Free Solved If the cell is initially at standard conditions, which of the following statement is true.


Screenshot 2024 01 07 221218

Screenshot 2024 01 07 221218

Step 1 of 2

Given is the if the cell is initially at standard state conditions, which of the following statement is true.

 

Zn2+ (aq) + 2e ↽−−⇀Zn (s); Eo=-0.76V

Cu2+(aq) + 2e↽−−⇀Cu (s); Eo=+0.34V

We found out the given A to E statements which statement is correct for the given case.

Explanation:

Here we use the concept of electrode potential and Gibbs free energy.

 

 

Step 2 of 2

As in this is given

 

Zn2+ (aq) + 2e ↽−−⇀Zn (s); Eo=-0.76V

Cu2+(aq) + 2e↽−−⇀Cu (s); Eo=+0.34V

Explanation:

Since electrons are produced at the Zn electrode (Left side), this electrode is rich in electrons and designated as the negative pole (Anode) at which oxidation takes place and Cu electrode (Right side) is in need of electrons for reduction of Cu2+ ions into Cu i.e., this electrode is deficient in electrons and act as positive pole (Cathode).

Eocell=Eo(cathode)-Eo(anode)

 

Eocell=EoRight-EoLeft

 

Eocell=+0.34 -(-0.76)=1.1V

 

DelG = -212.300 KJ

 

Explanation:

Option D is correct as initially ΔG is +212kJ and at equilibrium it becomes 0 and after with time it becomes more negative.

Final solution

Hence option D follows all given requirements as this statement becomes correct.

 

 

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