An inexpensive and accurate method of measuring th equantity of electricity passing through a circuit is to pass it through a solution of a metal ion and weigh the metal deposited.A silver electrode immersed in an Ag+ solution weighs 1.7854 g before the current passes and weighs 1.8016 g after the current has passed. How many coulombs have passed?

Q: A voltaic cell is constructed with two Zn2+−ZnZn2+−Zn electrodes. The two cell compartments have…

A: The cell is made up of Zn electrodes only. Hence both oxidation and reduction is happening for Zn…

Q: (o?locator=Dassignment-take A voltaic cell is constructed in which the following cell reaction…

A: The cell reaction is as follows-       Cl2(g) + 2I-(aq) ----> 2Cl-(aq) + I2(s)  At cathode,…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ Sn" (ag)…

A: Given: [Sn2+]=4.70 M[Ba2+]=6.41 MTemperature=25oC                       =(25+273) K…

Q: Consider these two entries from a fictional table of standard reduction potentials.…

A: Oxidation takes place at anode and reduction takes place at cathode. Loss of electrons is oxidation…

Q: A standard galvanic cell has a silver electrode in a .02M solution of Ag2SO4 and a gold electrode in…

A: From the standard reduction value, it can be conclude that which one will be oxidized or reduced.…

Q: Determine the molar mass (amu) of Metal (M) if it took 1.68 minutes for a current of 1.08 A to plate…

A: The metal will come out as M3++3e-= M . We can conclude from here that 3 moles of electrons are…

Q: A current of 0.452 A is passed through an electrolytic cell containing molten CaCl2 for 1.50 hours.…

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Q: 7. A voltaic cell based on the reaction between aqueous Br2 and vanadium(III) ions has Ecel = 0.73 V…

A:

Q: . Which phase changes result in ΔS < 0? 2. Which selection of coefficients properly balances the…

A: As per our guidelines , we can solve only first three questions. Please resubmit other questions as…

Q: A galvanic cell is set up by making 1 M solutions of FeSO4 and ZnSO4, with an iron (Fe) electrode in…

A: Interpretation-E0cell value. Concept introduction- Equation of half cell reaction anode-…

Q: If a soft bridge contain KNO3 as it electrolyte which ions diffuse into sulotion in the anode…

A: The salt bridge is a U-shaped tube which contains an electrolytic solution of inert electrolytes,…

Q: 5. For the following cell, write a balance equation for each half reaction occurring at the…

A: According to guidelines I am supposed to answer only first question asked by you In galvanic cell,…

Q: If a salt bridge contains KNO3 as its electrolyte, which ions diffuse into solution in the anode…

A: A galvanic cell is an electrochemical cell that is used to supply electric current through the redox…

Q: 5. For the following cell, write a balance equation for each half reaction occurring at the…

A: The following electrochemical cell problem can be approached as per follow.

Q: A galvanic cell consists of one half-cell that contains Ag( s) and Ag *(aq), and one half-cell that…

A: Two half cell reactions are given and asked that which species obtain at cathode and anode.

Q: A galvanic cell is set up by making 1 M solutions of FeSO4 and ZnSO4, with an iron (Fe) electrode in…

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Q: Consider the battery represented by the following notation. Ni(s) | Ni*"(aq) || Ag*(aq) | Ag(s)…

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Q: A common car battery consists of six identical cells each of which carries out the reaction:…

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Q: Consider these two entries from a fictional table of standard reduction potentials.…

A: To calculate standard potential of a galvanic cell:

Q: A zinc bar (atomic mass = 65.38 g/mol; ion charge = 2) is weighing 2.4 kg is attached to a buried…

A: The solution is given below -

Q: What mass of zinc (in grams) is deposited at the cathode when a current of 8.3 amperes passes…

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Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3Cu**…

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Q: A current 6.0 amperes is passed for 10 hours between copper electrodes in 800 ml of copper nitrate…

A: The charge carried by one electron is 96500 C. The electrode reaction:

Q: 4. The following materials are available to you: AgNO, to make any molarity of solution needed,…

A: Voltaic cell

Q: (c) The magnitudes but not the signs of the standard electrode potentials of two metals, X and Y…

A: In this given question we have to find out standard emf of a cell made up of X and Y metal.

