What volumes of H₂(g) and O₂(g) at STP are produced from the electrolysis of water by a current of 2.58 A in 15.5 min? L H₂(g) 0₂(g) L

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: How many hours are required to produce 115 g of Iron metal from the electrolysis of molten FeCl3…

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Q: A molten sample of CuCl2 is electrolyzed for 2.0 days at a current of 15.0 amps. How many grams of…

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Q: A constant current is passed through an electrolytic cell containing molten MgCl2 for 12 hours. If…

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Q: An electrolysis cell is set up with the cathode producing H₂ gas and with an unknown metal at the…

A: Electrolysis Electrolysis involves passing an electric current through either a molten salt or an…

Q: Metallic Magnesium can be made by the electrolysis of Molten MgCl2. What mass of Mg is formed by…

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

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Q: In the electrolysis of aqueous NaCl, how many grams of Cl2 are generated by a current of 4.65…

A: Question is based on first law Faraday's law of electrolytes. i.e., amount of substance deposited is…

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

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Q: What mass of chromium could be deposited by electrolysis of an aqueous solution of Cr2(SO4)3 for 171…

A: Time = 171 minutes  Current = 15.0 amperes  Chromium deposited during the process of electrolysis =…

Q: A certain metal M forms a soluble nitrate salt MNO3. Suppose the left half cell of a galvanic cell…

A: Given,  Concentration of MNO3 in left half = 22.5 mM  Concentration of MNO3 in right half = 4.50 M…

Q: A steady current was passed through molten CoSO. until 2.35 g of metallic cobalt was produced.…

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Q: A current of 5.25 A is passed through an aqueous solution of copper(II) nitrate for 71.0 min. How…

A: An swer:- this question is answered by using the simple concept of calculation of mass of a metal…

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: 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: Aluminum(III) ion (Al 3+) is reduced to solid aluminum at an electrode. If a current of 2.75 amperes…

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Q: A certain metal M forms a soluble nitrate salt MNO3. Suppose the left half cell of a galvanic cell…

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Q: What volumes of H3(g) and O,(g) at STP are produced from the electrolysis of water by a current of…

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

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

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Q: If a 30.0 A of current flow through an electrolytic cell containing molten aluminum oxide for 1.0…

A: The chemical reaction :  Al3+(l) + 3e- ---> Al(s)  Current = 30.0 A  Time = 1.0 hour  Weight of…

Q: Calculate the number of grams of aluminum produced in one hour by the electrolysis of molten…

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Q: In the electrolysis of aqueous NaCl, how many grams of Cl2 are generated by a current of 2.35…

A: moles of electrons  =6.2x1018 x2.35x140x60/6.022x1023 =20454 x 10-5 =0.2 Moles of electron = number…

Q: ) In the electrolysis of a 200 mL unknown metal solution, 0.0434 grams of cathode mass increases…

A: We have given that  Volume of solution = 200mL  Mass deposited at cathode = 0.0434g  Current = I =…

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: Che identity of the

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Q: Aluminum is produced commercially by the electrolysis of Al, 03 in the presence of a molten salt. If…

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Q: Aluminum is produced commercially by the electrolysis of Al203 in the presence of a molten salt. If…

A: Total current, I = 1.09 million Ampere                           = 1.09×106 Ampere Time, t = 3 hr…

Q: A factory wants to produce 1.00 x 103 kg barium from the electrolysis of molten barium chloride.…

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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: What period of time (in hours) is required to produce 1.00mol of chlorine using a current of 5.00A?

A: A numerical problem based on Faraday's law, which is to be accomplished.

Q: Suppose that a machine part requires 400 mg of copper to provide a coating that is thick enough for…

A: Given data,Current=0.5ATime=10min=10×60s=600s

Q: 7. How many grams of aluminum metal (26.982 g/mol) can be produced by the electrolysis of Al2O3…

A: In Al2O3, the oxidation number of Al is +3 and that of O is -2.  Hence uring electrolysis of Al2O3,…

Q: Calcium metal is obtained by direct electrolysis of molten CaCl2. If a metallurgical electrolysis…

A: Calcium metal is obtained by direct electrolysis of molten CaCl2. If a metallurgical electrolysis…

Q: Calculate the mass of chlorine in grams that can be produced by the electrolysis of 50.0 kg of…

A: The electrolysis of sodium chloride takes place as follows: 2NaCl(aq) + 2H2O(l) → 2NaOH(aq)+ Cl2(g)+…

Q: Gold (atomic mass = 197.0) is plated from a solution of chloroauric acid, HAuCl4; it deposits on the…

A: Given: Mass of god produced = 0.34 g. Current passed = 0.10 A

Q: A certain metal M forms a soluble nitrate salt MNO33 . Suppose the left half cell of a galvanic cell…

A: In this case both side same solution is present so it is a concentration cell and for concentration…

Q: Mass =

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Q: Copper metal (63.55 g/mol) is purified by electrolysis. How much copper metal (in grams) could be…

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Q: In the electrolysis of a sodium chloride solution, what volume of Ch (g) is produced in the same…

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

A: The two half-cells differ only in the concentration of electrolyte. Therefore, the given cell is a…

Q: What volume of Oxygen at STP can be produced by the electrolysis of 20.0 g water?…

A: Balanced chemical equation for electrolysis of water is given by 2 H2O (l) → 2 H2 (g) + O2 (g) Mass…

Q: A factory wants to produce 1.0 x 10³ kg Barium from the electrolysis of molten barium chloride. What…

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

A: Given, Current through cell (I) = 2.40 A Time (t) = 2.81 h = 2.81 x 60 x 60 sec = 10116 sec 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.