Hi there, I really need this chemistry homework to be answered please help me with that I will be really appreciated it. However, I have already done one of them and need this one but I don't know how to do this. Please by looking at my work on the first image complete the second image. I very much need this please help me. Electrochemical Cell ReactionsExplain why the following reactions occur by using both the electron transfer methodand the oxidation number method.The following half cells are prepared in 100mL beakers, connected by a multimeterand salt bridge. (Your teacher may demonstrate the electrochemical cells).1. Zn a / Zna - a zinc electrode placed in 50mL of 1.0 moll" zinc nitrate solutionCu* en)/ Cua – a copper electrode placed in 50mL of 1.0 moll" copper nitratesolutionObservationsThe silver zinc metal starts to lose mass, the colourlesssolution remains. A red/brown metal forms on the copperelectrode, causing the electrode to gain mass. The bluesolution starts to fade until it turns colourless.Half EquationsCu (aq) + 2e Cu (s) Zn (s) Zn*" (aq) + 2eOverall EquationZn (s) + Cu* (aq) Zn" (aq) + Cu (s)Species oxidisedZnSpeciesreducedCu*ReactionExplained(usingelectrontransfer andoxidationAt the cathode, the copper electrode increases in mass ascopper ions are reduced to produce copper metal. The bluesolution will fade till it is colourless as the blue copper ionconcentration decreases as copper is formed by reduction. Theoxidation number of copper decreases from +2 in Cu* to 0 inCu indicating reduction. The blue copper ions also gain twoelectrons forming red-brown copper metal which shows this is areduction reaction as a gain of electrons indicates reduction.Cu" (aq) + 2e Cu (s)numbers)At the anode, the zinc electrode decreases in mass as zincis oxidised to produce colourless zinc ions. The solutionremains colourless as the zinc ion concentration increases.The zinc is oxidised as the oxidation number of zinc increasesfrom 0 in Zn to +2 in Zn". Silver zinc also loses two electronsforming colourless zinc ions which shows this is an oxidationreaction as a loss of electrons indicates oxidation.Zn (s) Zn" (aq) + 2eThis results in the overall equation:Zn (s) + Cu?" (aq) Zn" (aq) + Cu (s) Task 1: Electrochemical cell (Galvanic Cell) – Lead nitrate/Lead andIron(II) nitrate/IronA dark grey electrode made of lead metal is put into a beaker with a colourlesssolution of 1.0mol/L Lead (II) nitrate. In a separate beaker, another grey electrodemade from iron metal is put into a solution of 1.0 mol/L iron (II) nitrate. The twoelectrodes are connected with a wire and the two solutions are connected with a saltbridge made from filter paper soaked in KNO, solution. Over time, the mass of thelead electrode increases but the mass of the iron electrode decreases. The verypale green iron (II) nitrate solution becomes slightly darker green, while the leadnitrate solution remains colourless.VElectrode: PbElectrodFeKNO,SolutianPb(NO,Fe(NO,3)23)2Half equations and overall equation:Species Oxidised:Species Reduced:Explain chemistry involved in electrochemical cell using electron transfer andoxidation numbers. In your discussion you must:• Link the observations made at each electrode to the species involved.• Link half equations for the reaction occurring at the anode and cathode andidentify these as either oxidation or reduction.• Use standard reduction potentials to calculate the cell potential and predictspontaneity.• Link the spontaneity to the relative strengths of the oxidant/ reductant

Question

Hi there, I really need this chemistry homework to be answered please help me with that I will be really appreciated it. However, I have already done one of them and need this one but I don't know how to do this. Please by looking at my work on the first image complete the second image. I very much need this please help me. Electrochemical Cell ReactionsExplain why the following reactions occur by using both the electron transfer methodand the oxidation number method.The following half cells are prepared in 100mL beakers, connected by a multimeterand salt bridge. (Your teacher may demonstrate the electrochemical cells).1. Zn a / Zna - a zinc electrode placed in 50mL of 1.0 moll&#34; zinc nitrate solutionCu* en)/ Cua – a copper electrode placed in 50mL of 1.0 moll&#34; copper nitratesolutionObservationsThe silver zinc metal starts to lose mass, the colourlesssolution remains. A red/brown metal forms on the copperelectrode, causing the electrode to gain mass. The bluesolution starts to fade until it turns colourless.Half EquationsCu (aq) + 2e Cu (s) Zn (s) Zn*&#34; (aq) + 2eOverall EquationZn (s) + Cu* (aq) Zn&#34; (aq) + Cu (s)Species oxidisedZnSpeciesreducedCu*ReactionExplained(usingelectrontransfer andoxidationAt the cathode, the copper electrode increases in mass ascopper ions are reduced to produce copper metal. The bluesolution will fade till it is colourless as the blue copper ionconcentration decreases as copper is formed by reduction. Theoxidation number of copper decreases from +2 in Cu* to 0 inCu indicating reduction. The blue copper ions also gain twoelectrons forming red-brown copper metal which shows this is areduction reaction as a gain of electrons indicates reduction.Cu&#34; (aq) + 2e Cu (s)numbers)At the anode, the zinc electrode decreases in mass as zincis oxidised to produce colourless zinc ions. The solutionremains colourless as the zinc ion concentration increases.The zinc is oxidised as the oxidation number of zinc increasesfrom 0 in Zn to +2 in Zn&#34;. Silver zinc also loses two electronsforming colourless zinc ions which shows this is an oxidationreaction as a loss of electrons indicates oxidation.Zn (s) Zn&#34; (aq) + 2eThis results in the overall equation:Zn (s) + Cu?&#34; (aq) Zn&#34; (aq) + Cu (s) Task 1: Electrochemical cell (Galvanic Cell) – Lead nitrate/Lead andIron(II) nitrate/IronA dark grey electrode made of lead metal is put into a beaker with a colourlesssolution of 1.0mol/L Lead (II) nitrate. In a separate beaker, another grey electrodemade from iron metal is put into a solution of 1.0 mol/L iron (II) nitrate. The twoelectrodes are connected with a wire and the two solutions are connected with a saltbridge made from filter paper soaked in KNO, solution. Over time, the mass of thelead electrode increases but the mass of the iron electrode decreases. The verypale green iron (II) nitrate solution becomes slightly darker green, while the leadnitrate solution remains colourless.VElectrode: PbElectrodFeKNO,SolutianPb(NO,Fe(NO,3)23)2Half equations and overall equation:Species Oxidised:Species Reduced:Explain chemistry involved in electrochemical cell using electron transfer andoxidation numbers. In your discussion you must:• Link the observations made at each electrode to the species involved.• Link half equations for the reaction occurring at the anode and cathode andidentify these as either oxidation or reduction.• Use standard reduction potentials to calculate the cell potential and predictspontaneity.• Link the spontaneity to the relative strengths of the oxidant/ reductant

Accepted Answer

Given:
Electrochemical cell
Lead nitrate/Lead and Iron nitrate/ Iron