Electrolysis of an aqueous solution of sodium chloride produces chlorine, Cl2 (9). The reaction that occurs at the anode is 2C1 (ag) → Cl, (9) + 2e- A constant electric current produces 137 g Cl2 in 46.2 min from an aqueous solution of sodium chloride. What is the current? Current = A

Q: A current of 4.21 A is passed through a N i ( N O 3 ) 2 solution. How long, in hours, would this…

A: Current (I) = 4.21 A  Mass of nickel deposited (m) = 4.50 g

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A: Write balanced half reaction of the given reaction---

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A: Given information:Current (I) = 6.4 ATime (t) = 69 minutes

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A: The balanced redox reaction involved:3 Cu(s) + BrO3–(aq) + 6 H+(aq) → 3 Cu2+(aq)  + Br–(aq) + 3…

Q: Chlorine, Cl2, is produced commercially by the electrolysis of aqueous sodium chloride. The anode…

A: Current =5.00×10^2A Mass of chlorine=4.18kg=(4.18×1000)g=4180g

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A: When electricity is passed through the electrolytic cell, then at the time the amount of substance…

Q: A current of 11.3 A is applied to 1.25 L of a solution of 0.552 M HBr converting some of the H+ to…

A: Equivalents of H+ ions reduced = QF=I×t96500=11.3 ×73 ×6096500= 0.513 Total equivalents of H+ ions…

Q: In the industrial "chlor-alkali" process, pure chlorine and sodium hydroxide are produced by…

A: The charge carried by 610A of current in 77 seconds is the product of current and time.q is the…

Q: your answer in the provided box. A constant current is passed through an electrolytic cell…

A: Given,produced volume of Cl2 gas at anode ( at STP ) = 4.18 Ltime taken = 16 h.

Q: Enter your answer in the provided box. A constant current is passed through an electrolytic cell…

A: Faraday's first law :-  The mass of the substance deposited at electrode is directly proportional to…

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: Enter your answer in the provided box. A constant current is passed through an electrolytic cell…

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Q: A constant current of 0.445 A is passed through an electrolytic cell containing molten BaCl2 for…

A: The reaction is, Ba2+ + 2e- ---> Ba(s) From this reaction, we can conclude that 2 mol of…

Q: n a copper plating experiment in which copper metal is deposited from a copper(II) ion solution, the…

A: Using Faraday's First of electrolysis: w = ZIt Z = Equivalent mass of metal96500w = Molar mass of Cu…

Q: Consider the electrochemical cell described by the following reaction at 310 K. The measured cell…

A: Given Cell potential is 0.242 V  E° CuI/I-/Cu= -0.17 V E° Cd 2+/Cd= -0.403V

Q: A galvanic cell is based on the following reaction(at 25°C)： Cu (aq)+Sn(s) → Cu(s)+Sn (aq) If the…

A: Note - The given reaction is incorrect. So, we will use the correct reaction for the question.   A…

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: 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.…

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Q: A current of 3.38 A3.38 A is passed through a Pb(NO3)2Pb(NO3)2 solution. How long, in hours, would…

A: Ans is 40.8min

Q: When an aqueous solution of potassium iodide is electrolyzed using platinum electrodes, the…

A: 8.15mA current flows which is equal to 0.00815A time is 12.6min = 756s The molar mass of I2 =…

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A: Given data,Current=29.0ATime=69.0sReaction at cathode;Pb2++2e-→Pb(s)

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Q: In the industrial "chlor-alkali" process, pure chlorine and sodium hydroxide are produced by…

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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…

A: Given ,

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Q: Enter your answer in the provided box. A constant current is passed through an electrolytic cell…

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Q: Write balanced half-reactions for the following redox reaction: 5 Ch(9)+2 Mn (aq)+16 OH (aq) → 10 CI…

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Q: 05 g Ru is produced at the cathode, what is the charge on the ruthenium ions in solution?

A: Dear student I have given answer to your question in the image format.

Q: An alternator recharges an automobile battery when the engine is running. If the alternator produces…

A: Given, Current produced by alternator = 1.540 A Engine operations requires = 1.179 A  mass of…

Q: Balance the following redox reaction when it occurs in acidic solution: 2+ Zn²+ (aq) + NH4+ (aq) →…

A: We have to balance the following redox reaction in acidic medium: Zn2+(aq) + NH4+(aq) --> Zn(s) +…

Q: When a lead acid car battery is recharged by the alternator, it acts essentially as an electrolytic…

A:

Q: In the industrial "chlor-alkali" process, pure chlorine and sodium hydroxide are produced by…

A:

Q: When a lead acid car battery is recharged by the alternator, it acts essentially as an electrolytic…

A:

Q: What is the amperage of a current if it takes 6.00 hours of the current passing through a 2.0 M…

A: The solution of the given question is

Q: In the industrial "chlor-alkali" process, pure chlorine and sodium hydroxide are produced by…

A:

Q: John set up a galvanic cell. The balanced redox reaction equation is Mg(s) + 2 Ag+ (aq) →Mg2+(aq) +…

A: emf of cell can be calculate by Nernst equation  Ecell = Eocell  - (0.0591/n ) log Q   ----(1)…

Q: A Cr+ (aq) solution is electrolyzed using a current of 7.30 A. What mass of Cr(s) is plated out…

A: a) Given: Current passed = 7.30 A. And time passed = 2.90 day = 2.90 × 24 × 60 × 60 = 250560 s…

Q: The electrolysis of a copper sulfate solution to get copper metal is carried out using a current of…

A: According to Faraday’s first law of electrolysis, the mass of the element deposited is directly…

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Q: 4. A galvanic cell consisting of a magnesium electrode and a standard hydrogen electrode is…

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Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2Cr³+ (aq) +…

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Q: A certain metal M forms a soluble sulfate salt MSO4. Suppose the left half cell of a galvanic cell…

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Q: Chlorine, Cl2, is produced commercially by the electrolysis of aqueous sodium chloride. The anode…

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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.