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
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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 | Cu2+ || Ag+ | Ag
D) Ag | Ag+ || Cu2+ | Cu
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Based on the table of standard reduction potentials, which of the following would be the strongest reducing agent at 298K
A) Zn2+ (aq)
B) Ni (s)
C) F- (aq)
D) Cu (s)
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Calculate the E°cell for the following reaction: Cu2+ (aq) + Ni (s) → Cu (s)...
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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electro Calculate the E°cell for the following reaction: Cu2+ (aq) + Ni (s) → Cu (s) + Ni2+ (aq)
Calculate the Ecell value at 298 K for the cell based on the reaction: Cu(s) + 2Ag+ (aq) → Cu2+ (aq) + 2Ag(s) where [Ag+] = 0.00350 M and [Cu2+] = 7.00x10-4 M. The standard reduction potentials are shown below: Ag+(aq) +e → Ag(s) E° = 0.7996 V Cu2+ (aq) + 2e -→ Cu(s) E° = 0.3419 V 2nd attempt Ecell = V
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Calculate the cell potential for the reaction below when the concentrations of ions are: [Ag+ ] = 0.010 M and [Cu2+] = 0.750 M, at 25 °C. Cu(s) + 2Ag+ (aq) --> Cu2+(aq) + 2Ag(s) Given the standard reduction potentials: Cu2+(aq) + 2e– → Cu(s) Eϴ = 0.34 V Ag+ (aq) + e– → Ag(s) Eϴ = 0.80 V (A) 0.35 V (B) 0.44 V (C) 0.46 V (D) 0.48 V (E) 0.57 V
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