Nickel-cadmium (nicad) alkaline batteries are currently very popular because they maintain a constant potential and are...
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 for a nicad battery
C) If such a battery produces a current of 50 milliamps for a period of 6.00 hours, how many electrons will be transferred?
D) What mass of cadmium will undergo oxidation (or reduction) during the process in part C?
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Nickel-cadmium (nicad) alkaline batteries are currently very
popular because they maintain a constant potential and are...
The following half-reactions occur during use of the rechargeable nickel-cadmium battery: Ca(OH)2(s) + 2e → Cd(s)...
The following half-reactions occur during use of the rechargeable nickel-cadmium battery: Ca(OH)2(s) + 2e → Cd(s) + 20H(aq) NiO(OH)(s) + H20(1) + e- → Ni(OH)2(s) + OH(aq) This battery has a potential of 1.35 V under standard conditions, with nickel as the cathode. What potential does this battery produce if its hydroxide ion concentration is 1.97 x 10-2 M? E = V the tolerance is +/-2%
Help with Part C please? Not sure if I have the correct information to determine an answer
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...
5. The nickel-cadmium battery, despite issues with the toxicity of Cd, is still used in some...
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)...
A rechargeable nickel-cadmium (NiCd) battery contains the following half-reactions: NiO2 +2H2O(l)+2e– → Ni(OH)2 +2OH– E0 =0.49V...
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...
Problem 6 (16 points): One of the most common types of rechargeable batteries is known as...
Problem 6 (16 points): One of the most common types of rechargeable batteries is known as the nickel metal hydride battery, which has the overall reaction NiOOH(aq) + MH(s) - Ni(OH)2(aq) + M(S) E° = 1.35 V where M is a generic transition metal. a. (4 points) Identify the oxidizing agent and the reducing agent in this reaction. b. (4 points) How many electrons are transferred during this reaction? Show your work. c. (8 points) Such batteries need to be...
Problem 6 (16 points): One of the most common types of rechargeable batteries is known as...
Problem 6 (16 points): One of the most common types of rechargeable batteries is known as the nickel metal hydride battery, which has the overall reaction NiOOH(aq) + MH(s) - Ni(OH)2(aq) + M(S) E° = 1.35 V where M is a generic transition metal. a. (4 points) Identify the oxidizing agent and the reducing agent in this reaction. b. (4 points) How many electrons are transferred during this reaction? Show your work. C. (8 points) Such batteries need to be...
In kJ If an alkaline battery produces a cell potential of 1.62 V, what is the...
In kJ
If an alkaline battery produces a cell potential of 1.62 V, what is the value of AG cell? The half-reactions in alkaline batteries are: Zno(s) +H,0(1) +2e → Zn(s) +20H (aq) 2MnO2 (s) +H20(1) +22 → Mn,oz (s) +20H (aq)
A Nickel-Cadmium rechargeable battery can provide about 1.2 V via the following reaction, which is occurring...
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...
Mercury cells as “button” batteries are very common and consist of HgO, ZnO, and Zn(OH)2 in...
Mercury cells as “button” batteries are very common and consist of HgO, ZnO, and Zn(OH)2 in a KOH paste. Useful half-cell reactions: HgO(s) + H2O(l) + 2e = Hg(l) + 2OH-(aq) eo = 0.0977 V Zn(OH)42-(aq) + 2e = Zn(s) + 4OH-(aq) eo = -1.285 V Zn(OH)42-(aq) = ZnO(s) + H2O(l) + 2OH-(aq) A)Such batteries have a + sign marked on them. Which half-reaction is occurring at the electrode so marked? B)Draw a schematic of a mercury...
07 Question (1 point) If an alkaline battery produces a cell potential of 1.48 V, what...
07 Question (1 point) If an alkaline battery produces a cell potential of 1.48 V, what is the value of God? The half-reactions in alkaline batteries are: ZnO(s) +H,0(1) +20 - Zn(s) - 20H(aq) 2MnO, (s) +H,0() +20" Mn,0, (s) +20H(aq) 5th attempt See Periodic Table See Hint Feedback AG 2.36
The following half-reactions occur during use of the rechargeable nickel-cadmium battery: Ca(OH)2(s) + 2e → Cd(s) + 20H(aq) NiO(OH)(s) + H20(1) + e- → Ni(OH)2(s) + OH(aq) This battery has a potential of 1.35 V under standard conditions, with nickel as the cathode. What potential does this battery produce if its hydroxide ion concentration is 1.97 x 10-2 M? E = V the tolerance is +/-2%
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...
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)...
Problem 6 (16 points): One of the most common types of rechargeable batteries is known as the nickel metal hydride battery, which has the overall reaction NiOOH(aq) + MH(s) - Ni(OH)2(aq) + M(S) E° = 1.35 V where M is a generic transition metal. a. (4 points) Identify the oxidizing agent and the reducing agent in this reaction. b. (4 points) How many electrons are transferred during this reaction? Show your work. c. (8 points) Such batteries need to be...
Problem 6 (16 points): One of the most common types of rechargeable batteries is known as the nickel metal hydride battery, which has the overall reaction NiOOH(aq) + MH(s) - Ni(OH)2(aq) + M(S) E° = 1.35 V where M is a generic transition metal. a. (4 points) Identify the oxidizing agent and the reducing agent in this reaction. b. (4 points) How many electrons are transferred during this reaction? Show your work. C. (8 points) Such batteries need to be...
In kJ
If an alkaline battery produces a cell potential of 1.62 V, what is the value of AG cell? The half-reactions in alkaline batteries are: Zno(s) +H,0(1) +2e → Zn(s) +20H (aq) 2MnO2 (s) +H20(1) +22 → Mn,oz (s) +20H (aq)
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...
07 Question (1 point) If an alkaline battery produces a cell potential of 1.48 V, what is the value of God? The half-reactions in alkaline batteries are: ZnO(s) +H,0(1) +20 - Zn(s) - 20H(aq) 2MnO, (s) +H,0() +20" Mn,0, (s) +20H(aq) 5th attempt See Periodic Table See Hint Feedback AG 2.36
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