Copper is purified by electrolysis. A 4.00−kg anode is used in a cell in which the...
Copper is purified by electrolysis. A 4.00−kg anode is used in a cell in which the current is 37.8 A. How long (in hours) must the current run to dissolve this anode and electroplate it onto the cathode?
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Copper is purified by electrolysis. A 4.00−kg anode is used in a
cell in which the...
Enter your answer in the provided box. Copper is purified by electrolysis. A 1.46 kg anode...
Enter your answer in the provided box. Copper is purified by electrolysis. A 1.46 kg anode is used in a cell in which the current is 37.8 A. How long in hours) must the current run to dissolve this anode and electroplate it onto the cathode? h
Electrolysis is often used to electroplate metal objects. Sketch an electrolysis cell used to sil...
Electrolysis is often used to electroplate metal objects. Sketch an electrolysis cell used to silver plate a metal spoon in an aqueous solution of silver cyanide, Ag(CN2. Label anode, cathode, direction of electron flow, and write the cathode half-reaction. Calculate the time required to plate 0.100 g of silver on a metal spoon using a current of 500 mA. (3 marks)
Electrolysis is often used to electroplate metal objects. Sketch an electrolysis cell used to silver plate a metal spoon...
solve for part a and b Consider an electrolysis cell that might be used to electroplate...
solve for part a and b
Consider an electrolysis cell that might be used to electroplate copper onto other metal surfaces. Label the anode and the cathode. Drag the appropriate labels to their respective targets. Show the reactions that occur at each. Express your answers as chemical equations separated by a comma. Identify all of the phases in your answer.
Fill the table with the raw data collected from your copper electrolysis Run # Initial Anode...
Fill the table with the raw data collected from your copper electrolysis Run # Initial Anode Mass (g) Final Anode Mass (g) Initial Cathode Mass (g) Final Cathode Mass (g) Current (A) Time (min) Time (s) 1 11.5 11.005 10.5 10.995 5.00 Amps 5:00 300 2 11.5 10.762 10.5 11.238 2.50 A 15:00 900 3 11.5 10.906 10.5 11.094 1.00 A 30:00 1800 Calculate the experimental mass loss at the anode and the experimental mass gain at the cathode for...
The Purification of copper can be achieved by electrorefining copper from an impure copper anode onto...
The Purification of copper can be achieved by electrorefining copper from an impure copper anode onto a pure copper cathode in an electrolytic cell. How many hours will it take to plate 16.5 kg of copper onto the cathode if the current passed through the cell is held constant at 35.0 amperes? Assume the copper in the electrolytic solution is present as Cu2+. (Faraday’s Constant = 96500 Coulombs/mol e–).
Part 2: Copper Electrolysis 1. Fill the table with the raw data collected from your copper...
Part 2: Copper Electrolysis 1. Fill the table with the raw data collected from your copper electrolysis Run # Time Initial Anode Mass (g) Final Anode Mass (g) 11.005 Initial Cathode Mass (9) 10.5 Final Cathode Mass (g) 10.995 Current (A) Time (min) 5:00 300 11.5 11.5 5.00 Amps 2.50 A 2 10.762 10.5 11.238 15:00 900 دیا 10.906 10.5 11.094 1.00 A 30:00 1800 11.5 1 2. Calculate the experimental mass loss at the anode and the experimental mass...
2. For each of the following cell notations: a. Identify the cathode and anode. b. Write...
2. For each of the following cell notations: a. Identify the cathode and anode. b. Write the net cell equation. c. Calculate the cell potential. I) Pb(e) 1 Pb2+(ag) 11 Ni2+ (aq) 1 Ni(s) II) Pts 1 So,"caq) H(aq) 1 H2SO3(aq) 11 Ag‘aq) 1 Ago) 4. Balance the following redox reaction occurring in a basic medium. NO2 (aq) + Al(s) + NH3(g) + AlO2 (aq) 5. A student wishes to set up an electrolytic cell to plate copper onto a...
a. For the electrolysis of molten BaCl2, diagram a cell. Include the direction in which a...
a. For the electrolysis of molten BaCl2, diagram a cell. Include the direction in which a battery would be placed to power the cell. Write out half-reactions. Label flow of electrons, anode, cathode, indicate what is formed at each electrode (assume electrodes are generic metal). Could this reaction be carried out in aqueous solution? Why or why not (justify numerically). b. 0.67 g of Ag is deposited electrolytically from AgNO3after a certain period of time when subjected to a 12A...
