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In cell reactions , oxidation takes place at anode and reduction
takes place at cathode.![is Zncs] + 200H) -> Zn(OH), +2é - In this So it ic reaction loss of electrons takes Oxidation Reactions (Anode) plance. Fi Ag](http://img.homeworklib.com/questions/ad41f7e0-70fd-11ea-bae1-cbf38e89f6e9.png?x-oss-process=image/resize,w_560)
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2) A silver oxide-zinc cell maintains a fairly constant voltage during dis charge (1.60V). The button...
4. Silver oxide is used in "button batteries to power electric watches and other trinkets. These ...
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4. Silver oxide is used in "button batteries to power electric watches and other trinkets. These batteries generate a potential of 1.55 V and consist of a Zn anode and a Ag20 cathode immersed in a concentrated solution of KOH. The cathode reaction is based on the reduction of Ag20 to Ag metal. At the anode, Zn is oxidized to solid Zn(OH)2. Write the net ionic balanced electrochemical cell reaction and calculate the value...
please solve all correctly Question: Consider the voltaic cell using silver and zinc. The net equation...
please solve all correctly
Question: Consider the voltaic cell using silver and zinc. The net equation for this voltaic cell is 2Ag+ (aq) + Zn(s)--> 2Ag(s) + Zn2+lag) Calculate the molar concentration of Ag+ if a potential of 1.58 V was measured across the cell when the molar concentration of Zn* was 0.150 M. Hint: You need to first calculate the of the cell. Given the following Data: Be sure to show all calculations Half-Reaction Standard Potential E* (volts) Ag...
A silver-zinc button cell battery is the type of battery found in watches and other small...
A silver-zinc button cell battery is the type of battery found in watches and other small electronics. The balanced redox reaction is shown below. Zn(s) + Ag2O(s)---- ZnO(s)+ 2Ag(S) Using the following thermodynamic data, determine what the voltage would be for E cell. rG [ZnO]= -318.3 kj/mol rG [Ag2O]= -11.20 kj/mol
Table 1 Cell Type Lithium-iodine Zinc-mercury Operating Cell Potential for Commercial Batteries, E (V) +2.80 +1.35...
Table 1 Cell Type Lithium-iodine Zinc-mercury Operating Cell Potential for Commercial Batteries, E (V) +2.80 +1.35 Table 2 Standard Reduction Potential, E" (V) Half-Reaction Zn(OH).1? +2e → Zn +40H Zn(OH), +2e → Zn +20H HgO + H2O +2e - Hg + 2OH 0, + 2 H2O + 4e 40H - 1.20 |--1.25 +0.10 +0.40 Pacemakers are electronic devices that help regulate the heart rate. Currently, lithium-iodine cells are commonly used to power pacemakers and have replaced zinc-mercury cells. Table 1...
In a copper-zinc voltaic cell, one half-cell consists of a ZnZn electrode inserted in a solution...
In a copper-zinc voltaic cell, one half-cell consists of a ZnZn
electrode inserted in a solution of zinc sulfate and the other
half-cell consists of a CuCu electrode inserted in a copper sulfate
solution. These two half-cells are separated by a salt bridge.
At the zinc electrode (anode), ZnZn metal undergoes oxidation by
losing two electrons and enters the solution as Zn2+Zn2+ ions. The
oxidation half-cell reaction that takes place at the anode is
Zn(s)→Zn2+(aq)+2e−Zn(s)→Zn2+(aq)+2e−
The CuCu ions undergo reduction...
A zinc air battery has the following reactions at the two electrodes: 1⁄2 O2 + H2O...
A zinc air battery has the following reactions at the two electrodes: 1⁄2 O2 + H2O + 2e- -> 2OH- Zn -> Zn2+ +2e- Zn&2+ + 2OH- -> Zn(OH)^2 a) Which of these reactions occurs at the anode and which at the cathode? Explain your answer. b) Determine the two half-cell potentials at the electrode-electrolyte interfaces using standard Gibbs free energy values (Note: Assume the phase of the Zn(OH)2 is the epsilon phase.) c) A zinc air battery is typically...
The silver oxide-zinc battery used in watches delivers a voltage of 1.60 V. Using this information...
