![2. Answer each of the following: (i) Explain using VSEPRT the difference in geometries of CH4 and H20. [4 Marks] (ii) Discuss](http://img.homeworklib.com/questions/dd3608c0-fd7b-11ea-ab91-f5bd6f7a0cfa.png?x-oss-process=image/resize,w_560)
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2. Answer each of the following: (i) Explain using VSEPRT the difference in geometries of CH4...
Help with Part C please? Not sure if I have the correct information to determine an answer
Help with Part C please? Not sure if I have the correct
information to determine an answer
Problems 1. Given the standard reduction potentials Cd(OH)2(s) +2e → Cd(s) + 2 OH-(aq) В"--0.76 V Ni0(OH)(s) + H20() + r-, Ni(OH)2(s) + OH-(aq) E。_ +0.49 V Write the reactions for the discharge and charge of a nickel-cadmium rechargeable battery. a. b. Calculate the standard potential of this battery. A typical nicad battery has a potential of 1.30 V. Why is there a...
The following half-reactions occur during use of the rechargeable nickel-cadmium battery: Ca(OH)2(s) + 2e → Cd(s)...
The following half-reactions occur during use of the rechargeable nickel-cadmium battery: Ca(OH)2(s) + 2e → Cd(s) + 20H(aq) NiO(OH)(s) + H20(1) + e- → Ni(OH)2(s) + OH(aq) This battery has a potential of 1.35 V under standard conditions, with nickel as the cathode. What potential does this battery produce if its hydroxide ion concentration is 1.97 x 10-2 M? E = V the tolerance is +/-2%
5. The nickel-cadmium battery, despite issues with the toxicity of Cd, is still used in some...
5. The nickel-cadmium battery, despite issues with the toxicity of Cd, is still used in some rechargeable batteries because it has very consistent voltage over long discharge times. a) Using only half-cell reactions given in Table 16.1, write the overall reaction and give the highest AV° value possible for a NiCd battery. b) The actual half-cell reactions used in a Nicd battery are: Ca(OH)2(8) + 2e → Cds + 2OH(aq) (Vº = -0.86V) NiO(OH)) + H2O) +e Ni(OH)2(s) + OH(aq)...
Question 2. [10 Marks] Given the following half-cell reduction potentials: Ni2+ (aq) + 2e-F Ni(s), Ered...
Question 2. [10 Marks] Given the following half-cell reduction potentials: Ni2+ (aq) + 2e-F Ni(s), Ered = -0.23 V Pt2+ (aq) + 2e-E Pt(s), Ered = +1.2 V Pd2+(aq) + 2e- EPd(s), Ered = 0.99 V a) Sketch the cell for which the overall cell potential is the greatest. [3 Marks) b) Identify the cathode and anode, and then show the direction of electron flow for the cell in the circuit (a). [3 Marks] c) Will Pt(s) reduce Pd2+(aq)? Explain...
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 +...
please I need answers to all these questions! Name 3 HW Electrochemistry Submit before Nov 20,...
please I need answers to all these questions!
Name 3 HW Electrochemistry Submit before Nov 20, 2019 at 12 PM D2L Submission: Submit one file containing all calculations and the original paper Assessments Assign ments HW Electrochemistry 1) Which two of the following half-reactions will combine to give the galvanic cell with the highest cell potential? Reduction Half-Reaction E (V) Metal Al3+ 3e- Al(s) Aluminum -1.66 Mn + 2e Mn(s) - 1.18 Manganese Zn 2e Zinc Zn(s) -0.76 Cr3 Зе-...
Name: Chem 1120 Electrochemical Potentials Perform each of the following calculations, showing all work. Use the...
Name: Chem 1120 Electrochemical Potentials Perform each of the following calculations, showing all work. Use the Electrochemical Potentials table provided on D2L if values are not provided. Standard State Electrochemical Cells 1. In each of the following systems two half-reactions are provided. For each system, a) write the balanced reaction occurring for a spontaneous system, and b) calculate the overall standard cell potential. a. Half Reaction Zn2+(aq) + 2e = Zn(s) Cr3+ (aq) + 38 = Cr(s) Eºred (V) -0.76...
I need the answers for page 2 and three do not pay attention to the first...
I
need the answers for page 2 and three do not pay attention to the
first page!
EXPERIMENT 10: DETERMINATION OF THE ELECTROCHEMICAL SERIES QUESTIONS Which metal was not oxidized by any of the other half-cells? 1. Using Table 1, what are two metal half-cells that would oxidize the metal from question #1? 2 3. Which metal was oxidized by all of the other half-cells? 4. Using Table 1, what are two metal half-cells that the metal from question #3...
Candidate l: Zn(s) | Zn2+(aq,0.500 M) I Cu2+(aq, 1.00 M) Cu(s) Candidate 2: Pb(s) | Pb2+(aq,...
Candidate l: Zn(s) | Zn2+(aq,0.500 M) I Cu2+(aq, 1.00 M) Cu(s) Candidate 2: Pb(s) | Pb2+(aq, 0.500 M) || Cu2+(aq, 1.00 M) Cu(s) Candidate 3: Mg(s) | Mg2+(aq, 0.500 M) | Pb2+(aq, 1.00 M)| Pb(s) (a) 6 pts) Choose one of the candidate voltaic cells #1, #2, or #3. Draw a schematic cell diagram for the candidate voltaic cell of choice. Clearly label anode, cathode, electrodes, ions and their concentrations, salt bridge, and the flow of electrons. (b) (5 pts)...