Copper can be electroplated at the cathode of an electrolysis cell by the half reaction. How...
Copper can be electroplated at the cathode of an electrolysis cell by the half reaction. How much time (in min) would it take for 313mg of copper to be plated at a current of 5.6A (1A=1C/s)? Cu^2+(aq) + 2e ---->Cu(s)
A galvanic cell consists of a manganese anode immersed in a MnSO4 solution and a copper cathode i...
A galvanic cell consists of a manganese anode immersed in a MnSO4 solution and a copper cathode immersed in a CuSo4 solution. A salt bridge connects the two half-cells (a) Write a balanced equation for the cell reaction. (b) A current of 1.34 A is observed to flow for a period of 1.99 hours. How much charge passes through the circuit during this time? How many moles of electrons is this charge equivalent to? mol (c) Calculate the change in...
Enter your answer in the provided box. Copper is purified by electrolysis. A 1.46 kg anode is used in a cell in which the current is 37.8 A. How long in hours) must the current run to dissolve this anode and electroplate it onto the cathode? h
Electrolysis is often used to electroplate metal objects. Sketch an electrolysis cell used to silver plate a metal spoon in an aqueous solution of silver cyanide, Ag(CN2. Label anode, cathode, direction of electron flow, and write the cathode half-reaction. Calculate the time required to plate 0.100 g of silver on a metal spoon using a current of 500 mA. (3 marks)
Electrolysis is often used to electroplate metal objects. Sketch an electrolysis cell used to silver plate a metal spoon...
solve for part a and b
Consider an electrolysis cell that might be used to electroplate copper onto other metal surfaces. Label the anode and the cathode. Drag the appropriate labels to their respective targets. Show the reactions that occur at each. Express your answers as chemical equations separated by a comma. Identify all of the phases in your answer.
Part 2: Copper Electrolysis 1. Fill the table with the raw data collected from your copper electrolysis Run # Time Initial Anode Mass (g) Final Anode Mass (g) 11.005 Initial Cathode Mass (9) 10.5 Final Cathode Mass (g) 10.995 Current (A) Time (min) 5:00 300 11.5 11.5 5.00 Amps 2.50 A 2 10.762 10.5 11.238 15:00 900 دیا 10.906 10.5 11.094 1.00 A 30:00 1800 11.5 1 2. Calculate the experimental mass loss at the anode and the experimental mass...
2. For each of the following cell notations: a. Identify the cathode and anode. b. Write the net cell equation. c. Calculate the cell potential. I) Pb(e) 1 Pb2+(ag) 11 Ni2+ (aq) 1 Ni(s) II) Pts 1 So,"caq) H(aq) 1 H2SO3(aq) 11 Ag‘aq) 1 Ago) 4. Balance the following redox reaction occurring in a basic medium. NO2 (aq) + Al(s) + NH3(g) + AlO2 (aq) 5. A student wishes to set up an electrolytic cell to plate copper onto a...
A galvanic cell consists of a manganese anode immersed in a MnSO4 solution and a copper cathode immersed in a CuSo4 solution. A salt bridge connects the two half-cells (a) Write a balanced equation for the cell reaction. (b) A current of 1.34 A is observed to flow for a period of 1.99 hours. How much charge passes through the circuit during this time? How many moles of electrons is this charge equivalent to? mol (c) Calculate the change in...
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