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)
Answer is given by two parts.
Answer -1
Answer - 2 is given below
These are the required solutions.
1- Consider the following redox reaction: Fe(s) + Cu2+(aq) --> Fe2+(aq) + Cu(s) EoCell =...
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.
Consider the redox reaction Fe(s) + Cu2+ (aq) — Fe2+(aq) + Cu(s) Which substance gets oxidized? Which substance gets reduced? What is the reducing agent? What is the oxidizing agent?
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1. What is the value (in V) of Eocell for the following reaction? Co2+ (aq) + Be (s) → Co (s) + Be2+ (aq) 2.What is Eocell (in V) for a redox reaction where one electron is transferred with an equilibrium constant (K) of 1.44 x 10-14? 3.Consider the following reaction: Cu2+ (aq) + Pb (s) → Cu (s) + Pb2+ (aq) What will be Ecell for this reaction (in V) when [Cu2+] = 0.500 M and [Pb2+] = 0.0350...
1.) For the complete balanced redox reaction below, what is the Eocell? Zn(s) + 2Cu+(aq) ⟶ 2Cu(s) + Zn2+(aq) Zn2+ + 2e- Zn(s) Eo = -0.76 V Cu+ + e- Cu(s) Eo = 0.52 A) -1.28 V B) +1.28 V C) 0.24 V D) -0.24 V E) +2.56 V 2.) For the redox reaction below, what is the Ecell if [Zn2+] = 0.072 M and [Cu+] = 1.27 M? T = 298 K Zn(s) + 2Cu+(aq) ⟶ 2Cu(s) + Zn2+(aq) Half Reactions:...
38. The following redox half reactions are combined in a voltaic cell. Which reaction occurs at the cathode and what is the Eceu? Fe2+(aq) + 2e → Fe(s) E°=-0.44 V Cu²+(aq) + 2e → Cu(s) E°= 0.34 V a) b) c) d) Cu2+(aq) + 2e → Cu(s), Ecell = 0.78 V Fe2+(aq) + 2e → Fe(s), Ecel = 0.78 V Fe2+(aq) + 2e → Fe(s), Ecell =-0.10 V Cu²+(aq) + 2e → Cu(s), Ecel = 0.10 V Cu²+ (aq) +...
please show work and how they got the answer 13. If [Cu2+] = 0.30 M for the same cell described below, then what concentration of Fe2+ is needed to result in Ecell = 0.76 V? You will need to use the standard reduction potential table. Cu2+/ Cu → E = +0.34 V Fe2+/ Fe → E = -0.45 Cu?* (aq) + Fe(s) - Fe* (aq) + Cu(s) Eºcell = +0.78 V, Q = x/ 0.30, X = [Fe2+], Using Nernst,...
Consider the balanced redox reaction below. 2Hg(I) + 2 Cu2 + (aq) +2CI-(aq)? Hg2CI2(aq) +2 Cu (s) Standard reduction Potentials are given below. Standard Reduction Potentials Reduction Half Reaction Cu2+ (aq) +2e-? Cu (s) 0.34 27 What is the cell potential, Ecell for the following concentrations at 298 K? Cu2+)-0.02M (CI1-0.3M [Hg2Cl21-0.005M Express your answer in units of Volts. 321
Calculate the E°cell for the following reaction: Cu2+ (aq) + Ni (s) → Cu (s) + Ni2+ (aq) A) (-0.59 ± 0.01) V B) (-0.09 ± 0.01) V C) (0.59 ± 0.01) V D) (0.09 ± 0.01) V --------------------------------------------------------------------------------------------------------- What is the proper line notation for the following reaction? Cu (s) + 2Ag+ (aq) → Cu2+ (aq) + 2Ag (s) A) Cu2+ | Cu || Ag | Ag+ B) Ag+ | Ag || Cu | Cu2+ C) Cu |...
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