Write equations for the half-reactions that occur in the electrolysis of a mixture of molten potassium bromide and molten lithium bromide.

Q: Describe the process of Electrolysis of water?

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

Q: Complete and balance the following half-reactions. In each case indicate whether the half-reaction…

A: NOTE: please note according to our policy , we can only answer first three subparts of a question.…

Q: Calculate the equilibrium constant for redox reaction between metallic zinc and silver Nitrate?

A: Equilibrium constant for a redox reaction is computed using the standard half-cell reduction…

Q: The chemistry of corrosion of iron is essentially an electrochemical phenomenon. Explain the…

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: What is the use of Platinum foil in the hydrogen electrode?

A: It is a type of gas electrode which we use as a reference for every other electrode to calculate…

Q: What half-reaction occurs at the cathode during the electrolysis of molten potassium bromide?

A: During the electrolysis process molten potassium bromide KBr broken into K+ and Br- ion.  K+ ion…

Q: Define the term half-Reactions?

A: ANSWERE IS DISCUSSED BELOW :

Q: Which of the following elements can be prepared by electrolysis of their aqueous salts: copper,…

A: The elements which lie above H2O in EMF series or having higher half cell potential can be prepared…

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

A:

Q: Sodium metal is produced commercially by the electrolysis of molten sodium chloride. The by-product…

A: Sodium metal is commercially produced by electrolysis of molten sodium chloride.  Sodium metal was…

Q: Balance the following oxidation-reduction reactions that occur in acidic solution using the…

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: what types of difficulties are to be faced during electrolysis of NaCl ?

A: We acquire hydrogen and chlorine by the electrolysis of aqueous sodium chloride where aqueous sodium…

Q: What process occurs at the anode in a galvanic cell? O galvanization O electrolysis oxidation O…

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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: Which of the following reactions occurs at the cathode of an electrolytic cell containing molten…

A: Eleсtrоlysis invоlves the mоvement оf iоns tо the eleсtrоde. Sоlid-stаte dоes nоt аllоw the mоvement…

Q: Write the name of the cell which is generally used in hearing aids. Write the reactions taking place…

A: Mercury battery Mercury battery is a non-rechargeable electrochemical battery. Mercury batteries…

Q: Complete and balance the following half-reaction in acidic solution Bi3+(aq) → BiO3(aq)

A: Write oxidation number of atom Bi. First balance atom other than O and H. Balance oxidation number…

Q: An active (metal) electrode was found to lose mass as the oxidation-reduction reaction was allowed…

A: Electrochemical cells The devices capable which are either produce electric current from chemical…

Q: Sketch the cell, labeling the anode and cathode and indicating the corresponding electrode…

A: In the voltaic cell, the electrical energy is produced by the redox reactions that occur…

Q: Assign each description as applying to the cathode or the anode of a galvanic cell. Where reduction…

A: The galvanic cell is a type of electrochemical cell that generates electrical energy from a…

Q: Complete the half-reaction equation for the conversion of hydrogen gas to water in a basic solution.…

A: This is oxidation reaction . Because electron is loosing.

Q: 4. Compare the product formed at the cathode in the electrolysis of copper(II) bromide solution…

A: Reduction potential is the measure of tendency  of a chemical species to be reduced by taking the…

Q: How to convert the electrolysis of liquid water into hydrogen ?

A: The question is about explaining the process of electrolysis to convert liquid water into hydrogen -

Q: What are the main components of an electrochemical cell?

A: An electrochemical cell is an apparatus or tool that produces electric current from chemical change…

Q: Lithium metal can be produced readily by the electrolysis of aqueous solutions of lithium nitrate,…

A: Lithium is  a chemical element with atomic number 3. It is a group 1 metal (alkali metal) Lithium is…

Q: Predict which cation will be reduced first if the following mixture of molten salts undergoes…

A: The Cations in the given salts are, NaCl = Na+ CaCl2 = Ca2+ AgCl = Ag+

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: Explain the process of electrolysis

A: The process of electrolysis has to be explained.

Q: Write the balanced equation, including states of matter, for the reduction half-reaction.

A:

Q: what electrochemical reaction uses in silver oxide battery

A: The electrochemical reaction used in the silver oxide battery is Redox reaction. The silver-oxide…

Q: Describe the process of Electrolysis?

A: Decomposition of electrolyte on passing electricity through its molten state or aqueous solution.…

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Q: How are reduction potential, oxidation potential, and cell potential obtained using the standard…

A: The standard reduction or oxidation potentials can be determined by using SHE, standard hydrogen…

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A: Write the half oxidation reaction

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A: The process of slowly eating away of the metal due to attack of the moisture and atmospheric gases…

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A: Given: Half reaction: Solution: Highest reduction potential=Cathode that undergoes reduction,MnO4…

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A: The elements which lie above H2O in EMF series or having higher half cell potential can be prepared…

Q: Complete and balance the following half-reaction in acidic solution NH_3(g)->NO_3(aq)

A: In the given reaction the ammonia is converted into nitrate ion: NH3g → NO3-aq

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: Write a balanced half-reaction describing the oxidation of solid iron to aqueous iron(II) cations.

A: a balanced half-reaction describing the oxidation of solid iron to aqueous iron(II) cations is as…

Q: Complete and balance this equation by the method of half-reaction.

A:

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

A: Answer  Electrolysis of NH44Cl

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Q: Write the half reaction for the anode and the cathode in the galvanic cell For Silver and Zinc

A: The concept of half reactions is used to describe what occurs in a electrochemical cell ,such as a…

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: Write a balanced half-reaction describing the oxidation of solid calcium to aqueous calcium cations.

A: Write a balanced half-reaction describing the oxidation of solid calcium to aqueous calcium cations.

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.