.0M

Test: Nernst Equation - Question 7

. The electrode potential at any concentration measured with respect to standard hydrogen electrode can be represented by:

Detailed Solution for Test: Nernst Equation - Question 7

The correct answer is Option B
Nernst equation is,

where, Q is the reaction quotient of the reaction
As, [M (s) ]=1
We get,

Test: Nernst Equation - Question 8

. For an equation: Ni(s) + 2Ag+(aq) → Ni2+ (aq) + 2Ag(s) the Nernst equation is written as:

Detailed Solution for Test: Nernst Equation - Question 8

The correct answer is Option A.
Oxidation: 
Ni(s) ---> Ni2+(aq) + 2e-
Reduction:
2Ni+(aq) + 2e- ----> 2Aq(s)
2e- are in the above reaction so;
         n = 2
We know that 
Ecell = Eocell – (RT/nF) lnKc
         = Eocell – (RT/nF) ln ([Ni]2+ / [Ag+]2

Test: Nernst Equation - Question 9

Nernst equation for an electrode is based on the variation of electrode potential of an electrode with:

Detailed Solution for Test: Nernst Equation - Question 9

Nernst equation for an electrode is based on the variation of electrode potential of an electrode with temperature and concentration of electrolyte.

Test: Nernst Equation - Question 10

The free energy change for the following cell reaction is given as :
2Au3+ (aq) + 3Cu (s) → 2Au (s) + 3Cu2+ (aq)

Detailed Solution for Test: Nernst Equation - Question 10

The correct answer is Option D.

EO = EOCa2+/ Ca  -  EOAu2+/ Au
        = -2.87 - (1.50)
     = -2.87 - 1.50
     = -4.37 V
rGO = -nFEO
           = -6 FEO

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