Homework Answers
In anode always oxidation take place
& in cathode reduction take place
So in this question you correctly shows oxidation in anode and reduction in cathode and E°cell = Reduction potential of (cathode- anode).
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help did i do this correct?
a ws4 wws C PRE-L AX I Mycs aws4 Panapowe...
need help for half cell potentials pls calculate step by step (NOTE - Remember that the...
need help for half cell potentials pls calculate step by step
(NOTE - Remember that the positive electrode is attached to the red wire and the negative electrode is attached to the black wire.) Electrode Systems Used Anode (oxidation) Negative Cathode (reduction) Positive Measured Potential (V) Positive (Ecu) Copper and silver Cu() - Cu2+ + 2e" Ag+ +1e Ag) 0.432 V Zinc + Silver Zn cs + 2n**+ Zé dat + leº nAg (s) 1.484 V Copper & Zinc Zn(s)...
need help with the rest of the table EXPERIMENT 10 DETERMINATION OF THE ELECTROCHEMICAL SERIES PURPOSE...
need help with the rest of the table
EXPERIMENT 10 DETERMINATION OF THE ELECTROCHEMICAL SERIES PURPOSE To determine the standard cell potential values of several electrochemical coll INTRODUCTION The basis for an electrochemical cell is an oxidation reduction Corredor be divided into two half reactions reaction. This reaction can Oxidation half reaction Gloss of electrons) takes place at the anode, which is the positive electrode that the anions migrate to Chence the name anode) Reduction half reaction (gain of electrons)...
I need help with questione 1-12 and discussion question 1 and 2. The previous pictures help...
I need help with questione 1-12 and discussion question 1 and
2. The previous pictures help determine the chart. Please Show Work
thank you so much
An oxidation half-reaction is characterized by electrons appearing on the product side. The oxidation of aluminum for instance would be represented thusly: Al(s) → Al3+ + 3e- (1) An reduction half-reaction is characterized by electrons appearing on the reactant side. The reduction of ferrous iron for instance would be represented thusly: Fe2+ + 2e...
Using the table below: 19. Three combinations of metals are listed below, which combination would produce...
Using the table below:
19. Three combinations of metals are listed below, which
combination would produce the largest voltage if they were used to
construct an electrochemical cell?
Copper (Cu) with zinc (Zn)
Lead (Pb) with zinc (Zn)
Lead (Pb) with cadmium (Cd)
Liu lur the reaction between Zn and Cu2+ ions is 1.1030 V, we can use the known value for the half-cell potential for zinc to determine the half-cell potential for copper: Zn(s) → Zn2+(aq) + 2e +...
For electrochemistry cell, the reduction of silver ions is helped b the oxidation of zinc. Given...
For electrochemistry cell, the reduction of silver ions is helped b the oxidation of zinc. Given the standard reduction half reactions, what is the standard potential of the cell? Ag* + e + Ag Ered= 0.799 V Zn²+ + 2e → Zn Ered = 0.763 V
Using the information in the table: Which combination of metals, if used to create an electrochemical...
Using the information in the table:
Which combination of metals, if used to create an
electrochemical cell, would produce the largest voltage?
Liu lur the reaction between Zn and Cu2+ ions is 1.1030 V, we can use the known value for the half-cell potential for zinc to determine the half-cell potential for copper: Zn(s) → Zn2+(aq) + 2e + Cu2+(aq) + 2e → Cu(s) Zn(s) + Cu2+ (aq) → Zn2+ (aq) + Cu(s) E half-cell = 0.7628 V Eºhalf-cell =...
how would you go about solving this problem via using equations just looking for the equation order i should go about solving this problem In this experiment you will be using the two half rea...
how
would you go about solving this problem via using equations
just looking for the equation order i should go about solving this
problem
In this experiment you will be using the two half reactions Cu?"/Cu and Zn2 /Zn. The standard electrode potential, E°, for these half reactions is +0.34V and-0.76V respectively, so the Nernst Equation for these half reactions is the following Cu ea)+2e - Cus) E - 0.34V 0.0592V Cu2+] 0.0592V Zn 2 Note that solids by definition...
i need help with all of these questions Chem 103A Electrochemistry 5. A voltaic cell is...
i need help with all of these questions
Chem 103A Electrochemistry 5. A voltaic cell is to be constructed using the Ag/Ag half cell and the Pb/Pb half-cell. Measurement shows that the silver electrode is positive. a) Write balanced half-reactions and the overall spontancous reaction, without using a table of half-cell potentials. b) Diagram the cell, labeling electrodes as anode and cathode, labeling the salt bridge, showing what ions are in solution, and showing the direction of electron flow in...
My percent error is high so before I keep going I wanted to make sure I...
My percent error is high so before I keep going I wanted to
make sure I am doing this right. Can someone check this over and
make sure everything is right?
Ered (V) Half-reaction F(g)+2e2F" (aq) Cl,(g)+2e2C (aq) Ag (aq)+leAg(s) Fe (aq)+le Fe (aq) Cu (aq)+2e-> Cu(s) 2H (aq)+2eH, (g) Ni (aq)+2eNi(s) Cd (aq)+2eCd(s) Fe (aq)+2e Fe(s) Zn2 (aq)+2e-> Zn(s) 2.87 1.36 0.80 0.77 0.34 0.00 0.28 -0.40 -0.44 -0.76 Mg (aq)+2e- Mg(s) -2.37 Table 1. Standard Reduction Potential for...
