PartA Identify the reactant that is oxidized in the following reaction. Cu(s) + 2Ag (aq) -...
For the reaction Cu (s) + 2Ag+ (aq) Cu2+ (aq) + 2Ag (s) at 25 °C, the cell potential is found to be 0.62 V. Everything is at standard state except the Cu2+ (aq). Calculate [Cu2+].
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 |...
Which of the following elements is being oxidized in the reaction below? Cu (s) + 2AgNO3 (aq) + 2Ag (s) + Cu(NO3)2 (aq) Cu(NO3)2 Ag o Cu ON
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 |...
Based on the reactions blow arrange the metals in their increasing reactivity. Cu(s)+ 2Ag+(aq)-->Cu2+(aq)+ 2Ag(s) 2Ag+(aq)+Zn(s)--->Zn2+(aq)+2Ag(s) Zn(s)+Cu2+(aq)-->Zn2+(aq)+Cu(s)
In each of the following reactions, identify the reactant that is oxidized and the reactant that is reduced: (its multiple choice) Number 1: Br2(g)+2KI(aq)→2KBr(aq)+I2(s) I− (in KI) loses electrons and is oxidized. Br2 gains electrons and is reduced. Br2 gains electrons and is oxidized. I− (in KI) loses electrons and is reduced. I− (in KI) gains electrons and is oxidized. Br2 loses electrons and is reduced. Br2 loses electrons and is oxidized. I− (in KI) gains electrons and is reduced....
a Cu(s) + 2Ag+ (aq) → 2 Ag(s) + Cu2+ (aq) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced b HCl(g) + NH3 (g) → NH4Cl(s) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced c SiCl4 (l) + 2H2O(l) → 4HCl(aq) + SiO2 (s) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced d C14 (1) + 2Mg(s) + 2MgCl2(8) + Si(s) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced e Al(OH)4-(aq) → AIO2- (aq) + 2H2O(l) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced
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)
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