Which one of the following reagents is capable of reducing Cu2+(1 M) to Cu(s)?
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Co2+(1M) |
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Br- (1M) |
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Fe |
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Au |
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Cl- (1M) |

Which one of the following reagents is capable of reducing Cu2+(1 M) to Cu(s)? Co2+(1M) Br-...
which one of the following reagents is capable of reducing Cu2+ (1M) to Cu(s)? a) I-(1M) b) Ni(s) c) Al3+ (1M) d) F-(1M) e) Ag(s)
E° (cal.) E° (exp.) 1. Fe(s)| Fe2+ (1 M) || Cu2+ (1 M) | Cu(s) 0.775 V 2. Pb(s) Pb2+ (1 M) || Cu2+ (1 M) Cu(s) 0.461 V 3. Sn(s) | Sn2+ (1 M) || Cu2+ (1 M) | Cu(s) 0.472 V 4. Zn(s) | Zn2+ (1 M) || Cu2+ (1 M) Cu(s) 1.095 V 5. Zn(s) | Zn2+ (1 M) || Cu2+ (1 M + NH3) | Cu(s) 0.928 V a) The Nernst equation for the cell in...
11. Write the balanced redox reaction corresponding to the following cell diagram: Cu(s) / Cu2+ ( 1M) || Ag+ (1M) / Ag(s)
Which of the following reagents would oxidize? 1) Which of the following reagents would oxidize Cr to Cr2 , but not Ag to Ag ? A) Co^2+ B) Ca^2+ C) Br^- D) Co E) Ca F) Br2 2) Which of the following reagents would oxidize Cu to Cu2 , but not Au to Au3 ? A) Br2 B) Co C) Co^2+ D) Br^- E) Ca^2+ F) Ca
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)
Cell: Fe(s)| Fe2+(aq, 1M) | Cu2+(aq, 1M) | Cu(S) Calculated Values ΔG° = -nFE° = ΔH° - TΔS° ΔH° = -0.34905 J/C * 2 mols * 96485 C/mol = -67,356.18 J =67.36kJ ΔS° = 0.8597 x 10-3 J/C * 2 mols * 96485 C/mol = 165.89 J ΔG° =-67356.18 J – (298*165.9 J) = -116794.4 J = -116.79 kJ Theoretical Values ΔG⁰ = -(2 mols *96485 C/mol * 1.07 J/C) = -206.48 kJ ΔH⁰ = ΔS⁰ = Cell: Zn(s)| Zn2+(aq,...
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?
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 |...
Find Ecell for the following cell. Cu(s)|CuCl(s)|Cl−(aq)(0.1M)|Cu+(aq)(1M)|Cu(s)
The Standard Cell Potential E0 for the following reaction: Zn(s) + Cu2+ (1M) --> Zn2+ (aq, 1M) + Cu(s) is E0=1.10V. What would be the cell potential E for reaction Zn(s) + Cu2+ (2M) --> Zn2+ (aq, 0.010M) + Cu(s) ? Is it smaller than 1.10V or larger than 1.10V? Explain your answer