Calculate the current at the cathode of a Hofmann Electrolytic cell with an Initial pH of the electrolyte solution of 5.56. A total time of 40min ,Cathode volume of 52mL and a final pH of 11.18 at the cathode.
Calculate the current at the cathode of a Hofmann Electrolytic cell with an Initial pH of...
help please! a piece of jewelry is connected to the cathode of an electrolytic cell and immersed in a solution of 1.00 M AgNO3 (aq). How long will it take to plate 45.0 mg of Ag onto the object using a current of 0.225 A?
What mass of silver is deposited on the cathode of an electrolytic cell if an electric current of 2.86 A is run through a solution of AgNO3 for one hour? Select one: O a. 11.5 g O b. 5.76 g O c. Og O d. 0.11 g o e. 0.192 g
What is the reduction half-reaction? In the electrolytic cell of this experiment, copper metal is the anode and zinc metal the cathode. The electrolyte solution is sulfuric acid, H2SO4. Oxidation occurs at the copper anode, where Cu is oxidized to Cu^2+: Cu (s) → Cu^2+ (aq) + 2 e– During the experiment, you might have noticed that at the end of the trials, the solution becomes slightly blue, which proves the existence of aqueous Cu^2+. What is the reduction half-reaction...
How many grams of Ag(s) could be plated out on the cathode of an electrolytic cell by the passage of 5.0 Amps of current through AgNO3 solution for 1 hour? A. 5.2 x 10-5 g B. 0.19 g C. 20 g D. 5.5 x 10-3 g
Draw a diagram of the electrolytic cell from Part 1. Identify the cathode, anode, directions in which the electrons, and ions move. Show how the nickel atoms migrate from the anode and how they deposit on the cathode. Show the power source and then identify the positive and negative terminals of the power source. Identify the positive and negative electrodes. Identify and write the oxidation and reduction half reactions and write the mass of each electrode at the start and...
Calculate the pH of the cathode compartment solution if the cell emf at 298 K is measured to be 0.660 V when [Zn2+]= 0.40 M and PH2= 0.91 atm .
Calculate the pH of the cathode compartment solution if the cell emf at 298 K is measured to be 0.630 V when [Zn2+]= 0.26 M and PH2= 0.99 atm . Express your answer using two decimal places
1. Calculate the pH of the cathode compartment solution if the cell emf at 298 K is measured to be 0.610 V when [Zn2+]= 0.20 M and PH2= 0.92 atm . Express your answer using two decimal places. pH= Switch 8.76 Voltmeter 7n anode NO, Na +H (8) Cathode compartment (standard hydrogen electrode) Anode compartment NO, Zn2+ NO NO, Zn(s) —> Zn2+ (aq)+ 2e 2H+ (aq) + 2e →H(8)
Part A Calculate the pH of the cathode compartment solution if the cell emf at 298 K is measured to be 0.640 V when [Zn240.27 M and PH = 0.85 atm. Express your answer using two decimal places. V ΑΣφ pH =$ Figure 1 of 1 Previous Answers Request Answer Submit Switch 8.76 X Incorrect; Try Again; 2 attempts remaining Voltmeter Zn anode NO Na - H2(g) Cathode compartment (standard hydrogen electrode) NO3 Zn2 Provide Feedback Next Anode compartment NO3...
Given the following electrolytic cell: The current is discharged into the electrolytic cell containing the solution CuSO4(aq) 1.0M at 25 oC. During the operation of the cell, copper Cu(s) is deposited on one electrode and oxygen O2(g) gas is released, near the second electrode. O2(g) + 4H3O+(aq) + 4e- 6H2O(l) Eo= 1.23V Cu2+(aq) + 2e- Cu(s) Eo= 0.34V A. The current in the cell is 1.5 amperes. The current is streamed in 40 minutes. i. Calculate the mass of copper...