t the cathode during the electrolysis of an aqueous solution of magnesium iodide, MgI2?

Q: The electrolysis of an aqueous solution of KBr has the overall reaction: 2H2O+2Br (aq) → H2(g) +…

A: The given balanced chemical equation is:              2H2O + 2Br-aq → H2g + Br2l + 2OH-aq Bromide…

Q: The reactions occurring at (i) anode, (ii) cathode, during working of a mercury cell. Why does the…

A: A voltaic cell is an example of electrochemical cell. It uses a chemical reaction to produce…

Q: Describe the process of Electrolysis of water?

A: Eleсtrоlysis  оf  wаter  is  the  рrосess  by  whiсh  wаter  is  deсоmроsed  intо  оxygenаnd…

Q: during the electrolysis of aqueous solution of LiNO3, what is the reaction of the environment that…

A:

Q: if 9.8g water is used in electrolysis, what is the percent yield if 5.6g of oxygen was collected…

A:

Q: What products are produced from the electrolysis of a solution of iron(II) bromide?

A: Electrolysis is a process in which an electrolyte in molten state or aqueous state is decomposed by…

Q: If 10 amp of current is passed through a solution of CaCl2 for 10 minutes in an electrolytic cell,…

A:

Q: Calculate the mass in grams of Zn deposited at the cathode in 42.5 minutes when 1.87A of current is…

A:

Q: 5. The mass of metal deposited by the electrolysis of an aqueous solution of metal ions increases in…

A:

Q: write the half-reactions that occur at the anode and cathode during the electrolysis of NH4NO3 in…

A: When aqueous solution of Ammonium nitrate (NH4NO3) is electrolysed then initially Following reaction…

Q: Why is it necessary to keep the chlorine and sodium, resulting from the electrolysis of sodium…

A:

Q: What are the products in the electrolysis of aqueous copper (II) iodide?

A:

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: 3. A factory wants to produce 1.0 x 103 kg Barium from the electrolysis of molten barium chloride.…

A: The given values are: m=1.0×103 kg=1.0×106 gt=4.0 h=4.0 ×3600 s The electrolysis step to form barium…

Q: What are the products obtained in the electrolysis of a molten mixture of KIKI and KBr

A:

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

A:

Q: The cathode reaction is: AUA13+

A: The voltaic cell is basically an electrochemical cell that generates electrical energy using 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: A steady current was passed through molten CoSO. until 2.35 g of metallic cobalt was produced.…

A:

Q: Aluminum is produced commercially by the electrolysis of Al2O3 in the presence of a molten salt. If…

A:

Q: What products are obtained in the electrolysis of molten NaI?

A: In an electrolytic cell, electrical current is used to drive a non-spontaneous redox reaction…

Q: Electrolysis plays an important role in the manufacture or purification of all of the following…

A:

Q: Write the anode and cathode reactions that cause the corrosion of iron metal to aqueous iron(II)

A: Corrosion is a natural process that converts a refined metal into a more chemically stable form such…

Q: 8. Which of the following is NOT produced during the electrolysis of water? Electricity a) b) Acid…

A: we have to select the option which is  not produced in electrolysis of water

Q: 2Al2O3 + 3C = 4Al +3CO2 If an elecltrolytic cell has a constant voltage of 4.4 V and produces a…

A: Given: 2Al2O3 + 3C = 4Al +3CO2 If an elecltrolytic cell has a constant voltage of 4.4 V and produces…

Q: Aluminum metal can be made from aluminum(III) ions by electrolysis. What is the half-reaction at the…

A:

Q: Please make a sketch in the electrolysis of aqueous potassium bromide and indicate the anode and…

A:

Q: write the half-reactions that occur at the anode and cathode during the electrolysis of (NH4)2SO4 in…

A: Electrolysis is the process in which electric energy is converted into chemical energy. During…

Q: >Why does the electrolysis of an aqueous sodium chloride solution produce hydrogen gas at the…

A: In electrolysis of aqueous solution of NaCl, the solution would simply result in the electrolysis of…

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

A:

Q: Electrolysis plays an important role in the manufacture or purification of all of the following…

A: There are different type of compounds, which are synthesized by different methods -  (1) Sodium, Na…

Q: Predict the products of the electrolysis of an aqueous solution of sodium chloride in cell using…

A: Electrolysis is a spontaneous redox process Here we are required to find the product when aqueous…

Q: In the electrolysis of an aqueous solution of Na2SO4, what reactions occur at the anode and the…

A: Explanation to the correct answer is given below

Q: what is Faraday's second law of electrolysis ?

A: Electrolysis:Separation of a liquid into its chemical parts by passing direct electric current…

Q: How many amperes of current needs to be passed through molten Sodium chloride (NaCl) to produce 2.1…

A: We have given that during the electrolysis of molten Sodium chloride 2.1 g of Sodium is produced at…

Q: Which products are obtained in the electrolysis of molten NaI?

A: Na metal produced at cathode and I2 produced at anode.

Q: Explain The Electrolysis of Aqueous Sodium Chloride and Overvoltage?

A: At the cathode, the half-reaction with higher reduction potential will be preferred. The reduction…

Q: Why is sodium metal not obtained when an aqueous solution of NaCl undergoes electrolysis?

A: In an electrolytic cell, there are two compartments. One is the cathode and the other is the anode.…

Q: If an electrolysis plant operates its electrolytic cells at a total current of 150. A, how long, (in…

A: According to Faraday's First Law of Electrolysis, The amount of product deposited is directly…

Q: How long would it take to deposit 7.54 g of copper (molar mass 63.55 g/mol) at the cathode of an…

A: current = 15.9 A  (given) Molar mass of copper = 63.55 g/mol   (given) Cu is having n factor of 2…

Q: According to the calculation, the electrolysis formed 0.107 mol M. During this time, 7.00 g M are…

A: Given: No. of mole of  (M ) = 0.107 mole Mass of ( M ) = 7 g   Find Molar mass of ( M )= ???

Q: write the half-reactions that occur at the anode and cathode during the electrolysis of NH4Cl in…

A: Answer  Electrolysis of NH44Cl

Q: A factory wants to produce 1.0 x 10³ kg Barium from the electrolysis of molten barium chloride. What…

A:

Q: during the electrolysis of aqueous solution (NH4) 2SO4, what is the reaction of the environment that…

A: Electrolysis is a technique in which the electric current passes through the solution known as the…

Q: Mention the reactions occurring at (i) anode, (ii) cathode, during working of a mercury cell. Why…

A: A voltaic cell is an example of electrochemical cell. It uses a chemical reaction to produce…

Q: When 1.00 mole of chlorine gas is reduced to chloride ions in an electrolytic cell, what charge (in…

A: Reduction of 1 mol of chlorine is given below, Number of moles of electrons is 2.

Q: How many grams of copper are deposited on the cathode of an electrolytic cell if an electric current…

A: Faraday's law of electrolysisAsW= Ite/FF= 965900 Ct=20 x 60 sece for copper if taken in copper…

Q: Calculate the concentration of the Zn2+(aq) ion at the cathode.

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.