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Task 1: Electrochemical cell (Galvanic Cell) – Lead nitrate/Lead and Iron(II) nitrate/lron A dark grey electrode made of lead metal is put into a beaker with a colourless solution of 1.0mol/L Lead (II) nitrate. In a separate beaker, another grey electrode made from iron metal is put into a solution of 1.0 mol/L iron (II) nitrate. The two electrodes are connected with a wire and the two solutions are connected with a salt

Task 1: Electrochemical cell (Galvanic Cell) – Lead nitrate/Lead and Iron(II) nitrate/lron A dark grey electrode made of lead metal is put into a beaker with a colourless solution of 1.0mol/L Lead (II) nitrate. In a separate beaker, another grey electrode made from iron metal is put into a solution of 1.0 mol/L iron (II) nitrate. The two electrodes are connected with a wire and the two solutions are connected with a salt

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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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 Reactions Explain why the following reactions occur by using both the electron transfer method and the oxidation number method. The following half cells are prepared in 100mL beakers, connected by a multimeter and 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 solution Cu* en)/ Cua – a copper electrode placed in 50mL of 1.0 moll" copper nitrate solution Observations The silver zinc metal starts to lose mass, the colourless solution remains. A red/brown metal forms on the copper electrode, causing the electrode to gain mass. The blue solution starts to fade until it turns colourless. Half Equations Cu (aq) + 2e Cu (s) Zn (s) Zn*" (aq) + 2e Overall Equation Zn (s) + Cu* (aq) Zn" (aq) + Cu (s) Species oxidised Zn Species reduced Cu* Reaction Explained (using electron transfer and oxidation At the cathode, the copper electrode increases in mass as copper ions are reduced to produce copper metal. The blue solution will fade till it is colourless as the blue copper ion concentration decreases as copper is formed by reduction. The oxidation number of copper decreases from +2 in Cu* to 0 in Cu indicating reduction. The blue copper ions also gain two electrons forming red-brown copper metal which shows this is a reduction reaction as a gain of electrons indicates reduction. Cu" (aq) + 2e Cu (s) numbers) At the anode, the zinc electrode decreases in mass as zinc is oxidised to produce colourless zinc ions. The solution remains colourless as the zinc ion concentration increases. The zinc is oxidised as the oxidation number of zinc increases from 0 in Zn to +2 in Zn". Silver zinc also loses two electrons forming colourless zinc ions which shows this is an oxidation reaction as a loss of electrons indicates oxidation. Zn (s) Zn" (aq) + 2e This results in the overall equation: Zn (s) + Cu?" (aq) Zn" (aq) + Cu (s)
Transcribed Image Text:Electrochemical Cell Reactions Explain why the following reactions occur by using both the electron transfer method and the oxidation number method. The following half cells are prepared in 100mL beakers, connected by a multimeter and 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 solution Cu* en)/ Cua – a copper electrode placed in 50mL of 1.0 moll" copper nitrate solution Observations The silver zinc metal starts to lose mass, the colourless solution remains. A red/brown metal forms on the copper electrode, causing the electrode to gain mass. The blue solution starts to fade until it turns colourless. Half Equations Cu (aq) + 2e Cu (s) Zn (s) Zn*" (aq) + 2e Overall Equation Zn (s) + Cu* (aq) Zn" (aq) + Cu (s) Species oxidised Zn Species reduced Cu* Reaction Explained (using electron transfer and oxidation At the cathode, the copper electrode increases in mass as copper ions are reduced to produce copper metal. The blue solution will fade till it is colourless as the blue copper ion concentration decreases as copper is formed by reduction. The oxidation number of copper decreases from +2 in Cu* to 0 in Cu indicating reduction. The blue copper ions also gain two electrons forming red-brown copper metal which shows this is a reduction reaction as a gain of electrons indicates reduction. Cu" (aq) + 2e Cu (s) numbers) At the anode, the zinc electrode decreases in mass as zinc is oxidised to produce colourless zinc ions. The solution remains colourless as the zinc ion concentration increases. The zinc is oxidised as the oxidation number of zinc increases from 0 in Zn to +2 in Zn". Silver zinc also loses two electrons forming colourless zinc ions which shows this is an oxidation reaction as a loss of electrons indicates oxidation. Zn (s) Zn" (aq) + 2e This results in the overall equation: Zn (s) + Cu?" (aq) Zn" (aq) + Cu (s)
Task 1: Electrochemical cell (Galvanic Cell) – Lead nitrate/Lead and Iron(II) nitrate/Iron A dark grey electrode made of lead metal is put into a beaker with a colourless solution of 1.0mol/L Lead (II) nitrate. In a separate beaker, another grey electrode made from iron metal is put into a solution of 1.0 mol/L iron (II) nitrate. The two electrodes are connected with a wire and the two solutions are connected with a salt bridge made from filter paper soaked in KNO, solution. Over time, the mass of the lead electrode increases but the mass of the iron electrode decreases. The very pale green iron (II) nitrate solution becomes slightly darker green, while the lead nitrate solution remains colourless. V Electrode: Pb Electrod Fe KNO, Solutian Pb(NO, Fe(NO, 3)2 3)2 Half equations and overall equation: Species Oxidised: Species Reduced: Explain chemistry involved in electrochemical cell using electron transfer and oxidation 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 and identify these as either oxidation or reduction. • Use standard reduction potentials to calculate the cell potential and predict spontaneity. • Link the spontaneity to the relative strengths of the oxidant/ reductant
Transcribed Image Text:Task 1: Electrochemical cell (Galvanic Cell) – Lead nitrate/Lead and Iron(II) nitrate/Iron A dark grey electrode made of lead metal is put into a beaker with a colourless solution of 1.0mol/L Lead (II) nitrate. In a separate beaker, another grey electrode made from iron metal is put into a solution of 1.0 mol/L iron (II) nitrate. The two electrodes are connected with a wire and the two solutions are connected with a salt bridge made from filter paper soaked in KNO, solution. Over time, the mass of the lead electrode increases but the mass of the iron electrode decreases. The very pale green iron (II) nitrate solution becomes slightly darker green, while the lead nitrate solution remains colourless. V Electrode: Pb Electrod Fe KNO, Solutian Pb(NO, Fe(NO, 3)2 3)2 Half equations and overall equation: Species Oxidised: Species Reduced: Explain chemistry involved in electrochemical cell using electron transfer and oxidation 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 and identify these as either oxidation or reduction. • Use standard reduction potentials to calculate the cell potential and predict spontaneity. • Link the spontaneity to the relative strengths of the oxidant/ reductant
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