Determine the molecular mass and identity of a +2 metal, X, that plates 46.3g of X in 6.75 hours at a current of 2 A.

Q: A current of 3.79 A is passed through a Sn(NO^), solution. How long, in hours, would this current…

A: Oxidation is the process that involved the loss of electrons and oxidized to cation.  Hence when a…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ Cu²+ (aq)…

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Q: Consider the electrolysis reactions cathode Cu?"(aq, 0.177 M) + 2e-= Cu(s) H,O) =0,(g, 1 bar) + 2H*…

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Q: A certain metal M forms a soluble sulfate salt M2SO4. Suppose the left half cell of a galvanic cell…

A: To solve  given problem , let's break down  information  provided and use our understanding of…

Q: • Part D Hg (1) + HgCl, (aq) → Hg,Cl2 (s) Express your answer using ftwo significant figures. ΑΣφ ?…

A: The given reaction, Hg(l)+HgCl2(aq) → Hg2Cl2(s)

Q: Calculating the mass of an electrolysis product from the applied... In the industrial "chlor-alkali"…

A: Current is defined as the rate of flow of charge. Current= Charge÷ time  Charge = current x time  1…

Q: [References] A particular voltaic cell operates on the reaction Zn(s) + Cl2 (g) → Zn²+ (ag) + 2CI…

A: The solution is as follows :

Q: 7. Consider the galvanic cell shown below (the contents of each half-cell are written beneath each…

A: Given,E∘C3+/Cr=-0.727VE∘Br2/Br-=+1.090V

Q: A galvanic cell is established to power a torch, as shown.For this cell, the overall equation will…

A: The given cell diagram is : Options are : Overall cell equation for this reaction = ?

Q: iv Write the potential for each half-reaction next to it (the values are in your text) V Calculate…

A: Dear student , since you have posted multiple parts questions we are allowed to solve only first…

Q: How long would it take

A: Farrady law of electrolysis  m=Z I t

Q: 'red A certain half-reaction has a standard reduction potential Eed = -0.94 V. An engineer proposes…

A: Ecello​≥1.10VEcato​−Eano​≥1.10V−Eano​≥1.10V−Ecato​Eano​≤−(1.10V−(−0.94V))Eano​≤−2.04VBased on our…

Q: A galvanic cell was formed using Avium and Beanium:[hypothetical elements] Reduction Potentials:…

A: Answer - According to the question - Reduction Potentials: Av3+(aq) + 3e- → Av(s).       Eo = -0.48…

Q: given the following equation identify the oxidizing agent 2 Mg + O2 --> 2 MgO

A: The balanced reaction given is, => 2 Mg + O2 → 2 MgO

Q: A certain metal M forms a soluble nitrate salt MNO, Suppose the left half cell of a galvanic cell…

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Q: [References] A particular voltaic cell operates on the reaction Zn(s) + Cl2 (g) → Zn+ (ag) + 2C1…

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Q: O ELECTROCHEMISTRY Understanding concentration cells 1/5 A certain metal M forms a soluble sulfate…

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Q: 6. Which of the following correctly differentiate a galvanic from an electrolytic cell? GALVANIC…

A: Galvanic cell is a cell which converts chemical energy into electrical energy. It is also known as…

Q: A certain metal M forms a soluble nitrate salt M (NO), Suppose the left half cell of a galvanic cell…

A:

Q: 5. a) What type of voltaic cell is constructed from half cells consisting of the same electrode…

A: An electrolytic cell is one which converts electrical energy to the chemical energy i.e. an external…

Q: Use the following data to calculate the molar mass of naturally occurring silicon: Isotope…

A: Average Atomic mass = M1X1+M2X2+M3X3/(X1+X2+X3) Where,  M1 ,M2 & M3 are atomic masses and X1 ,X2…

Q: In an car battery recharging occurs when the car is running by supplying a current to the battery.…

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Q: 9. How many grams of Cu are plated out from a CuSO4 solution by a current of 7.8 amps flowing for…

A: We have to predict the mass of Cu deposited.

Q: 6. Zinc (Zn) can be purified by the electrolysis of aqueous zinc sulfate. Suppose an electrolytic…

A: Given that, In the electrolytic cell : Molarity of ZnSO4 solution = 0.050 M Weight of zinc deposited…

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.