A     constant current     of     0.800     A     is     used to deposit copper     at    the cathode and oxygen    at    the anode    of    an    electroly6c cell.    Calculate the number of     grams     of     each product formed     in     15.2     min.     assuming no other redox reac6on.    The two half-reac6ons are:     (MW    Cu:    63.55    g/mol;    MW    O2:    32.00    g/mol)    (F    =    96485    C)                                      Cu2+        +    2e-                                                                Cu(s)     2H2O                                            4e-        +        O2(g)        +        4H+

Q: Assume the specifications of a Ni-Cd voltaic cell include delivery of 0.29 A of current for 1.00 h.…

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Q: A constant current of 1.6 A is used to precipitate copper at the cathode and oxygen at the anode of…

A: value of constant current = 1.6 A Time = 30.4 minutes cathode - copper Anode - oxygen

Q: Chromium can be electroplated from aqueous potassium dichromate, with the reduction shown below. If…

A: Given data Current (i) = 6 A Voltage (v) = 4.5 V Volume of K2Cr2O7 = 215 mL Concentration of K2Cr2O7…

Q: A 5.77 g of zinc is deposited at the cathode when a current of 7.1 amperes passes through an…

A: Given : Current = 7.1 A And time = 40 min = 40 X 60 = 2400 s…

Q: How much time in minutes would it take to deposit 4.01 grams of X (MW 163.10 g/mol) on a cathode in…

A: Faraday's second law states that, the amount of substances deposited by the passage of same amount…

Q: Calculate AGixn and Eo (cell

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Q: A half-cell is prepared by immersing a strip of indium metal in a solution containing 1 M In(NO3)3.…

A: Since you have posted question with multiple sub-parts, we are entitled to answer the first 3 only.…

Q: Three electrolytic cells are connected in a series. The electrolytesin the cells are aqueous…

A: The given data contains, current = 2.33 A. Mass of Cu = 1.74 g.

Q: All WOTK men A solution of NaCl (aq) is electrolyzed for 15.5 min using a current of 3.45 A. Write…

A: Given that, a solution of NaCl (aq) is electrolyzed. The time is t = 15.5 min = (15.5×60) sec = 930…

Q: An electrolytic cell was set up to investigate the electrolysis process for an aqueous solution of…

A: At the cathode (reduction) - 2 H+(aq) + 2e− → H2(g) E = 0.00 V At the anode (oxidation) 2 H2O(l) →…

Q: Copper is electroplated from CuSO4 solution. A constant current of 4.28 A is applied by an external…

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Q: During the discharge of an alkaline battery, 4.50 g of Zn is consumed at the anode of the battery.…

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Q: Suppose a current of 690 mA is passed through an electroplating cell with an aqueous solution of…

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Q: In a copper plating experiment in which copper metal is deposited from a copper(II) ion solution,…

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Q: A Voltaic cell is set up such that, a copper electrode and 1.0 M Cu(NO3)2 solution are placed in one…

A: Ans

Q: The galvanic cell utilizes the following reaction of oxidation of iron and reduction of cadmium at…

A: Fe + Cd+2       - - - - - > Fe+2  + Cd Cd+2 +2e- - - - - - > Cd         E° = - 0.40 V Fe - - -…

Q: A voltaic cell consists of a strip of cadmium metal in asolution of Cd1NO322 in one beaker, and in…

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…

Q: 10

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Q: The following half-cell is on the left and coupled with the standard hydrogen electrode on the right…

A: 1).

