How many grams of cobalt metal will be deposited when a current of 20.0 A is passed through a solution of cobalt(II) chloride for 54.5 minutes?

Q: Solve for Ecell given the following notation for galvanic cell Cu | NH3 (0.533 M), [Cu(NH3)42+]…

A: Given cell is :  Cu | NH3 (0.533 M), [Cu(NH3)42+] (0.033 M) || Cu2+ (0.10 M) | Cu Solve for Ecell…

Q: An engineer is assigned to design an electrochemical cell that will deliver a potential of exactly…

A: In this we have design an electrochemical cell of given electrode potential i.e 1.52 V with…

Q: Draw a picture of a galvanic cell (labeling all important parts), based on the following species…

A: Interpretation : We have to draw the galvanic cell ,

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

A:

Q: Calculate the number of moles of electrons driven through an electrolytic cell with 3457 A of…

A:

Q: A zinc bar (atomic mass = 65.38 g/mol; ion charge = 2) is weighing 2.08 kg is attached to a buried…

A:

Q: Brass, an alloy of copper and zinc, can be produced by simultaneously electroplating the two metals…

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Q: current of 0.075A passes through a solution of silver nitrate for 10 minutes. How much silver is…

A:

Q: How many seconds (s) are needed to deposit 3.62 g of copper metal from an aqueous solution of CuCl2,…

A: We have given current of 5.3 A . Mass of copper deposit required is 3.62 g Time required is being…

Q: Compute for the oxidation number of the following elements. a. C2042 с. НСО:1 e. FeO42 b. B4072 d.…

A: Oxidation number :- Charge of a particular atom in a  compound or molecule is considered to be…

Q: (Q96) Which of the following is true of both voltaic and elecrolytic cells? An outside energy source…

A: The correct answer is given below

Q: The electrode potential is given positive sign if the electrode reaction involves reduction, i.e…

A: Firstly ,we have to understand what means of Liberation of electron, The Liberation of electron…

Q: What statement is true for a galvanic cell? O Oxidation takes place at the anode. O The standard…

A: A galvanic cell is an electrochemical cell in which an electric current is generated from a…

Q: A current of 4.21 A is passed through a Fe(NO,), solution for 1.30 h. How much iron is plated out of…

A: According to Faraday's law  W= ZIt = (E/F)It  E = equivalent weight of Fe = 28 F =  Faraday's…

Q: What statement is true for a galvanic cell? Periodic Table and Datasheet Cations from the salt…

A: An electrochemical cell which produces electrical energy from chemical energy occurred during the…

Q: How many grams of aluminum can form by passing 305 Cthrough an electrolytic cell containing a molten…

A: The balanced half cell reaction is: Amount of current passed = 305 C Charge of 96485 C is carried…

Q: Tin-plated steel is used for “tin” cans. Suppose that in the production of sheets of tin-plated…

A: Given: Current passed = 100.0 A. Time taken = 8 hours = 8 × 60 × 60 = 28800 s…

Q: Construct a complete galvanic cell/voltanic cell set up. Label it and show the flow of electrons and…

A:

Q: Give the standard line notation for each cell.

A: In an electrochemical cell, the electrical energy is produced from the spontaneous cell reaction at…

Q: A current of 5.37 A is passed through a Cu(NO,), solution for 1.20 h. How much copper is plated out…

A: We will first take out the quantity of charge passes in given time interval. Then we will relate…

Q: A zinc bar (atomic mass = 65.38 g/mol; ion charge = 2) is weighing 2.18 kg is attached to a buried…

A:

Q: A certain half-reaction has a standard reduction potential E=-1.25 V. An engineer proposes using…

A: Answer

Q: The partial pressure in atm required for half-cells that generate or consume gas for its standard…

A: Electroanalytical chemistry is a branch of analytical chemistry which pressurizes on the…

Q: The electrolyte concentration in Mat which an electrochemical cell is at its standard state. Round…

A:

Q: current of 2.505 A deposits 1.371 g of a metal M from a solution that contains the metal ion M²⁺ in…

A: Given, current (i) = 2.505 A Time (t) = 30 × 60 = 1800 s Mass = 1.371 g  Using Faraday's law,  Mass…

Q: In an experiment two electrolytic cells were connected so that the same current passed through both…

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Q: Aluminum plating is sometimes used to reduce corrosion in materials exposed to the outdoors. A…

A: Aluminium sulfate , Al2(SO4)3 is an Electrolytic Substance which on Electrolysis gives aluminium and…

Q: How many hours are required to produce 795 grams of lead from molten lead(II) chloride (PbCl2, 278.1…

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Q: If an electrolytic cell contains a mixture of species that can be oxidized, how do you determine…

A: Electrolytic cell is also known as electrochemical cell, the reduction or oxidation reaction takes…

Q: 1. A current of A passes through an electrolytic cell for 6 mins. How many moles of electrons are…

A: If a charge Q flows through the cross-section of a conductor in time t , then we know ,…

Q: 1. Briefly define the following terms. (a) Anode and cathode (b) Reference electrode (c) Standard…

A: "To get remaining sub-parts solved please repost the complete question and mention the sub-parts to…

Q: To get electrical energy from an Galvanic cell the emf should ans. Positive None Zero Negative

A:

Q: What to do: Read each statement below and identify if it defines electrode potential, reduction…

A: A question based on electrochemistry that is to be accomplished.

Q: Enter your answer in the provided box. What is the emf of a cell consisting of a Pb2+ / Pb half-cell…

A:

Q: Consider electrode potential data given in Question 4 (c). Predict which two electrodes combination…

A: Standard EMF of an electrochemical cell is given by the equation: Eocell = Eocathode - Eoanode…

Q: An engineer is assigned to design an electro chemical cell that will deliver a potential of exactly…

A: Given information: Cell potential = 1.52 V

Q: Where are electrons received and donated at in a galvanic cell?

A: In galvanic cell electrons are produced at anode and moving towards cathode or electrons are donated…

Q: An active (metal) electrode was found to lose mass as the oxidation-reduction reaction was allowed…

A: In the oxidation - reduction reaction, oxidation occurs at anode and reduction occurs at cathode.…

Q: construct the table of aluminum electrode potentials as a function of the concentration of Al3 +…

A: Considering Al electrode to be an anode, the reaction taking place will be: Al(s)→Al3+(aq)+3e- The…

Q: How would you know whether a redox reaction is taking place in an acidic / alkaline or neutral…

A: Reactions where both oxidation and reduction is taking place are redox reactions. In oxidation half…

Q: Explain corrosion using electrochemical principles.

A: Corrosion happens when metals are attacked by acid or moisture and get corrode. This process is…

Q: A baby's spoon with an area of 6.25 square centimeter is plated with silver from silver nitrate…

A: (A)

Q: The electrolyte concentration in M at which an electrochemical cell is at its standard state. Round…

A: The cell potential of the electrochemical cell in its standard conditions give the vaues of standard…

Q: What mass of aluminum metal can be produced per hour in the electrolysis of a molten aluminum salt…

A:

Q: What is E° for this cell?

A: Ecello = SRP of Cathode - SRP of Anode  Ecello = Ecathodeo  - Eanodeo   Potential difference of…

Q: How many grams of nickel remains in a 100 ml of 1.50 M NiCl4 solution if 3.0 ampere current is…

A: The amount of Nickel deposited has to be calculated.

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.