Advertisements
Advertisements
Question
E°cell for the given redox reaction is 2.71 V
Mg(s) + Cu2+ (0.01 M) → Mg2+ (0.001 M) + Cu(s)
Calculate Ecell for the reaction. Write the direction of flow of current when an external opposite potential applied is
(i) less than 2.71 V and
(ii) greater than 2.71 V
Solution
Ecell = `"E"°_"cell" - (0.0591)/(n)log ["Mg"^(2+)] // ["Cu"^(2+)]`
= `2.71 - (0.0591)/(2)log (0.001)/(0.01)`
=`2.71 - 0.0295 xx (-1)`
= `2.7395 "V"`
i) When an external potential is less than 2.71 then current will flow from copper to magnesium.
ii) When an external potential is greater than 2.71 then current will flow from magnesium to copper.
APPEARS IN
RELATED QUESTIONS
What happens if external potential applied becomes greater than E°cell of electrochemical cell?
Why cannot we store AgNO3 solution in copper vessel?
Cell equation: \[\ce{A + 2B^- -> A^{2+} + 2B}\]
\[\ce{A^{2+} + 2e^- -> A}\] E0 = +0.34 V and log10 k = 15.6 at 300 K for cell reactions find E0 for \[\ce{B^+ + e^- -> B}\]
Write a note on sacrificial protection.
Electrode potential for Mg electrode varies according to the equation
`E_(Mg^(2+) | Mg) = E_(Mg^(2+) | Mg)^Θ - 0.059/2 log 1/([Mg^(2+)])`. The graph of `E_(Mg^(2+) | Mg)` vs `log [Mg^(2+)]` is ______.
Which of the following statement is not correct about an inert electrode in a cell?
The electrochemical cell stops working after some time because
If the half-cell reaction A + e– → A– has a large negative reduction potential, it follow that:-
What should be the signs (positive/negative) for \[\ce{E^0_{cell}}\] and ΔG0 for a spontaneous redox reaction occurring under standard conditions?
What is an electrochemical cell? What does it consist of?
