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
How much charge is required for the following reduction?
1 mol of Al3+ to Al.
How much charge is required for the following reduction?
1 mol of Cu2+ to Cu.
Calculate the mass of Ag deposited at cathode when a current of 2 amperes was passed through a solution of AgNO3 for 15 minutes.
(Given : Molar mass of Ag = 108 g mol−1 lF = 96500 C mol−1)
According to Faraday’s First Law of Electrolysis, the amount of chemical reaction which occurs at any electrode during electrolysis by a current is proportional to the ____________.
In the electrolysis of aqueous sodium chloride solution which of the half cell reaction will occur at anode?
Assertion: Electrolysis of NaCl solution gives chlorine at anode instead of O2.
Reason: Formation of oxygen at anode requires overvoltage.
Time Required to deposite one millimole of aluminium metal by the passage of 9.65 ampere through aqueous solution of aluminium is
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).
On passing electricity through nitrobenzene solution, it is converted into azobenzene. The mass of azobenzene is ______ mg, if the same quantity of electricity produces oxygen just sufficient to burn 96 mg of fullerene (C60)·
How much electricity in terms of Faraday is required to produce 40.0 g of Al from molten Al2O3?
(Given: Molar mass of Aluminium is 27 g mol−1.)
