The galvanic cell Zn(s) | Zn2+(aq) | | Ni2+(aq)| Ni(s) is constructed using a completely immersed zinc electrode that weighs 32.68 g and a nickel electrode immersed in 575 mL of 1.00 M Ni2+(aq) solution. A steady current of 0.0715 A is drawn from the cell as the electrons move from the zinc electrode to the nickel electrode.(a) Which reactant is the limiting reactant in this cell?(b) How long does it take for the cell to be completely discharged?(c) How much mass has the nickel electrode gained when the cell is                   completely discharged?(d) What is the concentration of the Ni2+(aq) when the cell is completely           discharged?

Q: A student does an experiment to determine the molar solubility of lead(II) bromide. He constructs a…

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Q: Calculate the standard cell potential for the reaction below, and note whether the reaction is…

A: Given, Mg(s)+Ni2+(aq)⟶Mg2+(aq)+Ni(s)   Ni2+(aq)+2e−⟶Ni(s) −0.257 Mg2+(aq)+2e−⟶Mg(s) −2.372

Q: Given the standard cell potential, E°ce = 1.10 V, for the cell, Zn(s) | Zn(NO,)(aq) || Cu(NO,)(aq) |…

A: Standard cell potential (E°cell) = 1.10 V  Temperature = 25°C.  The reaction :  Zn(s) + Cu2+(aq)…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: Cu²* (aq)+…

A: The reaction given is, Cu2+aq+Zns→Cus+Zn2+aq Cu2+ is being reduced to Cu and Zn is being oxidised to…

Q: 1,Find the standard change in free energy and the equilibrium constant for the galvanic cell…

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Q: Under standard conditions, hydrogen gas reacts with Hg2+ ions to produce H. The (aq) net cell…

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

A: Given: Cell reaction: Sn2+(aq) + Ba (s)---> Ba2+(aq) + Sn (s)

Q: Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is…

A: Given : Table of half reactions and reduction potential.  To find: Complete the given table.…

Q: For the cell described by the cell diagram below: solve for the total cell potential  Cu (s) | Cu+2…

A: The objective of the question is to calculate the total cell potential for the given electrochemical…

Q: How long would it take to deposit 3.75 g of iron from an aqueous solution of iron (III) sulfate by…

A: According to Faraday's First Law of Electrolysis, the chemical deposition due to flow of current…

Q: A Zn²+ Zn half-cell is connected to a Cu²+ Cu half-cell to make a galvanic cell, in which [Zn²+] =…

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Q: What is the cell potential for the (non-standard) cell at 298.15 K represented by:Pt(s) | Sn2+(aq)…

A: 1. Determine the half-reactions and their standard potentials (E^∘):   - For the anode (oxidation),…

Q: 19.69 Calculate the standard cell potential of the following cell at 25°C.…

A: In the electrochemical cell notation, chromium electrode function as anode and mercury function as…

Q: Use the Nernst equation to calculate the cell potential,  Ecell, for a galvanic cell consisting of…

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Q: galvanic cell is constructed in which a Pt | Fe2+ Fe3+ half-cell is connected to a Cd2+ | Cd…

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Q: 1) The standard reduction potentials of Cu2+ (aq) Cu(s) and Ag+ (aq) Ag(s) are +0.34 and +0.80 V,…

A: Calculate the cell potential of the given galvanic cell.  Given  At Anode  Cu/Cu2+; E°=-0.34 V At…

Q: What is the balanced chemical equation for this galvanic cell reaction? Cr(s) | Cr3*(aq), 1M || CI-…

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Q: Cr(s) | Cr^3+(aq) || VO2+(aq), H+(aq), VO^2+(aq) | Pt(s)   Calculate the equilibrium constant…

A: Anode or oxidation half-cell reaction

Q: This is an example of a disproportionation reaction:…

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Q: Identify the CORRECT cell notation for the galvanic cell (diagram below) that involves an…

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Q: What is E at 25 °C for the reaction described by Mg(s) | Mg²⁺ (1.60 M) || Pb²⁺ (0.850 M) | Pb(s)?…

A: Mg(s) | Mg²⁺ (1.60 M) || Pb²⁺ (0.850 M) | Pb(s) Standard cell potential (E°cell) = +2.231 V Cell…

Q: What mass of material will be deposited at the cathode when a current of 10.5 A is applied for 2.0…

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Q: What is the maximum amount of work that could be done by the following electrochemical cell?…

A: Ans  Maximum work done by the electrochemical cell is equal to the change in the Gibbs free energy

Q: Using values from the table of standard reduction potentials, calculate the cell potential (in V) 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.