When 1.00 mole of chlorine gas is reduced to chloride ions in an electrolytic cell, what charge (in Coulombs) is passed through the electrochemical cell?

Q: When a galvanic cell operates long enough, we notice as the electrodes undergo physical changes.…

A: Answer - galvanic cell  - A galvanic cell or voltaic cell, respectively, is an electrochemical cell…

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

A:

Q: Electrolysis of an aqueous magnesium iodide solution at standard conditions would form the following…

A: Given,  Electrolysis of an aqueous magnesium iodide solution at standard conditions would form the…

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: explain why a galvanic cell can only work when the electrolyte solution remains electrically…

A: Galvanic cells also known as voltaic cells, are electrochemical cells in which spontaneous…

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: A voltaic cell was constructed using a zinc electrode (submerged in zinc sulfate), a copper…

A: Statement (d) is false as Cu will not released to copper sulfate solution.

Q: Question attached

A: Hello. Since the question contains multiple subparts, the first three subparts are solved. In case…

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: How many seconds are required to produce 8.00g of aluminum metal from the electrolysis of molten…

A: Assume that the required seconds as x. 1 A = 1 C/s. Coulombs generated by 12.0 A in x seconds is 12…

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

A: Given elements: strontium, gold, tin and chlorine To find: The elements which are prepared by the…

Q: electrochemical system, what is being described by the following? positive electrode A. electrolytic…

A: In an electrochemical system, 1) positive electrode - C. Cathode

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: The cathode is the electrode at which oxidation occurs. O True O False

A: We are authorised to call for the one question at a time. Please post the other question separately.

Q: What statement is true for a galvanic cell? Periodic Table and Datasheet Cations from the salt…

A: An electrochemical cell which produces electrical energy from chemical energy occurred during the…

Q: How many grams of aluminum can form by passing 305 Cthrough an electrolytic cell containing a molten…

A: The balanced half cell reaction is: Amount of current passed = 305 C Charge of 96485 C is carried…

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: Explain the process involve in Electrolysis.

A: There are some non-sponteneous redox reaction, that naturally does not occurr. To carry out those…

Q: What happens if you interchanged the assigned anode as cathode and the cathode as anode In terms of…

A: In electrochemical cell the electrical energy  is form by doing anodic oxidation and cathodic…

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: 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: Why must an electrochemical process involve a redox reaction?

A: Electrochemical process The process that is caused by applying electric current is called…

Q: Calculate the number of moles of electrons driven through an electrolytic cell with 3097 A of…

A:

Q: Which of the following is true for a galvanic cell?

A: Galvanic cells is also known as voltaic cells, they are electrochemical cells in which…

Q: in the electrolysis of water, does the reaction take place at a standard or non standard state?…

A:

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: Diagram an electrochemical cell indicating the anode, cathode, polarity of the electrodes, the half…

A: Redox reaction is a simultaneous reduction of one compound and oxidation of another compound.…

Q: Which of the following cell reactions would require the use of an inert electrode?

A: We have to tell which option is correct

Q: Identify those elements that can be prepared by electrolysisof their aqueous salts: strontium, gold,…

A: It is given that four elements strontium, gold, tin and chlorine are present, and which can be…

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

A: Given : the electrode is losing mass as the reaction is taking place.

Q: Identify those elements that can be prepared by electrolysisof their aqueous salts: copper, barium,…

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

Q: Does the oxidizing agent react at the anode or at the cathode in a galvanic cell?

A:

Q: Which of the following is the purpose of a salt bridge in an electrochemical cell? a. Stabilization…

A: Generally electrochemical cell is the device which is used to produce electric current through…

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

A: Redox reactions are the combination of reduction and oxidation reactions. The type of reaction in…

Q: Explain the working of the oxygen probe by referring to reactions that take place at the cathode and…

A: An oxygen sensor (or lambda sensor, where lambda refers to air–fuel equivalence ratio, usually…

Q: Where are electrons received and donated at in a galvanic cell?

A: In galvanic cell electrons are produced at anode and moving towards cathode or electrons are donated…

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

A: Answer  Electrolysis of NH44Cl

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: Calculate the number of moles of electrons driven through an electrolytic cell with 3503 A of…

A:

Q: Would you expect a mercury cell to give a constant voltage and why?

A: Yes, mercury cell provides a constant voltage throughout life. This is because there are no ions…

Q: During the electrolysis of a solution of Zn(NO3)2, 1.572 g of metal plated out at the cathode. How…

A: Given  Mass of Zn ( W )= 1.572 gram  Number of Coulombs ( Q )= ?

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.