Chem 1212 Lab Report on electrochemistry Electrochemistry When electrons transfer between reaction components in a redox...
Chem 1212 Lab Report on electrochemistry
Electrochemistry When electrons transfer between reaction components in a redox reaction, we can harness the motion of the electrons to create a potential. Electrochemistry revolves around the separation of the two half-reactions in a redox reaction and establishing two different electrodes. This might involve physically separating the half-reactions or including a separator, such as a semi-permeable membrane or plastic dividers. With the reactions separated, the electrons will need to flow through the wire connecting...
need help for half cell potentials pls calculate step by step
(NOTE - Remember that the positive electrode is attached to the red wire and the negative electrode is attached to the black wire.) Electrode Systems Used Anode (oxidation) Negative Cathode (reduction) Positive Measured Potential (V) Positive (Ecu) Copper and silver Cu() - Cu2+ + 2e" Ag+ +1e Ag) 0.432 V Zinc + Silver Zn cs + 2n**+ Zé dat + leº nAg (s) 1.484 V Copper & Zinc Zn(s)...
need help with the rest of the table
EXPERIMENT 10 DETERMINATION OF THE ELECTROCHEMICAL SERIES PURPOSE To determine the standard cell potential values of several electrochemical coll INTRODUCTION The basis for an electrochemical cell is an oxidation reduction Corredor be divided into two half reactions reaction. This reaction can Oxidation half reaction Gloss of electrons) takes place at the anode, which is the positive electrode that the anions migrate to Chence the name anode) Reduction half reaction (gain of electrons)...
I need help with questione 1-12 and discussion question 1 and
2. The previous pictures help determine the chart. Please Show Work
thank you so much
An oxidation half-reaction is characterized by electrons appearing on the product side. The oxidation of aluminum for instance would be represented thusly: Al(s) → Al3+ + 3e- (1) An reduction half-reaction is characterized by electrons appearing on the reactant side. The reduction of ferrous iron for instance would be represented thusly: Fe2+ + 2e...
Using the table below:
19. Three combinations of metals are listed below, which
combination would produce the largest voltage if they were used to
construct an electrochemical cell?
Copper (Cu) with zinc (Zn)
Lead (Pb) with zinc (Zn)
Lead (Pb) with cadmium (Cd)
Liu lur the reaction between Zn and Cu2+ ions is 1.1030 V, we can use the known value for the half-cell potential for zinc to determine the half-cell potential for copper: Zn(s) → Zn2+(aq) + 2e +...
For electrochemistry cell, the reduction of silver ions is helped b the oxidation of zinc. Given the standard reduction half reactions, what is the standard potential of the cell? Ag* + e + Ag Ered= 0.799 V Zn²+ + 2e → Zn Ered = 0.763 V
Using the information in the table:
Which combination of metals, if used to create an
electrochemical cell, would produce the largest voltage?
Liu lur the reaction between Zn and Cu2+ ions is 1.1030 V, we can use the known value for the half-cell potential for zinc to determine the half-cell potential for copper: Zn(s) → Zn2+(aq) + 2e + Cu2+(aq) + 2e → Cu(s) Zn(s) + Cu2+ (aq) → Zn2+ (aq) + Cu(s) E half-cell = 0.7628 V Eºhalf-cell =...
how
would you go about solving this problem via using equations
just looking for the equation order i should go about solving this
problem
In this experiment you will be using the two half reactions Cu?"/Cu and Zn2 /Zn. The standard electrode potential, E°, for these half reactions is +0.34V and-0.76V respectively, so the Nernst Equation for these half reactions is the following Cu ea)+2e - Cus) E - 0.34V 0.0592V Cu2+] 0.0592V Zn 2 Note that solids by definition...
i need help with all of these questions
Chem 103A Electrochemistry 5. A voltaic cell is to be constructed using the Ag/Ag half cell and the Pb/Pb half-cell. Measurement shows that the silver electrode is positive. a) Write balanced half-reactions and the overall spontancous reaction, without using a table of half-cell potentials. b) Diagram the cell, labeling electrodes as anode and cathode, labeling the salt bridge, showing what ions are in solution, and showing the direction of electron flow in...
My percent error is high so before I keep going I wanted to
make sure I am doing this right. Can someone check this over and
make sure everything is right?
Ered (V) Half-reaction F(g)+2e2F" (aq) Cl,(g)+2e2C (aq) Ag (aq)+leAg(s) Fe (aq)+le Fe (aq) Cu (aq)+2e-> Cu(s) 2H (aq)+2eH, (g) Ni (aq)+2eNi(s) Cd (aq)+2eCd(s) Fe (aq)+2e Fe(s) Zn2 (aq)+2e-> Zn(s) 2.87 1.36 0.80 0.77 0.34 0.00 0.28 -0.40 -0.44 -0.76 Mg (aq)+2e- Mg(s) -2.37 Table 1. Standard Reduction Potential for...
Chem 1212 Lab Report on electrochemistry
Electrochemistry When electrons transfer between reaction components in a redox reaction, we can harness the motion of the electrons to create a potential. Electrochemistry revolves around the separation of the two half-reactions in a redox reaction and establishing two different electrodes. This might involve physically separating the half-reactions or including a separator, such as a semi-permeable membrane or plastic dividers. With the reactions separated, the electrons will need to flow through the wire connecting...
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