Use the galvanic cell notation to describe the Daniell cell. (4 marks) Using the reduction potential...
Use the galvanic cell notation to describe the Daniell cell. (4 marks) Using the reduction potential table calculate Eº for the Daniel cell. 12 marks) Calculate the equilibrium constant K for the reaction Cu2+ + Zn → Cu + Zn²+, at 25 °C. (4 marks) Standard Potentials at 25°C Half Reaction Potential Potential +2.87 V 0.000 V +2.07 V -0.04 V +2.05 V -0.13 V -1.69 V -0.14 V +1.69 V -0.23 V +1.67 V -0.26 V +1.63 v -0.28...
Help with Part C please? Not sure if I have the correct
information to determine an answer
Problems 1. Given the standard reduction potentials Cd(OH)2(s) +2e → Cd(s) + 2 OH-(aq) В"--0.76 V Ni0(OH)(s) + H20() + r-, Ni(OH)2(s) + OH-(aq) E。_ +0.49 V Write the reactions for the discharge and charge of a nickel-cadmium rechargeable battery. a. b. Calculate the standard potential of this battery. A typical nicad battery has a potential of 1.30 V. Why is there a...
The following half-reactions occur during use of the rechargeable nickel-cadmium battery: Ca(OH)2(s) + 2e → Cd(s) + 20H(aq) NiO(OH)(s) + H20(1) + e- → Ni(OH)2(s) + OH(aq) This battery has a potential of 1.35 V under standard conditions, with nickel as the cathode. What potential does this battery produce if its hydroxide ion concentration is 1.97 x 10-2 M? E = V the tolerance is +/-2%
5. The nickel-cadmium battery, despite issues with the toxicity of Cd, is still used in some rechargeable batteries because it has very consistent voltage over long discharge times. a) Using only half-cell reactions given in Table 16.1, write the overall reaction and give the highest AV° value possible for a NiCd battery. b) The actual half-cell reactions used in a Nicd battery are: Ca(OH)2(8) + 2e → Cds + 2OH(aq) (Vº = -0.86V) NiO(OH)) + H2O) +e Ni(OH)2(s) + OH(aq)...
Question 2. [10 Marks] Given the following half-cell reduction potentials: Ni2+ (aq) + 2e-F Ni(s), Ered = -0.23 V Pt2+ (aq) + 2e-E Pt(s), Ered = +1.2 V Pd2+(aq) + 2e- EPd(s), Ered = 0.99 V a) Sketch the cell for which the overall cell potential is the greatest. [3 Marks) b) Identify the cathode and anode, and then show the direction of electron flow for the cell in the circuit (a). [3 Marks] c) Will Pt(s) reduce Pd2+(aq)? Explain...
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 +...
please I need answers to all these questions!
Name 3 HW Electrochemistry Submit before Nov 20, 2019 at 12 PM D2L Submission: Submit one file containing all calculations and the original paper Assessments Assign ments HW Electrochemistry 1) Which two of the following half-reactions will combine to give the galvanic cell with the highest cell potential? Reduction Half-Reaction E (V) Metal Al3+ 3e- Al(s) Aluminum -1.66 Mn + 2e Mn(s) - 1.18 Manganese Zn 2e Zinc Zn(s) -0.76 Cr3 Зе-...
Name: Chem 1120 Electrochemical Potentials Perform each of the following calculations, showing all work. Use the Electrochemical Potentials table provided on D2L if values are not provided. Standard State Electrochemical Cells 1. In each of the following systems two half-reactions are provided. For each system, a) write the balanced reaction occurring for a spontaneous system, and b) calculate the overall standard cell potential. a. Half Reaction Zn2+(aq) + 2e = Zn(s) Cr3+ (aq) + 38 = Cr(s) Eºred (V) -0.76...
I
need the answers for page 2 and three do not pay attention to the
first page!
EXPERIMENT 10: DETERMINATION OF THE ELECTROCHEMICAL SERIES QUESTIONS Which metal was not oxidized by any of the other half-cells? 1. Using Table 1, what are two metal half-cells that would oxidize the metal from question #1? 2 3. Which metal was oxidized by all of the other half-cells? 4. Using Table 1, what are two metal half-cells that the metal from question #3...
Candidate l: Zn(s) | Zn2+(aq,0.500 M) I Cu2+(aq, 1.00 M) Cu(s) Candidate 2: Pb(s) | Pb2+(aq, 0.500 M) || Cu2+(aq, 1.00 M) Cu(s) Candidate 3: Mg(s) | Mg2+(aq, 0.500 M) | Pb2+(aq, 1.00 M)| Pb(s) (a) 6 pts) Choose one of the candidate voltaic cells #1, #2, or #3. Draw a schematic cell diagram for the candidate voltaic cell of choice. Clearly label anode, cathode, electrodes, ions and their concentrations, salt bridge, and the flow of electrons. (b) (5 pts)...
Use the galvanic cell notation to describe the Daniell cell. (4 marks) Using the reduction potential table calculate Eº for the Daniel cell. 12 marks) Calculate the equilibrium constant K for the reaction Cu2+ + Zn → Cu + Zn²+, at 25 °C. (4 marks) Standard Potentials at 25°C Half Reaction Potential Potential +2.87 V 0.000 V +2.07 V -0.04 V +2.05 V -0.13 V -1.69 V -0.14 V +1.69 V -0.23 V +1.67 V -0.26 V +1.63 v -0.28...
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