I really apologise for posting the same Q please consider this one as I really need it please help me. However, the first image is the one that I did not understand how to do and I really need, and the second one is that what I already have done. so please do the first image like the second that I have done, I mean in the same way but different topic 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 2: Electrolysis of Lead Bromide (PbBr,)White, solid lead (I) bromide is heated until it becomes molten, thus allowing ions toseparate and electricity to flow through it. Once molten, two carbon electrodes,which are attached to a 12V power supply, are placed in the clear and colourlessmolten liquid. Around the electrode connected to the positive terminal, orange/brownsolution is formed At the electrode connected to the negative terminal, a grey solidformed.Electrical energyElectrode:Electrode:Graphite/CarbonGraphite/CarbonSolution:PbBr,2 (aq)Half equations and overall equation:Species Oxidised:Species Reduced:Explain chemistry involved in electrolytic 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

I really apologise for posting the same Q please consider this one as I really need it please help me. However, the first image is the one that I did not understand how to do and I  really need, and the second one is that what I already have done. so please do the first image like the second that I have done, I mean in the same way but different topic 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 2: Electrolysis of Lead Bromide (PbBr,)White, solid lead (I) bromide is heated until it becomes molten, thus allowing ions toseparate and electricity to flow through it. Once molten, two carbon electrodes,which are attached to a 12V power supply, are placed in the clear and colourlessmolten liquid. Around the electrode connected to the positive terminal, orange/brownsolution is formed At the electrode connected to the negative terminal, a grey solidformed.Electrical energyElectrode:Electrode:Graphite/CarbonGraphite/CarbonSolution:PbBr,2 (aq)Half equations and overall equation:Species Oxidised:Species Reduced:Explain chemistry involved in electrolytic 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

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Solution:
We know in electrochemistry there are two type of cell. Electrolytic cell and galvanic…