Homework Answers
Ans. Cu(NO3)2 + Zn = Cu(s) + Zn(NO3)2
The element Copper, Cu is being reduced from +2 to +0.
The element Zn gets oxidized from +0 to +2.
This cell is known as Galvanic cell in which Zn metal gets dissoved and form Zn2+ from Zn electrode and Cu2+ gets deposited to Cathode as Cu. and form electrochemical cell and produce electricity.
Oxidation takes place in anode and reduction take place in cathode.
Anode reaction:- Zn(s) = Zn2+ + 2e
Cathode reaction:- Cu2+ + 2e = Cu(s)
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Electrochemical (or voltaic) cell notes AP chemistry Write the re Identify the elements being oxidized and...
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...
Calculate the theoretical cell potential (E°) of a galvanic cell under standard conditions made up of...
Calculate the theoretical cell potential (E°) of a galvanic cell
under standard conditions made up of copper and magnesium (see Part
II and Table 1 for more information).
PARTIL Creating and Testing Voltaic Cells Introduction and Background for the Voltaic Cells A galvanic cell (sometimes more appropriately called a voltaic cell) consists of two half-cells joined by a salt bridge that allow ions to pass between the two sides in order to maintain electroneutrality. Each half-cell contains the Components of...
Magnesium metal is oxidized and silver ions are reduced in a voltaic cell using: Mg(s) |...
Magnesium metal is oxidized and silver ions are reduced in a voltaic cell using: Mg(s) | Mg2+ (aq, 1M) || Ag+ (aq, 1M) | Ag(s) a. Draw the voltaic cell. Label each part of the cell. b. Write the equations for the half-reactions occurring at the anode and cathode. c. Write the overall reaction for the cell. d. Draw arrows to show the movement of electrons in the external circuit. Assuming the salt bridge contains NaNO3, indicate the movement of...
3. Write the electrochemical half-cell reactions for oxidation and reduction during uniform corrosion in the following:...
3. Write the electrochemical half-cell reactions for oxidation and reduction during uniform corrosion in the following: (Also indicate if corrosion is possible) a. Corrosion of Aluminum in air free sulfuric acid (i.e., No oxygen in the solution) b. Iron in air free acid ferric sulfate solution (assume no O2 in the solution) Hint Fe3+ to Fe reaction is possible due to the presence of the ferric ions c. Carbon steel in aerated seawater (With O2 in the solution) d. Zinc...
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)...
Voltaic cells chemistry please help with A-C, H and I. 3. A voltaic cell is built...
Voltaic cells chemistry
please help with A-C, H and I.
3. A voltaic cell is built from two half-cells using the reduction reactions given below: Sn 2(aq) → Sn(s); Eredn = -0.14 V Cr20;2(aq) → Cr+ (aq) Eredin = 1.33 V a) Write the balanced cathode half reaction in acidic medium: (show work step by step and box your answer) b) Write the balanced anode half reaction and box your answer: c) Write the balanced overall cell reaction and box...
How would I do the follow equation? What are the steps? Identify and write the (unbalanced)...
How would I do the follow equation? What are the steps? Identify and write the (unbalanced) oxidation and reduction half-reactions for the following reactions. (a) Solid copper dissolves in an acidic solution containing nitrate ions to form copper (II) ions and nitrogen dioxide gas. (b) Solid zinc dissolves in hydrochloric acid to form zinc ions (+2 charge) in solution and hydrogen gas. (c) Solid iron (III) oxide reacts with solid carbon to produce solid iron and and gaseous carbon dioxide.
Parts a-j of this question refer to the following cell at 298 K. Complete the diagram...
