The half reaction at an electrode during electrolysis is        Mg2+ (molten) + 2 e- → Mg (s) Calculate the number of grams of magnesium that can be produced by supplying 20,000 Coulomb charge to this electrode. The molar mass of Mg is 24.31 g/mol. There is 96,500 Coulomb charge in every mol of electrons.

Q: A total of 1.740 F of electricity (1 F=1 mol e−) was required to electrodeposit all of the Zn and Co…

A: The mass of each compound is calculated by the number of moles of the compound. The number of moles…

Q: 23) Consider an electrochemical cell based on the reaction: 2H+ (aq) + Sn (s) → Sn2+ (aq) + H₂ (g)…

A: The objective of the question is to understand which of the given actions would change the measured…

Q: Hint: In this question you must make use of your knowledge of thermodynamics and the redox potential…

A: The above problem is from electrochemistry.

Q: a) If Mg(OH)2 and H2 are in water in a covered container and a voltage is applied to produce…

A: When an electric current is passed through a solution containing Magnesium Hydroxide (Mg(OH)2) and…

Q: 1. In an electrolysis cell similar to the one employed in this experiment, a student observed that…

A: Given volume of hydrogen gas is 94.50 mL  Given barometric pressure is 740mmHg and vapour pressure…

Q: MISSED THIS? Read Section 20.8 (Page). Silver can be electroplated at the cathode of an electrolysis…

A: According to Faraday first Law of Electrolysis "  The chemical deposition due to the flow of current…

Q: sof s of a That is

A: We will identify the alkaline earth metal

Q: Why does the electrolysis of an aqueous sodium chloride solu-tion produce hydrogen gas at the…

A: Electrolysis is a method of passing electric current through ionic or molten salt resulting in the…

Q: A certain metal M forms a soluble nitrate salt MNO 3. Suppose the left half cell of a galvanic cell…

A: To answer  questions in  problem , we need to determine which electrode will be positive and…

Q: Electrolysis - 4.00 Amps of current is passed through a solution of NiSO4 (aq) for 12.0 minutes.…

A:

Q: Write a balanced chemical equation (including states of matter) for an electrochemical cell that has…

A: An electrochemical cell is a device which is used to generate electrical energy from the chemical…

Q: Write the half reaction in the cathode, if the Ag+ cation is reduce to form silver metal.       Ag+…

A:

Q: Which metal will get oxidized? what is the total Coulomb?

A: Those metal which have high standard reduction potential act ascathode & low reduction potential…

Q: write the half-reactions that occur at the anode and cathode during the electrolysis of NH4OH in…

A:

Q: In the commercial preparation of aluminum, aluminum oxide, Al,O3, is electrolyzed at 1000°C. (The…

A: Since from the above reaction we can see that 1 mole of Al is produced when 3 moles of electrons is…

Q: Balance the following redox reaction that occurs under basic, aqueous conditions: NiO2 + Fe →…

A: To balance a redox reaction,follow the below mentioned steps: 1) Consider oxidation and reduction…

Q: A proposed battery involves the reaction of Zn(s) and Cl2(g) to give ZnCl2. If you want such a…

A: The Faraday’s first law of electrolysis state that the mass of the substance  deposited at any…

Q: A galvanic cell reaction transfers 4 electrons as it proceeds. Calculate ΔGº in kJ/mol if the Eº for…

A: Standard cell potential (E°) = +0.589 V = +0.589 J/C Faraday constant (F) = 96485 C/mol Number of…

Q: Chlorine, Cl2, is produced commercially by the electrolysis of aqueous sodium chloride. The anode…

A: 1 F = 96500 C  Moles of chlorine = 1090 / 71 = 15.35 moles  Total charge = 2 × 15.35  F = 2 × 15.35…

Q: ammonia, NH3, Produced in the organ process (nitrogen gas and hydrogen gas are used as starting…

A: Since you have asked multiple questions with multiple subparts, we will solve the first question for…

Q: Sketch the galvanic cell based on the following overall reactions. Calculate E°; show the direction…