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: How many minutes does it take to plate 164.8g of chromium onto a car part using 16.75 A of current…

A:

Q: Determine the molar mass (amu) of Metal (M) if it took 2.95 minutes for a current of 1.8 A to plate…

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Q: A galvanic cell consists of one half-cell that contains Ag(s) and Ag+(aq), and one half-cell that…

A: The galvanic cell consists of two half-cell ; at one half cell oxidation reaction occurs and at the…

Q: Consider these two entries from a fictional table of standard reduction potentials. X3+ + 3e X(s) E°…

A: Given, The equation of standard reduction potential; X3+ + 3e- → Xs    ....(1) E0 = -1.75 V Y3+ +…

Q: Given the following notation for an electrochemical cell, what is the balanced overall (net) cell…

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Q: Write the Nernst equation for the cell Pt(s) U H2(g, 1.0 X 1026 bar) U H1(aq, 0.50 M) i Ag1(aq, 1.0…

A: Nernst equation The equation that relates cell potential to the concentration of oxidized and…

Q: 5) During the operation of lead storage battery, the reaction at the two electrodes is as follows:…

A:

Q: Consider these two entries from a fictional table of standard reduction potentials. X³+ + 3e → X(s)…

A:

Q: b) Diagram below shows a galvanic cell that operates under standard conditions represented by the…

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

Q: 5. Consider a galvanic cell consisting of 5Feta) + MnOñcag) + 8H°aq) → 5Fečq) + Mnřa) + 4H20u) Write…

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Q: A current of 0.4 Amps flows for 2 hours through an electrolytic cell containing copper sulphate…

A: This problem can be solved by using Faraday's first law of electrolysis accordingto which weight of…

Q: A current 6.0 amperes is passed for 10 hours between copper electrodes in 800 ml of copper nitrate…

A: Electrolysis is a process in which current is passed through a substance .In this chemical reactions…

Q: How long would it take to deposit 2.72 g of copper from an aqueous solution of copper II sulfate by…

A: Given that : Mass of copper to be deposited (w) = 2.72 g Current (i) = 2 amps

Q: Consider these two entries from a fictional table of standard reduction potentials. X3+ + 3e- X(s)…

A: The solution is as follows :

Q: galvanic cell is made using 0.25M ZnSO4 and an unknown amount of CuSO4. The cell potential is 105V…

A:

Q: The two half-reactions in a voltaic cell are: Zn(s) Zn2*(aq) + 2 e CIO3 (ag) + 6 H*(aq) + 6 e¯ CI…

A: Answers are explained below.  Between the given two half-reactions, former is the oxidation reaction…

Q: A concentration cell consists of two Sn/Sn2+ half-cells. The electrolyte in compartment A is 0.13M…

A: The given cell is an example of concentration cell.In concentration cell, the concentration of two…

Q: Balance the redox reaction equation (occurring in acidic solution) and choose the correct…

A: Introduction In order to do the balancing of any particular reaction, first thing we need to do is…

Q: For the reaction S₄O₆²⁻(aq)+ 2I⁻(aq) →I₂(s)+ S₂O₃²⁻(aq) ΔG°=87.8 kJ/mol(a) Identify the…

A: Given reaction: S4O62-aq+2I-aq→I2s+S2O32-aq

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

A: Faraday's Law of Electrolysis: The Faraday's law of electrolysis states that the amount of electric…

Q: Silver can be electroplated at the cathode of an electrolysis cell according to the following…

A: Current = 7.9 A Time = 73 min Ag^+(aq)+ e^-→Ag(s) From this Reaction we get that ,  1 mole e- is…

Q: A galvanic cell runs for 1 minute with a current of 0.25 A. How much charge passed through the cell…

A: Given : Current passed = 0.25 A And time = 1 min F=96500 C/mol

Q: II. 1.Represent in the conventional manner, i.e., anode/cathode, the voltaic cell in which each of…

A:

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.