Advertisements
Advertisements
Question
Using the E° values of A and B, predict which is better for coating the surface of iron [E°(Fe+2/Fe) = -0.44V] to prevent corrosion and why?
Given: E° (A+2/A)=-2.37 V: E°(B+2/B)= -0.14V
Advertisements
Solution
Given:
E°(A+2 / A) = 2.37 V
E°(B+2 / B) = -0.14 V
`E_(cell)=E_(cell)^@ - (0.0591)/n log [Cr^(3+)]^2/[Fe^(2+)]^3`
(Nernst Equation)
`0.261 = E_(cell)^@ = 0.0591/6 log [0.001]^2/[0.001]^3`
`0.261 = E_(cell)^@ - (0.591 xx 2)/6`
`E_(cell)^@ = 0.2807V`
APPEARS IN
RELATED QUESTIONS
The charge of how many coulomb is required to deposit 1.0 g of sodium metal (molar mass 23.0 g mol-1) from sodium ions is -
- 2098
- 96500
- 193000
- 4196
96500 coulombs correspond to the charge on how many electrons?
How much electricity in terms of Faraday is required to produce 20 g of Ca from molten CaCl2?
(Given: Molar mass of Calcium is 40 g mol−1.)
Number of faradays of electricity required to liberate 12 g of hydrogen is:
How much charge is required for the following reduction?
1 mol of Cu2+ to Cu.
Three electrolytic cells A, B, C containing solutions of ZnSO4, AgNO3 and CuSO4, respectively, are connected in series. A steady current of 1.5 amperes was passed through them until 1.45 g of silver deposited at the cathode of cell B. How long did the current flow? What mass of copper and zinc were deposited?
State second law of electrolysis
What will happen during the electrolysis of aqueous solution of CuSO4 in the presence of Cu electrodes?
(i) Copper will deposit at cathode.
(ii) Copper will dissolve at anode.
(iii) Oxygen will be released at anode.
(iv) Copper will deposit at anode.
The quantity of electricity needed to separately electrolyse 1 M solution of ZnSO4, AlCl3, and AgNO3 completely is in the ratio of ______.
A current of 4 amp was passed for 2 hours through a solution of copper sulphate when 5.0 g of copper was deposited. The current efficiency is ______% (Cu = 63.5).