Q: Chromium can be electroplated from aqueous potassium dichromate, with the reduction shown below. If…

A: a) 215 ml  ofb1.25  potassium  means (1.25/1000)×215 = 0.26 mol of potassium dichromate.   From the…

Q: Determine the molar mass (amu) of Metal (M) if it took 2.85 minutes for a current of 1.1 A to plate…

A: Molar mass can be calculated as:-

Q: What mass of copper could be deposited from a copper(II) sulfate solution using a current of0.50 A…

A: The given problem can be solved by using the formula as; Q=I×t…

Q: If a constant current of 115 A is applied for 15.0 hours to the plating of cobalt from a cobalt(III)…

A:

Q: Two electrolytic cells are connected in series. The 1st cell contains copper sulfate solution while…

A: Given the current supplied to both the electrodes, I = 0.5 A Given the Ag electrode has 0.2 g lesser…

Q: 2) How long, in minutes, will it take to plate out 25.0g of Au from a AuCl3 solution if the current…

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Q: A galvanic cell using Mg|Mg2+ and Cu|Cu2+ half-cells operates under standard-state conditions at…

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Q: 8. A solution containing a metal ion (M2+ (aq)) is electrolyzed by a current of 7.8 A. After 15.5…

A: Given:Current (c)= 7.8 A time (t)= 15.5 min=15.5×60=930 s Mass of the metal-plated out =1.19 g To…

Q: A galvanic cell is constructed by linking a Co2+ | Co(s) half-cell to an Ag+ | Ag(s) half-cell…

A: a) The half cell reactions at cathode and anode are  - cathode - Co(s) →Co2+(aq) + 2e- Anode    - 2…

Q: An electrolytic cell for depositing copper from copper sulfate solutions is placed in series with…

A: We use the formula below to find the weight of a metal(W) deposited in an electrode during…

Q: Giorno Giovanna likes golden stuff. However, since he is currently broke, he has to settle for…

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Q: If a water electrolysis cell operates at a current of 7.9 AA , how long will it take to generate…

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Q: VOLTAIC CELL AND ELECTROLYSIS 1. Fischl, a scientist from Mondstadt specializing in…

A: Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: Determine AG (in kJ/mol) for a galvanic electrochemical cell at 38.01°C composed of a platinum…

A:

Q: An antique automobile bumper is to be chrome plated. The bumper, which is dipped into a dichromate…

A: Current passed = 21.4 A Mass of chromium to be deposited = 1.72 x 102 g Time required is to be…

Q: In an electrolytic cell, how many grams of nickel (MM = 58.69 g/mol) will be deposited on a metal…

A: we have to calculate the mass of Ni deposited

Q: A constant current of 0.50 A is used to deposit copper at the cathode and oxygen at the anode of an…

A: Current = 0.50 A  Time = 10 minutes  F = 96485 C  Molar mass of copper = 63.55 g/mol  Weight of…

Q: Assume the specifications of a Ni-Cd voltaic cell include delivery of 0.46 A of current for 1.00 h.…

A:

Q: Calculate the current supplied in Amperes if 5.0 g of lead is used, Pb is formed at the cathode…

A:

Q: A solution containing a metal ion (M2+ (aq)) is electrolyzed by a current of 7.8 A. After 15.5…

A: The amount of substance that undergoes a chemical reaction at any electrode during electrolysis is…

Q: products

A:

Q: In an electrolysis of a solution containing Ni2+ (aq), metallic Ni(s) deposits on the cathode. Using…

A: Given,  Current in ampere = I =  0.150 A  Electrolysis of Ni2+ (aq) ion  Time period in minutes = t…

Q: A half-cell is prepared by immersing a strip of indium metal in a solution containing 1 M In(NO3)3.…

A: Since you have posted questions with multiple sub-parts, we are entitled to answer the first 3 only.…

Q: Giorno Giovanna likes golden stuff. However, since he is currently broke, he has to settle for…

A: Ionic gold gains 3 electrons to get reduced to gold Au3+ + 3e-  --> Au

Q: How many seconds are required to deposit 0.150 grams of tin metal from a solution that contains Sn2+…

A: Mass = 0.150 g Current (i) = 0.652 A = 0.652 C/s  Time (t) = ?

Q: Suppose we construct a galvanic cell by placing two identical platinum electrodes in two beakers…

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Q: Consider the half reactions in  a cell:  Pb2+   +  2 e ------ Pb(s)  Eo  =  - 0.126  V…

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Q: 4. An electrolysis cell that deposits gold (from Au*(aq) operates for 15 minutes at a current of…

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Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.