The silver oxide-zinc battery used in watches delivers a voltage of 1.60 V. Using this information and the balanced chemical equation, calculate the standard free energy change for the cell reaction at 25C. Balanced equation: Zn(s) + Ag2O(s) --> ZnO(s) + 2 Ag(s)
8 pts Question 5 The silver oxide-zinc battery used in watches delivers a voltage of 1.60...
8 pts Question 5 The silver oxide-zinc battery used in watches delivers a voltage of 1.60 V. Using this information and the balanced chemical equation calculate the standard free energy change for the cell reaction at 25C. Balanced equation: Zn(s) + Ag2015) --> ZnO(s) + 2 Ag(s) 154) 154] 310 -310
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...
salt bridge Zn(s) electrode Culs) electrode 1.0M Zn (a 1.0 M Cu (aq A voltaic cell...
salt bridge Zn(s) electrode Culs) electrode 1.0M Zn (a 1.0 M Cu (aq A voltaic cell similar to that shown in the figure above is constructed. The electronic device shown at the top of the figure is a volt meter. One electrode compartment consists of a zinc strip placed in a 1.0 M ZnCl2 solution, and the other has a copper strip placed in a 1.0 M CuSOA solution. The overall cell reaction is: Zn(s)Cu2+(aq)= zn2+ (aq ) Cu (s)...
can u answer the following
questions?
4. Silver oxide is used in "button batteries to power electric watches and other trinkets. These batteries generate a potential of 1.55 V and consist of a Zn anode and a Ag20 cathode immersed in a concentrated solution of KOH. The cathode reaction is based on the reduction of Ag20 to Ag metal. At the anode, Zn is oxidized to solid Zn(OH)2. Write the net ionic balanced electrochemical cell reaction and calculate the value...
please solve all correctly
Question: Consider the voltaic cell using silver and zinc. The net equation for this voltaic cell is 2Ag+ (aq) + Zn(s)--> 2Ag(s) + Zn2+lag) Calculate the molar concentration of Ag+ if a potential of 1.58 V was measured across the cell when the molar concentration of Zn* was 0.150 M. Hint: You need to first calculate the of the cell. Given the following Data: Be sure to show all calculations Half-Reaction Standard Potential E* (volts) Ag...
Table 1 Cell Type Lithium-iodine Zinc-mercury Operating Cell Potential for Commercial Batteries, E (V) +2.80 +1.35 Table 2 Standard Reduction Potential, E" (V) Half-Reaction Zn(OH).1? +2e → Zn +40H Zn(OH), +2e → Zn +20H HgO + H2O +2e - Hg + 2OH 0, + 2 H2O + 4e 40H - 1.20 |--1.25 +0.10 +0.40 Pacemakers are electronic devices that help regulate the heart rate. Currently, lithium-iodine cells are commonly used to power pacemakers and have replaced zinc-mercury cells. Table 1...
In a copper-zinc voltaic cell, one half-cell consists of a ZnZn
electrode inserted in a solution of zinc sulfate and the other
half-cell consists of a CuCu electrode inserted in a copper sulfate
solution. These two half-cells are separated by a salt bridge.
At the zinc electrode (anode), ZnZn metal undergoes oxidation by
losing two electrons and enters the solution as Zn2+Zn2+ ions. The
oxidation half-cell reaction that takes place at the anode is
Zn(s)→Zn2+(aq)+2e−Zn(s)→Zn2+(aq)+2e−
The CuCu ions undergo reduction...
The silver oxide-zinc battery used in watches delivers a voltage of 1.60 V. Using this information and the balanced chemical equation, calculate the standard free energy change for the cell reaction at 25C. Balanced equation: Zn(s) + Ag2O(s) --> ZnO(s) + 2 Ag(s)
8 pts Question 5 The silver oxide-zinc battery used in watches delivers a voltage of 1.60 V. Using this information and the balanced chemical equation calculate the standard free energy change for the cell reaction at 25C. Balanced equation: Zn(s) + Ag2015) --> ZnO(s) + 2 Ag(s) 154) 154] 310 -310
salt bridge Zn(s) electrode Culs) electrode 1.0M Zn (a 1.0 M Cu (aq A voltaic cell similar to that shown in the figure above is constructed. The electronic device shown at the top of the figure is a volt meter. One electrode compartment consists of a zinc strip placed in a 1.0 M ZnCl2 solution, and the other has a copper strip placed in a 1.0 M CuSOA solution. The overall cell reaction is: Zn(s)Cu2+(aq)= zn2+ (aq ) Cu (s)...
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