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You intend to construct a very expensive) battery using PtCl2/Pt and AgNO3/Ag as your materiais Which...
You intend to construct a very expensive battery using PtCl2/Pt and AgNO/Ag as your materiais Which...
You intend to construct a very expensive battery using PtCl2/Pt and AgNO/Ag as your materiais Which half-reaction is the anode, and which is the cathode? PtCl (aq) + 2e - Pt(s) + 2 Cl. (aq) E= +1.20 V AgNO3(aq) + e - Ag (s) + NO3- (aq) E = +0.80 V Explain how you determined the appropriate half reaction for the anode. Calculate Ecall for the battery you have constructed. Ecell = Write the balanced equation for the overall reaction...
Table provided below for context Please answer all parts that you can. 1. Which electrochemical cell...
Table provided below for context
Please answer all parts that you can.
1. Which electrochemical cell had the greatest voltage? Identify the anode and the cathode for this pair, the measured cell potential, and the calculated Eºcell- 2. Which electrochemical cell had the smallest voltage? Identify the anode and the cathode for this pair, the measured cell potential, and the calculated Eºcell- 3. If the oxidation and reduction half-reactions are separated in a battery, this means the oxidizing agent is...
17.32. Voltaic cells based on the following pairs of half-reactions are constructed. For each pair, write a balance...
17.32. Voltaic cells based on the following pairs of half-reactions are constructed. For each pair, write a balanced equation for the cell reaction, and identify which half-reaction takes place at each anode and cathode. a. Cdº'(aq) + 2 e - Cd(s) Agt(aq) + e - Ag(s) b. AgBr(s) + e - Ag(s) + Br"(aq) MnO2(s) + 4 H*(aq) + 2 e-Mn2(aq) + 2 H2O(0) c. PtCl 2- (aq) + 2 e-Pt(s) + 4 Cl(aq) AgCl(s) + e- Ag(s) + Cl(aq)
Given are two half-cells, described by the equations: Zn^(2+)(aq) + 2e- -> Zn(s) E(standard) = -0.76 V Ag^(+)(aq) + e...
Given are two half-cells, described by the equations: Zn^(2+)(aq) + 2e- -> Zn(s) E(standard) = -0.76 V Ag^(+)(aq) + e- -> Ag(s) E(standard) = +0.80 V A. Write down the net equation for the spontaneous reaction that takes place in the cell. B. Draw the two half cells and mark the anode and the cathode. C. Mark the solutions' concentration necessary in order to reach the standard potential. D. How will the cell's potential be influenced by the addition of...
Standard Reduction Please write your answers here Reduction Half-Reactin Potential (V) F2(g) + 2e-→ 2F-(aq) S2082 (ag) +2e-2SO42(ag) O2(g) + 4H(a)+ 4e 2H200) +2.87 +2.01 +1.23 +1.09 +0.80 +0.77 +0.54...
Standard Reduction Please write your answers here Reduction Half-Reactin Potential (V) F2(g) + 2e-→ 2F-(aq) S2082 (ag) +2e-2SO42(ag) O2(g) + 4H(a)+ 4e 2H200) +2.87 +2.01 +1.23 +1.09 +0.80 +0.77 +0.54 +0.34 +0.15 +0.14 0.00 0.14 0.26 0.44 0.74 0.76 0.83 1.18 2.71 3.04 2 4 Ag+(aq) + e-→ Ag(s) Fe3+(ag)eFe2*(aq) 20)+ 2e- 21(aq) Cu2(ag)+ 2e Cus) SAMPLE QUIZ 4 S(s) + 2H+(aq) + 2e. → H2S(g) 2H(a)+ 2eH2g) Sn2(ag) 2e Sng) 1. What is the purpose of the salt bridge...
Draw out a cell for Al in Al(NO3)3 and Ag in AgNO3. Label the anode and...
Draw out a cell for Al in Al(NO3)3 and Ag in AgNO3. Label the anode and cathode sides, including charge on each electrode. (hint: use a table of standard reduction potentials). Indicate direction of electron flow. Write the net reaction, and the half reactions. What is the standard cell potential? Indicate for both electrodes whether they are dissolving, growing, or staying the same size. Assuming the salt bridge contains KNO3, indicate flow of ions into and out of salt bridge....
Half-cell Potentials: Half Reaction: E value +0.80 V Agt + e → Ag Fe3+ + €...
Half-cell Potentials: Half Reaction: E value +0.80 V Agt + e → Ag Fe3+ + € → Fe2+ +0.77 v +0.34 V -0.13 V Cu2+ +2e → Cu Pb2+ + 2e - → Ib Ni2+ + 2e → Ni Cd2+ +2e → Cd -0.25 V -0.40 V Fe2+ + 2e → Fe -0.44 V Zn2+ + 2e → Zn -0.76 V Al3+ +3e → AI - 1.66 V Consider an electrochemical cell constructed from the following half cells, linked by...
please help fill out chart 1 by using the data belowed thank you! DATA:Cag] "Ay No₃...
please help fill out chart 1 by using the data belowed thank
you!
DATA:Cag] "Ay No₃ cell cell CUCNO3)27144-1.0m AgNO3 ! Agu = 10M Part I: Cell Potential of voltaic cells under standard conditions: Give the half Half cell reaction at Oxidation Combinations Reduction E the anode and Theoretical with [ion] takes place takes place cathode. Write in M here here (V) above the arrow if it is oxidation or reduction. -0.340 Ag - Cu Cucs) Agters oxi Anode: 0.3440.00...
