Advertisements
Advertisements
Question
Can you store copper sulphate solutions in a zinc pot?
Solution
\[\ce{E^Θ_{{Zn^{2+}/{ Zn}}}}\] = −0.76 V; \[\ce{E^Θ_{{Cu^{2+}/{ Cu}}}}\] = 0.34 V
We have to check whether the following reaction takes place or not.
\[\ce{Zn_{(s)} + CuSO4_{(aq)} -> ZnSO4_{(aq)} + Cu_{(s)}}\]
The cell can be represented as:
\[\ce{Zn | Zn^{2+} || Cu^{2+} | Cu}\]
\[\ce{E^Θ_{cell} = E^Θ_{{Cu^{2+}/{ Cu}}} - E^Θ_{{Zn^{2+}/{ Zn}}}}\]
= 0.34 V – (– 0.76 V)
= 1.1 V
Since \[\ce{E^Θ_{cell}}\] is positive, the reaction takes place, and we cannot store \[\ce{CuSO4}\] solution in a zinc pot.
APPEARS IN
RELATED QUESTIONS
Arrange the following metals in the order in which they displace each other from the solution of their salts.
\[\ce{Al, Cu, Fe, Mg}\] and \[\ce{Zn}\]
How many electrons flow through a metllic wire if a current of 0·5 A is passed for 2 hours? (Given : 1 F = 96,500 C mol−1)
Define the following term:
Fuel cell
How many faradays of electricity are required to produce 6 g of Mg from MgCl2?
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
For the electrochemical cell:
M | M+ || X− | X,
E0(M+ | M) = 0.44 V, E0(X | X−) = 0.33 V
Which of the following is TRUE for this data?
A solution of CuSO4 is electrolysed using a current of 1.5 amperes for 10 minutes. What mass of Cu is deposited at cathode? [Atomic mass of Cu = 63.7]
What is the SI unit tor electrochemical equivalent?
In the electrochemical cell: Zn|ZnSO4 (0.01 M)||CuSO4 (1.0 M)|Cu, the emf of this Daniel cell is E1. When the concentration of ZnSO4 is changed to 1.0 M and that CuSO4 changed to 0.01 M, the emf changes to E2. From the above, which one is the relationship between E1 and E2?
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 \[\ce{B^+ + e^- -> B}\]
Define cathode
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 ______.
How will the pH of brine (aq. \[\ce{NaCl}\] solution) be affected when it is electrolysed?
Assertion: Mercury cell does not give steady potential.
Reason: In the cell reaction, ions are not involved in solution.
The electrochemical cell stops working after some time because
If the value of Ksp for Hg2Cl2 (s) is X then the value of X will be ____ where pX = - log X.
Given:
\[\ce{Hg2Cl2 + 2e- -> 2Hg(l) + 2Cl-}\], E° = 0.27 V
\[\ce{Hg+2 + 2e- -> 2Hg(l)}\] E° = 0.81 V
State the term for the following:
Two metal plates or wires through which the current enters and leaves the electrolytic cell.
