A 5.77 g of zinc is deposited at the cathode when a current of 7.1 amperes passes through an electrolytic cell for 40.0 minutes. What is the oxidation state of the zinc in the aqueous solution?

Q: 5) A certain electrochemical cell has a cell potential of +0.12 V. Which of the following is a true…

A: Electrochemical cell or galvanic cell converts chemical energy into electrical energy. In galvanic…

Q: How many moles of oxygen, O2, will be produced by the electrolysis of water with a current of 1.5…

A:

Q: A current of 10.0 amperes flows for 2.00 hours through an electrolytic cell containing a molten salt…

A: According to the reaction given, we have  Xn+ (aq) + ne-→X (s) t=2 hours=7200 sec (since 1 hr =3600…

Q: A constant current of 1.6 A is used to precipitate copper at the cathode and oxygen at the anode of…

A: value of constant current = 1.6 A Time = 30.4 minutes cathode - copper Anode - oxygen

Q: An electrolytic cell contans 50.0 mL of a 0.152 M solution of FeCl3. A current of 0.775 A is passed…

A:

Q: one process used for electroplating silver, a current of 10.23 A was passed through an electrolytic…

A: Electroplating is a process in which a thin layer of one metal is deposited on another metal surface…

Q: An aqueous solution of gold nitrate is electrolyzed with a current of 0.555 ampere until 1.32 g of…

A: The relationship between charge (q), time (t), and current (I) can be given as: q=I×t…

Q: How many moles of oxygen, O 2, will be produced by the electrolysis of water with a current of 1.5…

A:

Q: Consider an electrolytic cell where silver metal is plated (reduced) from an  aqueous silver nitrate…

A:

Q: A 215-mL sample of a 0.500 M NaCl solution with an initial pH of 7.00 is subjected to electrolysis.…

A: Gien: Volume of a sample = 215 mL NaCl = 0.500M pH = 7 After 15 minutes, Volume removed = 10 mL HCl…

Q: In an electrolytic cell, two inert carbon electrodes were immersed in an aqueous solution of tin…

A:

Q: Rhodium is a bright, hard, and highly reflective metal. It is most commonly used to plate white gold…

A:

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

A: Use the first law of Faraday.

Q: Rhodium is a bright, hard, and highly reflective metal. It is most commonly used to plate white gold…

A: To find out the oxidation state, first find out the moles of e- and the moles of the rhodium. Then…

Q: 3.53 L of 0.362 M  solution are electrolyzed (Cu is plated out of solution as metal.) A current of…

A: NOTE: Assuming that the solution contains Cu2+ ions and the concentration data given is for the Cu2+…

Q: An electrochemical cell is constructed in which the silver ions in silver chloride are reduced to…

A: Given,  A current of 0.500 A is passed through the cell for 101 minutes. The mass of copper metal…

Q: In one process used for electroplating silver, a current of 10.23 A was passed through an…

A: Dear student, this question is related to electroplating process.

Q: Tin-plated steel is used for "tin" cans. Suppose that in the production of sheets of tin-plated…

A:

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

A:

Q: What mass (in grams) of nickel could be electroplated from a solution of nickel(II) chloride by a…

A: From Faraday's first law of electrolysis, the weight of a chemical substance(w) deposited at an…

Q: A solution containing vanadium (chemical symbol V) in an unknown oxcidation state was electrolyzed…

A:

Q: An aqueous copper (II) chloride solution is electrolyzed for a period of 156 minutes. Using a…

A: We have given that  An aqueous copper (II) chloride solution is electrolyzed for a period of 156…

Q: A galvanic cell is set-up in the laboratory with a copper anode and an unidentified cathode. Your…

A:

Q: A current of 0.46 A was passed through a copper (II) sulfate solution using copper electrodes for 16…

A: According to faraday law of Electrolysis:

Q: A 220 mL sample of a 0.500 M NaCl solution with an initial pH of 7.00 is subjected to electrolysis.…

A:

Q: A solution containing vanadium (chemical symbol V) in an unknown oxidation state was electrolyzed…

A: Current I = 1.46 A  time t = 23.1 minutes = 23.1 * 60 s = 1386 s Mass of vanadium deposited = 0.534…

Q: A 0.1 M aqueous CaCl, solution is electrolyzed by usina inert electrodes. If 1.25 ampere current is…

A: At cathode this reaction is taking place,Ca2+  +  2e-   →  Ca  Calculate the charge first,Q = it and…

Q: A constant current of 0.800 A was used to deposit copper at the cathode and oxygen at the anode of…

A: The half-reactions that will occur are as follows:

Q: A galvanic cell is set-up in the laboratory with a copper anode and an unidentified cathode. Your…

A:

Q: A copper rod was purified by using it as the anode in the electrolysis of a 1.0 M copper II)…

A:

Q: Faraday constant. Suppose that after the electroplating was complete, you wiped the cathode copper…

A: Explanation to the correct answer is given below

Q: A solution containing vanadium (chemical symbol V) in an unknown oxidation state was electrolyzed…

A:

Q: A galvanic (voltaic) cell contains a copper cathode immersed in a copper(II) chloride solution and a…

A: In this question, we have to find out the correct answer of given problem by the help of the…

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.