Use the tables on the next page and your initials to generate a ‘cell diagram’ where...
Use the tables on the next page and your
initials to generate a ‘cell diagram’ where the first
reaction (first initial) is the anode and the second reaction
(second initial) is the cathode and determine whether the reaction
is spontaneous. For gasses, assume an inert Platinum electrode.
First Initial: K . Last Initial: D
Rxn K --> anode (off table, as a reduction) Zn
+2(aq) + 2 e- -----> Zn(s)
Rxn S --> cathode (off table) ...
Refer to this table of reduction potentials to answer the questions. Reduction half-reaction Potential (V) +2.87...
Refer to this table of reduction potentials to answer the questions. Reduction half-reaction Potential (V) +2.87 Electrolytic cells use electricity to cause a nonspontaneous redox reaction to occur. An electrolytic cell is constructed using the following components: • a power source, such as a battery, • the substance that will undergo electrolysis, and • two inert electrodes (usually platinum), which serve as the electrical connection between the power source and the substance undergoing electrolysis. As with any cell, oxidation occurs...
You intend to construct a very expensive battery using PtCl2/Pt and AgNO/Ag as your materiais Which half-reaction is the anode, and which is the cathode? PtCl (aq) + 2e - Pt(s) + 2 Cl. (aq) E= +1.20 V AgNO3(aq) + e - Ag (s) + NO3- (aq) E = +0.80 V Explain how you determined the appropriate half reaction for the anode. Calculate Ecall for the battery you have constructed. Ecell = Write the balanced equation for the overall reaction...
Table provided below for context
Please answer all parts that you can.
1. Which electrochemical cell had the greatest voltage? Identify the anode and the cathode for this pair, the measured cell potential, and the calculated Eºcell- 2. Which electrochemical cell had the smallest voltage? Identify the anode and the cathode for this pair, the measured cell potential, and the calculated Eºcell- 3. If the oxidation and reduction half-reactions are separated in a battery, this means the oxidizing agent is...
17.32. Voltaic cells based on the following pairs of half-reactions are constructed. For each pair, write a balanced equation for the cell reaction, and identify which half-reaction takes place at each anode and cathode. a. Cdº'(aq) + 2 e - Cd(s) Agt(aq) + e - Ag(s) b. AgBr(s) + e - Ag(s) + Br"(aq) MnO2(s) + 4 H*(aq) + 2 e-Mn2(aq) + 2 H2O(0) c. PtCl 2- (aq) + 2 e-Pt(s) + 4 Cl(aq) AgCl(s) + e- Ag(s) + Cl(aq)
Standard Reduction Please write your answers here Reduction Half-Reactin Potential (V) F2(g) + 2e-→ 2F-(aq) S2082 (ag) +2e-2SO42(ag) O2(g) + 4H(a)+ 4e 2H200) +2.87 +2.01 +1.23 +1.09 +0.80 +0.77 +0.54 +0.34 +0.15 +0.14 0.00 0.14 0.26 0.44 0.74 0.76 0.83 1.18 2.71 3.04 2 4 Ag+(aq) + e-→ Ag(s) Fe3+(ag)eFe2*(aq) 20)+ 2e- 21(aq) Cu2(ag)+ 2e Cus) SAMPLE QUIZ 4 S(s) + 2H+(aq) + 2e. → H2S(g) 2H(a)+ 2eH2g) Sn2(ag) 2e Sng) 1. What is the purpose of the salt bridge...
Half-cell Potentials: Half Reaction: E value +0.80 V Agt + e → Ag Fe3+ + € → Fe2+ +0.77 v +0.34 V -0.13 V Cu2+ +2e → Cu Pb2+ + 2e - → Ib Ni2+ + 2e → Ni Cd2+ +2e → Cd -0.25 V -0.40 V Fe2+ + 2e → Fe -0.44 V Zn2+ + 2e → Zn -0.76 V Al3+ +3e → AI - 1.66 V Consider an electrochemical cell constructed from the following half cells, linked by...
please help fill out chart 1 by using the data belowed thank
you!
DATA:Cag] "Ay No₃ cell cell CUCNO3)27144-1.0m AgNO3 ! Agu = 10M Part I: Cell Potential of voltaic cells under standard conditions: Give the half Half cell reaction at Oxidation Combinations Reduction E the anode and Theoretical with [ion] takes place takes place cathode. Write in M here here (V) above the arrow if it is oxidation or reduction. -0.340 Ag - Cu Cucs) Agters oxi Anode: 0.3440.00...
Use the tables on the next page and your
initials to generate a ‘cell diagram’ where the first
reaction (first initial) is the anode and the second reaction
(second initial) is the cathode and determine whether the reaction
is spontaneous. For gasses, assume an inert Platinum electrode.
First Initial: K . Last Initial: D
Rxn K --> anode (off table, as a reduction) Zn
+2(aq) + 2 e- -----> Zn(s)
Rxn S --> cathode (off table) ...
Refer to this table of reduction potentials to answer the questions. Reduction half-reaction Potential (V) +2.87 Electrolytic cells use electricity to cause a nonspontaneous redox reaction to occur. An electrolytic cell is constructed using the following components: • a power source, such as a battery, • the substance that will undergo electrolysis, and • two inert electrodes (usually platinum), which serve as the electrical connection between the power source and the substance undergoing electrolysis. As with any cell, oxidation occurs...
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