In the electrolysis of water, how long will it take to produce 125.0 L of H2 at 1.0 atm and 273 K using an electrolytic cell through which the current is 158.0 mA?

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

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Q: What volumes of H2 (g) and O2 (g) at STP are produced from the electrolysis of water by a current of…

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Q: Magnesium metal can be produced industrially by electrolysis of MgCl2. What mass of magnesium metal,…

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Q: A current of 12.0 A is passed through molten magnesium chloride for 14.0 h. How many moles of…

A: Given: Current = 12.0 A Time = 14.0 h

Q: What volumes of H2(g) and O2(g) at STP are produced from the electrolysis of water by a current of…

A: Amount of charge (Q) = I . t  where I = current and t = time

Q: A 5.77 g of zinc is deposited at the cathode when a current of 7.1 amperes passes through an…

A: Given : Current = 7.1 A And time = 40 min = 40 X 60 = 2400 s…

Q: In the electrolysis of water, how long will it take to produce 95.00 L of H2 at 1.0 atm and 273 K…

A: Given Current = 249 mA Volume = 95 L Pressure = 1 atm Temperature = 273 K

Q: In the electrolysis of water, how long will it take to produce 155.0Lof H2 at 1.0 atm and 273 K…

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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: A constant current of 0.912 A is passed through an electrolytic cell containing molten MgCl2 for…

A: According to the Faraday's first law of electrolysis, the amount of any substance deposited at the…

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

A:

Q: Calculate the mass of cobalt plated onto the cathode of an electrolytic cell by a current of 15.0 A…

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Q: Electrolysis of an NaCl solution with a current of 2.00 A for a period of 200 s produced 59.6 mL of…

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Q: Copper is plated onto the cathode of an electrolytic cell containing CuCl2(aq). How long does it…

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Q: Molten CaCl2 can be electrolyzed to form metallic Ca. For what duration should an electrolysis be…

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Q: An aqueous solution of a platinum salt is electrolyzed for 1.00 hour using a current of 1.50 A to…

A: According to Faraday's law when a solution of an element is electrolysed then it will deposited.…

Q: What volume of chlorine gas at standard temperature and pressure is evolved when a solution of MgCl2…

A: Provided time=1hour Molar mass of Cl2=70.906g/mol Let w gram Cl2 evolve So provided time…

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: Consider the galvanic cell. In a certain experiment, the emf () of the cell is found to be Q.54 V at…

A: Solution :    Nernst equation is used to calculate the potential of the cell at non-standard…

Q: Molten CaCl₂ can be electrolyzed to form metallic Ca. For what duration should an electrolysis be…

A: For CaCl2 , the given data is- Current(I) = 2.06A Mass of Ca = 29.3g Atomic mass of Ca = 40.078 g…

Q: How long, in minutes, will it take to produce 370.0 g of pure lithium by running a current of 330 A…

A: Given, Current passing = 330 A Mass of Li = 370.0 g  Molar mass of Li = 6.94 g/mol

Q: Determining volume of a gas by electrolysis. What volume of chlorine gas at standard temperature and…

A: Given information: Current = 12.4 A Time = 1.0 h Charge flown:  Q = It= 12.4×60×60= 44640 C For the…

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 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: What volumes of H2(g) and O2(g) at STP are produced from the electrolysis of water by a current of…

A: According to Faraday's 1st law weight of the substance from in each electrolyte  W = ZIt where , W…

Q: In the electrolysis of water, how long will it take to produce 225.0 L of H2 at 1.0 atm and 273 K…

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Q: How many moles of hydroxide ion will be produced at the cathode during the electrolysis of water…

A: The given cathode reaction is: 2H2O + 2e- → H2 + 2OH- The balanced equation shows that for every 2…

Q: In the electrolysis of water, how long will it take to produce 200.0 L of H2 at 1.0 atm and 273 K…

A: Current = 161.0 mA = 0.161 A Volume = 200.0 L Pressure = 1 atm Temperature = 273 K

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: Molten CaCl2 can be electrolyzed to form metallic Ca. For what duration should an electrolysis be…

A: Answer = 1268.9 min

Q: What volumes of H2(g) and O2(g) at STP are produced from the electrolysis of water by a current of…

A: Using farday's law of electrolysis we can solve this problem.

Q: In the electrolysis of water, how long will it take to produce 1.00 × 102 L of H2 at STP (273 K and…

A: During the electrolysis of water, H2 molecules are produced at cathode. Number of moles of H2…

Q: An unstirred solution of 2.00 M NaCl was electrolyzed for a period of 28.9 min and then titrated…

A: Concentration of NaCl = 2M Time duration of electrolysis = 28.9min Concentration of HCl = 0.314M…

Q: Molten CaCl2 can be electrolyzed to form metallic Ca. For what duration should an electrolysis be…

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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.