Calculate the time required for a constant current of 0.758 A to deposit 0.300 g of...
Calculate the time required for a constant current of 0.758 A to deposit 0.300 g of Tl(III) as Tl(s) on a cathode.
Calculate the mass of Tl(I) that can be deposited as Tl2O3(s) on an anode at a constant current of 0.758 A over the same amount of time as calculated above.
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Calculate the time required for a constant current of 0.758 A to
deposit 0.300 g of...
1. Calculate the time required for a constant current of 0.817 A to deposit 0.390 g...
1. Calculate the time required for a constant current of 0.817 A to deposit 0.390 g of Tl(III) as Tl(s) on a cathode. 2. Calculate the mass of Tl(I) that can be deposited as Tl2O3(s) on an anode at a constant current of 0.817 A over the same amount of time as calculated above.
Question 33: A constant current of 0.156 A is applied over 319 s to deposit lead...
Question 33: A constant current of 0.156 A is applied over 319 s to deposit lead (from Pb2 in solution) at the cathode of an electrode. How many grams of lead are deposited, assuming no other redox reaction occurs. (Note: The atomic mass of lead is 207.2 g/mol and the Faraday constant is 96,485 C) 1.79 x 102g P 0.686 g Pb O5.34 x 102 g Pb 0.343 g Pb O 1.02 g Pb
1.Calculate time required to deposit 0.100 g of Thallium on a cathode when 100mA current is...
1.Calculate time required to deposit 0.100 g of Thallium on a cathode when 100mA current is passed through a 100Ml 0.01M Thallium solution. 2. A solution containing an unknown concentration of Cu2+ ions gives a diffusion current of 12.3 µA on a DC polarogram. Upon addition of 0.100 mL of 1.00 x 10-3 M Cu2+ solution to the 5ML of the Unknown, the new current is 28.2µA. Calculate the concentration of CU2+ in the unknown solution 3. Zinc is to...
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...
Initial mass of the anode was 10.00 g of Zinc and the initial mass of the...
Initial mass of the anode was 10.00 g of Zinc and the initial
mass of the cathode was 10.00g of iron. A simulation was done with
the current to 6.00 A and a 40.00 min time. (this information may
not be needed)
Part C: Electrolytic Cell and Calculation of Faraday's Constant (Using hits media.pearson me som/bc bemedia_chemchemummillest php) Cathode Final Mass 104.88 Cathode Initial Mass 16.00 4.88 Difference (m) g What do you notice in comparison to the change at...
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...
Part B and D Please show all of the steps. Learning Goal: To relate current, time,...
Part B and D
Please show all of the steps.
Learning Goal: To relate current, time, charge, and mass for electroplating calculations. Electroplating is a form of electrolysis in which a metal is deposited on the surface of another metal. To quantify electrolysis, use the following relationships. Electric current is measured in amperes (A), which expresses the amount of charge, in coulombs (C), that flows per second (s): 1 A 1 C/s Another unit of charge is the faraday (F),...
i cant get B for some reason!!! if you can help that would be great !!!!...
i cant get B for some reason!!! if you can help that would be
great !!!!
2 attempts left Check my work Be sure to answer all parts. When an aqueous solution containing gold (III) salt is electrolyzed, metallic gold is deposited at the cathode, and oxygen gas is generated at the anode. (a) If 8.61 g of Au is deposited at the cathode, calculate the volume of Oz generated at 23°C and 749 mmHg. 0.809 (b) What is the...
Standard free energy change (Delta degree G) and cell potential (E degree) can be said to...
Standard free energy change (Delta degree G) and cell potential (E degree) can be said to measure the same thing and are convertible by the equation: Delta G degree = nF E degree _cell where n is the total number of moles of electrons being transferred, and F is Faraday constant 9.6- 1853415 times 10^C/mol. The free energy (Delta G degree) of a spontaneous reaction is always negative. For each of the electrochemical cells below, calculate the free energy of...
need help !! with questions 2,4,5,6 Initial Mass of Cathode electrode (Fe) Initial Mass of Anode...
need help !! with questions 2,4,5,6
Initial Mass of Cathode electrode (Fe) Initial Mass of Anode electrode (Zn) Final Mass of Cathode 10.0g 10, og 10,209 .2g Fe 3+ (aq)+32 z Fecs) Mass of Zinc deposited on cathode (g) Half reaction in Cathode Half reaction in Anode Zn(s) Eszn²+ (aq) + Ze Za(s) + 2 Fest (1) ► 2* (g) +2 Fe²+ (aq) Overall Cell Reaction Standard Cell Potential, Ecellº .440 +.763 3.32 3 (Eºcell = Ecathode - Eanode) Number...
Question 33: A constant current of 0.156 A is applied over 319 s to deposit lead (from Pb2 in solution) at the cathode of an electrode. How many grams of lead are deposited, assuming no other redox reaction occurs. (Note: The atomic mass of lead is 207.2 g/mol and the Faraday constant is 96,485 C) 1.79 x 102g P 0.686 g Pb O5.34 x 102 g Pb 0.343 g Pb O 1.02 g Pb
Initial mass of the anode was 10.00 g of Zinc and the initial
mass of the cathode was 10.00g of iron. A simulation was done with
the current to 6.00 A and a 40.00 min time. (this information may
not be needed)
Part C: Electrolytic Cell and Calculation of Faraday's Constant (Using hits media.pearson me som/bc bemedia_chemchemummillest php) Cathode Final Mass 104.88 Cathode Initial Mass 16.00 4.88 Difference (m) g What do you notice in comparison to the change at...
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...
Part B and D
Please show all of the steps.
Learning Goal: To relate current, time, charge, and mass for electroplating calculations. Electroplating is a form of electrolysis in which a metal is deposited on the surface of another metal. To quantify electrolysis, use the following relationships. Electric current is measured in amperes (A), which expresses the amount of charge, in coulombs (C), that flows per second (s): 1 A 1 C/s Another unit of charge is the faraday (F),...
i cant get B for some reason!!! if you can help that would be
great !!!!
2 attempts left Check my work Be sure to answer all parts. When an aqueous solution containing gold (III) salt is electrolyzed, metallic gold is deposited at the cathode, and oxygen gas is generated at the anode. (a) If 8.61 g of Au is deposited at the cathode, calculate the volume of Oz generated at 23°C and 749 mmHg. 0.809 (b) What is the...
Standard free energy change (Delta degree G) and cell potential (E degree) can be said to measure the same thing and are convertible by the equation: Delta G degree = nF E degree _cell where n is the total number of moles of electrons being transferred, and F is Faraday constant 9.6- 1853415 times 10^C/mol. The free energy (Delta G degree) of a spontaneous reaction is always negative. For each of the electrochemical cells below, calculate the free energy of...
need help !! with questions 2,4,5,6
Initial Mass of Cathode electrode (Fe) Initial Mass of Anode electrode (Zn) Final Mass of Cathode 10.0g 10, og 10,209 .2g Fe 3+ (aq)+32 z Fecs) Mass of Zinc deposited on cathode (g) Half reaction in Cathode Half reaction in Anode Zn(s) Eszn²+ (aq) + Ze Za(s) + 2 Fest (1) ► 2* (g) +2 Fe²+ (aq) Overall Cell Reaction Standard Cell Potential, Ecellº .440 +.763 3.32 3 (Eºcell = Ecathode - Eanode) Number...
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