A cell that consists of a standard hydrogen half-cell and a Cu/Cu2+ half-cell has Eo = 0.34 V. If the cell contains 0.00366 M concentrations of HCl and CuSO4, what potential does it produce?
i tried to solve it and got 0.27 but it was wrong
Lower the value of standard reduction potential, then the given electrode acts as anode and higher the value of standard reduction potential, then the given electrode acts as cathode.
a. The anode half reaction (oxidation): H2(g) -----> 2H+(aq) + 2e-
The cathode half reaction (reduction): Cu2+(aq) + 2e- ---> Cu(s)
The overall cell reaction : H2(g) + Cu2+(aq)
---> 2H+(aq) + Cu(s)
E0cell = Ec - Ea = 0.34-(0.0) = 0.34 V
The cell potential of the cell at 25 degree Celsius at diffeerent condition is given by Nernst equation
E = Eo- (0.0591/2)* log([H+]^2/[Cu2+])
= 0.34 - (0.0591/2)*log((0.00366)^2/(0.00366))
The potential for the redox reaction below at 25 degrees celsius = 0.412 v
A cell that consists of a standard hydrogen half-cell and a Cu/Cu2+ half-cell has Eo =...
A cell that consists of a standard hydrogen half-cell and a Cu/Cu2+ half-cell has Eo = 0.34 V. If the cell contains 0.00318 M concentrations of HCl and CuSO4, what potential does it produce?
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