A: For a cell   Cell potential = E°Reduction half  - E°Oxidation half Species whose reduction potential…

Q: 14.106 A voltaic cell is constructed in which the following reaction takes place: Cu (s) + 2Ag+ (aq)…

A: Number of moles of a substance is defined as ratio of mass in gram of substance to the molar mass of…

Q: Use the References to access important values if needed for this question. Enter electrons as e. Use…

A: Anode is the electrode where the oxidation take place. Reduction potential of all the species are…

Q: Which statement explains why an over-potential must be used in the Chlor-Alkali process? 02 will be…

A: Chlor-Alkaline process is the electrolysis of NaCl solution. As it is an aqueous solution there are…

Q: Consider the electrolysis of molten barium chloride, BaCl₂. a) Write the half-reactions for anode…

A: Given, Consider the electrolysis of molten barium chloride BaCl2 : a) Half reaction for anode and…

Q: A certain metal M forms a soluble nitrate salt MNO3. Suppose the left half cell of a galvanic cell…

A: Electrochemical cells that have same electrolyte in two half-cells but with difference in their…

Q: A certain metal M forms a soluble nitrate salt MNO3. Suppose the left half cell of a galvanic cell…

A:

Q: Which of the following metals can be used to cathodically protect an iron sculpture? Nickel Lead…

A:

Q: Sketch the galvanic cell based on the following overall reactions. Calculate E°; show the direction…

A:

Q: A galvanic cell is powered by the following redox reaction: Cl,(g) + H,(g) + 2 OH (aq) → 2 Cl (aq) +…

A: Given : We have to write half reaction taking place at anode and cathode.

Q: Chromium can be plated from solution of CrCl3(aq) according to the following half reaction. How many…

A:

Q: Why EMF of the cell increases when the concentration of the solution at the anode decreases? Why EMF…

A:

Q: The electrolysis of water is often done with a small amount of sulfuric acid added to the water.…

A: The addition of sulphuric acid increases the conductivity of water.

Q: An unknown metal, X, has been deposited on the cathode of an electrolytic cell using an electric…

A: Given: Mass of X collected = 1.51 g. Current passed = 3.30 A Time = 25.0 min = 25.0 × 60 = 1500 s…

Q: The electrolysis of a copper sulfate solution to get copper metal is carried out using a current of…

A: According to Faraday’s first law of electrolysis, the mass of the element deposited is directly…

Q: What reactions take place at the cathode and the anode when each of the following solutions is used…

A: •Here NiBr2(aq) Solution given means NiBr2 dissolved in water(H2O). •Reduction potential of given…

Q: Che identity of the

A:

Q: Using the following standard reduction potential table, select 8 sets of atoms (4 pairs) from the…

A: Before doing this activity, you should know about some things.The higher the reduction potential,…

Q: Write a balanced chemical equation (including states of matter) for an electrochemical cell that has…

A:

Q: Electrolytic process of determining molar mass.  An electrolysis cell contains X3+ ions. When a 5.45…

A: In a electrolytic process, cations go to the anode and anions go to the cathode.

Q: For the electrochemical cell, Cd(s) | Cd2*(aq) || Co2*(aq) | Co(s), determine the equilibrium…

A: In this question, we will determine the value of Keq ( equilibrium constant) value. First we will…

Q: Over a period of time, the concentration of sulfuric acid in the lead storage battery of an…

A: Given data,Initial % by mass of H2SO4=38.0 %Final % by mass of H2SO4=26.0%Volume of H2SO4=734…

Q: A certain metal M forms a soluble sulfate salt MSO4. Suppose the left half cell of a galvanic cell…

A:

Q: grams of iron

A:

Q: Suppose the galvanic cell sketched below is powered by the following reaction: Fe(s) + SnSO4(aq) →…

A: Oxidation : Loss of electrons with an increase in the oxidation state. Oxidation takes place at…

Q: Electrolytic process of determining molar mass.  An electrolysis cell contains X3+ ions. When a 5.45…

A: Given: Current=5.45A Time=2.16×103s Mass of the element=8.50 g To find: Molar mass of X

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.