which of the following reactions would require the use of an inert electrode? po

Question

which of the following reactions would require the use of an inert electrode? point Which of the following cell reactions would require the Which of the following cell reactions would require the use of an inert use 7. (1/2 point) of an inert electrode? 1 . Zn(s) + 2Fe3+(aq) Zn2+(aq) + 2Fe2+ (aq) 2. Zn(s) + 2Ag+(aq) Zn2+(aq) + 2Ag(s) 3. 3Cu(s) + 2Au3+(aq) 3Cu2+ (aq) + 2Al(s) 4. Ch(g) + 21(aq) 2Cl(aq) + I2(s) aqaq)+/Cu2+(a ) +2Au(s) a. 1 only b. 1 and 3 only c. 2 and 3 only d. 1 and 4 only e. 3 and 4 only 8. (1/2 point) Consider the following electrode potentials: 8. (1/2 point) Consider the following eleetrode potentials E"red = 0.15 V E"red=-1.18 V Ered =-2.37 V Cu2+ + e- Cu Mg2+ +2e- Mg Which one of the reactions below will proceed spontaneously from left to right? e. none of these

Explanation / Answer

7) A galvanic cell requires an inert electrode in case of half cell reactions where no solid reduced product is formed, so we need some inert electrode to carry out oxidation and reduction on that inert electrode.

So here in case of first three reactions :

(i) Zn and Fe electrode can be used

(ii) Zn and Ag electrode can be used

(iii) Cu and Au electrode can be used

(iv) however in this reaction we can not use Chlorine or iodin electrode as they are gas.

8) Remember : In a cell a metal with low reduction potential will act as anode on which oxidation will take place, whil the metal wiht high reduction potential will act as cathode on which reduction will take place

It this is not the case, the reaction will not be feasible

a) Mg+2 + V --> V+2 + Mg

E0cell = E0cathode -E0anode

E0cell = -2.37 - (-1.18) = -1.19 (negative emf means the reaction will not be possible, non spontaneous

b) Mg+2 + 2Cu+ --> 2Cu+ + Mg

E0cell = E0cathode -E0anode

E0cell = -2.37 - 0.15 = -2.52 (negative emf means the reaction will not be possible, non spontaneous

c) V+2 + 2Cu+ --> V + 2Cu+2

E0cell = E0cathode -E0anode

E0cell = -1.18 - 0.15 = -1.03 (negative emf means the reaction will not be possible, non spontaneous

d) V + 2Cu+2 --> V+2 + 2Cu+

E0cell = E0cathode -E0anode

E0cell = 0.15 - (-1.18) = 1.33

Postive emf means the reaction will be spontaneous

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