Consider the following reaction at 25 °C;
Cu2+ (aq) + Fe (s) → Cu (s) + Fe2+ (aq); E0cell = 0.78 V (25 °C)
What would be the value of Ecell at 25 °C, if [Fe2+] = 0.40 M and [Cu2+] = 0.040 M.
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Consider the following reaction at 25 °C; Cu2+ (aq) + Fe (s) → Cu (s) +...
1- Consider the following redox reaction: Fe(s) + Cu2+(aq) --> Fe2+(aq) + Cu(s) EoCell = 0.78 V If [Cu2+] = 0.3 M, what [Fe2+] is needed so that Ecell = 0.76 V 2- Calculate the Eocell for the following redox reaction: Cu(s) + 2Ag+(aq) --> Cu2+(aq) + 2Ag(s)
I have no clue on how to do this, please help. Consider the following reaction: Cu2+ (aq) + Fe(s) → Cu(s) + Fe2+ (aq) AE° = 0.78 Volts Calculate the cell potential (AE) when the concentration of Cu2+ is 0.040 M and Fe2+ is 0.40 M.
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