Parts a-j of this question refer to the following cell at 298 K. Complete the diagram of the following voltaic cell: Zinc and iron electrodes, aqueous zinc nitrate, aqueous iron (III) nitrate, potassium nitrate salt bridge. Fe3+ (aq) + 3e- → Fe (s) E°= -0.040 V Ag+(aq) + e- → Ag(s) E°= 0.795 V a. Identify the electrodes as Anode or Cathode. Write the correct metal for each assuming the reactions are spontaneous b. Show the direction of the electron...
please show all work. thank you 4. Consider an electrochemical cell (a.k.a. galvanic cell or voltaic...
please show all work. thank you
4. Consider an electrochemical cell (a.k.a. galvanic cell or voltaic cell) with Ag(s) and 1.0 M AgNO3(aq) in one compartment and Cu(s) and 1.0 M Cu(NO3)2(aq) in the other compartment. Write the reactions and calculate the standard state cell potential at 298 K. E cathode = a. Reduction (cathode): Eanode = b. Oxidation (anode): Eºcell = C. Net (overall cell reaction): 5. Consider a galvanic cell with Sn(s) and 1.0 M Sn(NO3)2(aq) in one...
2. Consider the voltaic cell illustrated below, constructed by coupling a Ni/Ni half-cell with an Ag/Ag* half-cell a...
2. Consider the voltaic cell illustrated below, constructed by coupling a Ni/Ni half-cell with an Ag/Ag* half-cell and allowing them to react spontaneously. Refer to the table of reduction potentials and write the half-reaction that occurs at each electrode (nickel and silver). Then combine the half-reactions into the overall reaction. a. Calculate the standard cell potential. b. Annotate the diagram below. First, randomly label one electrode as Ag and one as Ni. Then identify which is the anode and which...
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...
Calculate the theoretical cell potential (E°) of a galvanic cell
under standard conditions made up of copper and magnesium (see Part
II and Table 1 for more information).
PARTIL Creating and Testing Voltaic Cells Introduction and Background for the Voltaic Cells A galvanic cell (sometimes more appropriately called a voltaic cell) consists of two half-cells joined by a salt bridge that allow ions to pass between the two sides in order to maintain electroneutrality. Each half-cell contains the Components of...
3. Write the electrochemical half-cell reactions for oxidation and reduction during uniform corrosion in the following: (Also indicate if corrosion is possible) a. Corrosion of Aluminum in air free sulfuric acid (i.e., No oxygen in the solution) b. Iron in air free acid ferric sulfate solution (assume no O2 in the solution) Hint Fe3+ to Fe reaction is possible due to the presence of the ferric ions c. Carbon steel in aerated seawater (With O2 in the solution) d. Zinc...
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)...
Voltaic cells chemistry
please help with A-C, H and I.
3. A voltaic cell is built from two half-cells using the reduction reactions given below: Sn 2(aq) → Sn(s); Eredn = -0.14 V Cr20;2(aq) → Cr+ (aq) Eredin = 1.33 V a) Write the balanced cathode half reaction in acidic medium: (show work step by step and box your answer) b) Write the balanced anode half reaction and box your answer: c) Write the balanced overall cell reaction and box...
please show all work. thank you
4. Consider an electrochemical cell (a.k.a. galvanic cell or voltaic cell) with Ag(s) and 1.0 M AgNO3(aq) in one compartment and Cu(s) and 1.0 M Cu(NO3)2(aq) in the other compartment. Write the reactions and calculate the standard state cell potential at 298 K. E cathode = a. Reduction (cathode): Eanode = b. Oxidation (anode): Eºcell = C. Net (overall cell reaction): 5. Consider a galvanic cell with Sn(s) and 1.0 M Sn(NO3)2(aq) in one...
2. Consider the voltaic cell illustrated below, constructed by coupling a Ni/Ni half-cell with an Ag/Ag* half-cell and allowing them to react spontaneously. Refer to the table of reduction potentials and write the half-reaction that occurs at each electrode (nickel and silver). Then combine the half-reactions into the overall reaction. a. Calculate the standard cell potential. b. Annotate the diagram below. First, randomly label one electrode as Ag and one as Ni. Then identify which is the anode and which...
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