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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In a common car battery, six identical cells each carry out the following reaction where two moles of e- are transferred from Pb to Pb4+:
Pb + PbO2 + 2HSO4– + 2H+ → 2PbSO4 + 2H2O (E° = 2.04 V)
For such a cell, calculate ΔG° at 25°C
A) (-98 ± 1) kJ
B) (-394 ± 1) kJ
C) (-787 ± 1) kJ
D) (-197 ± 1) kJ
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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 |...
In a common car battery, six identical cells each carry out the following reaction where two moles of e- are transferred from Pb to Pb4+: Pb + PbO2 + 2HSO4– + 2H+ → 2PbSO4 + 2H2O (E° = 2.04 V) For such a cell, calculate ΔG° at 25°C A) (-98 ± 1) kJ B) (-394 ± 1) kJ C) (-787 ± 1) kJ D) (-197 ± 1) kJ ------------------------------------------------------------------------------------------------------------ Calculate Ecell at 298K for a concentration cell made with silver...
electro Calculate the E°cell for the following reaction: Cu2+ (aq) + Ni (s) → Cu (s) + Ni2+ (aq)
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Given that E o = 0.52 V for the reduction Cu+(aq) + e− → Cu(s), calculate E o , ΔG o , and K for the following reaction at 25°C: 2Cu+(aq) ⇌ Cu2+(aq) + Cu(s) E o = V ΔG o = kJ K = × 10 Enter your answer in scientific notation.
Identify the complete redox reaction for a CulCu2+||Ag+Ag cell. A. Cu(s) + Ag(s) Cu2+ (aq) + Ag+ (aq) B. Cu(s) + Ag+ (aq) + Cu2+ (aq) + Ag(s) c. Cu(s) + 2 Ag+ (aq) (aq) + 2 Ag(s) D. Cu²+ (aq) + 2 Ag(s) + Cu(s) + 2 Ag+ (aq) → Cu2+
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)
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