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The following half-reactions occur during use of the rechargeable nickel-cadmium battery: Ca(OH)2(s) + 2e → Cd(s)...
A rechargeable nickel-cadmium (NiCd) battery contains the following half-reactions: NiO2 +2H2O(l)+2e– → Ni(OH)2 +2OH– E0 =0.49V Cd(OH)2 +2e– →Cd(s)+2OH– E0 =–0.81V a. What is the standard cell potential or voltage of this NiCd cell? b. Write the net chemical reaction in the direction of spontaneous reaction. Is cadmium oxidized or reduced? c. Write an expression for the reaction quotient Q. What is Q if the electrolyte concentrations are: [NiO2] = 1 M and [Cd(OH)2] = 0.01M and [Ni(OH)2] = 0.001...
5. The nickel-cadmium battery, despite issues with the toxicity of Cd, is still used in some rechargeable batteries because it has very consistent voltage over long discharge times. a) Using only half-cell reactions given in Table 16.1, write the overall reaction and give the highest AV° value possible for a NiCd battery. b) The actual half-cell reactions used in a Nicd battery are: Ca(OH)2(8) + 2e → Cds + 2OH(aq) (Vº = -0.86V) NiO(OH)) + H2O) +e Ni(OH)2(s) + OH(aq)...
Help with Part C please? Not sure if I have the correct information to determine an answer Problems 1. Given the standard reduction potentials Cd(OH)2(s) +2e → Cd(s) + 2 OH-(aq) В"--0.76 V Ni0(OH)(s) + H20() + r-, Ni(OH)2(s) + OH-(aq) E。_ +0.49 V Write the reactions for the discharge and charge of a nickel-cadmium rechargeable battery. a. b. Calculate the standard potential of this battery. A typical nicad battery has a potential of 1.30 V. Why is there a...
Nickel-cadmium (nicad) alkaline batteries are currently very popular because they maintain a constant potential and are rechargeable. The relevant half-cell reactions for such batteries are given in this table. Half-Reaction, Cd(OH)2(s) + 2e- -> Cd(s) + 2 OH- (aq) E(volts) = -0.809 NiOOH(s)+ H2O(l) + e- -> Ni(OH)2(s)+OH-(aq) E(volts) = +0.490 A) Write a balanced equation for the process that produces electricity in a nicad battery and specify the half- reaction that occurs at the anode. B) Calculate the potential expected...
A Nickel-Cadmium rechargeable battery can provide about 1.2 V via the following reaction, which is occurring in the battery: Cd(s) + NiO2(s) + 2H2O(1) 4Cd(OH)2 + Ni(OH)2(s) Eventually, the battery dies and you have to plug in your battery-powered device to recharge the battery. While the battery is plugged in and being recharged, what chemical reaction occurs in the battery? (We didn't really talk about it, but you're smart people so use your brains!) - The forward reaction as shown...
In a nickel-cadmium battery, NiO(OH) is reduced to: Ni(OH)4, NiOH, NiO2, Ni, or Ni(OH)2
Classify the half-reactions as reduction half-reactions or oxidation half-reactions. H(g)2 H (aq) +2e Answer Bank 0, (8)+2H (aq)+2e H,O(g) oxidation reduction Cd(s)+20H (aq) Cd(OH), (s) + 2 e 2 NiO (OH)(s)+2H,O(1)+2 e 2 Ni(OH), (s)+ 2 OH (aq) Fe(s)Fe (aq) +2 e
Consider the half‑reaction for the reduction of Cd 2+ Cd2+ to Cd(s) Cd(s) . Cd 2 +(aq)+2 e − ⟶Cd(s) ? ∘ Cd 2+ /Cd =−0.403 V Cd2+(aq)+2e−⟶Cd(s)ECd2+/Cd∘=−0.403 V Calculate the potential of the cadmium electrode at 25 ∘ C 25 ∘C when immersed in a 0.0560 M 0.0560 M solution of CdBr 2 . CdBr2. ? Cd = ECd= V V Calculate the potential of the cadmium electrode at 25 ∘ C 25 ∘C when immersed in a 0.0330...
Classify the half‑reactions as reduction half‑reactions or oxidation half‑reactions. H2(g)⟶2H+(aq)+2e−H2(g)⟶2H+(aq)+2e− 12O2(g)+2H+(aq)+2e−⟶H2O(g)12O2(g)+2H+(aq)+2e−⟶H2O(g) Cd(s)+2OH−(aq)⟶Cd(OH)2(s)+2e−Cd(s)+2OH−(aq)⟶Cd(OH)2(s)+2e− 2NiO(OH)(s)+2H2O(l)+2e−⟶2Ni(OH)2(s)+2OH−(aq)2NiO(OH)(s)+2H2O(l)+2e−⟶2Ni(OH)2(s)+2OH−(aq) Fe(s)⟶Fe2+(aq)+2e−Fe(s)⟶Fe2+(aq)+2e− oxidation reduction reduction oxidation reduction
NiCad battery: Ca(OH)2 (s) + 2 eCd (s) + 2 OH- (aq) E° = -0.40 V 2 NiOOH (s) + 2 H2O () + 2 e + 2 Ni(OH)2 (s) + 2 OH- (aq) E° = 1.32 V Calculate the cell potential, Eºcell, using the formula Eºcell = Eºcathode - E°anode. Include the correct unit. Answer: Check