Test: Nernst Equation - NEET MCQ

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.

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.

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.

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
 

The correct answer is Option B.
The relationship between ΔG^o and E^o is given by the following equation: ΔG^o=−nFE^o. Here, n is the number of moles of electrons and F is the Faraday constant.

The correct answer is Option D.

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

The correct answer is Option B
Nernst equation is,

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

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 
E_cell = E^o_cell – (RT/nF) lnK_c
         = E^o_cell – (RT/nF) ln ([Ni]²⁺ / [Ag⁺]²

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

The correct answer is Option D.

E^O = E^O_Ca²⁺/ _Ca  -  E^O_Au²⁺/ _Au
        = -2.87 - (1.50)
     = -2.87 - 1.50
     = -4.37 V
rG^O = -nFE^O
           = -6 FE^O