What volume of chlorine gas at standard temperature and pressure is evolved when a solution of MgCl2 is electrolyzed using a current of 12.4 A for 1.0 h?

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: How long will it take to plate out 3.9 g Ni from aqueous Ni2+ with a current of 108.2 A? HOW DO WE…

A: To plate Ni using the process of electrolysis, the reaction that needs to be employed on the…

Q: How many minutes would be required to deposit 0.375g of calcium using a current of 3.93A?

A: Given,  Mass of Ca = w = 0.375 g  Current = I = 3.93 A  Time required = t = ?

Q: What mass of aluminum metal can be produced per hour in the electrolysis of a molten aluminum salt…

A: Faraday’s first law of electrolysis:                 The mass of the substance deposited at the…

Q: If the potential of a cell is 0.51 V at 25°C when [Zn2+(aq)]=0.111M and the pressure of the hydrogen…

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Q: How many seconds will be required to produce 1.00 g of nickel metal (58.693 g/mol) by the…

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Q: How long would it take to electroplate all the Zn^ 2+ in 0.280 L of .210 M ZnSO 4 solution with a…

A: The question is based on the concept of electrochemistry. It involves  application of first law of…

Q: How long will it take to plate out 3.0 g Ni from aqueous Ni2+ with a current of 113.1 A? HOW DO WE…

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Q: A current of 11.8 A is applied to 1.25 L of a solution of 0.549 mol L- aqueous HBr converting some…

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Q: 7. Determining volume of a gas by electrolysis. What volume of chlorine gas at standard temperature…

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: How much Ca will be produced in an electrolytic cell of molten CaCl2 if a current of 0.452 A is…

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Q: Manganese metal can be produced industrially by electrolysis of MnO2. How many hours would it take…

A: The compound of manganese electrolysed is MnO2 having Mn4+ ion. Hence the electrolysis reaction to…

Q: 5. Consider the following reactions: 3 Ni 2"taq) + 2Cr(OH)3 (s) + 10 OH ¯ (aq) → 3 Ni (s) + 2 CrO4…

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Q: What mass of chromium could be deposited by electrolysis of an aqueous solution of Cr2(SO4)3 for 143…

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Q: state and explain Faraday’s laws of electrolysis. What is Electrochemicalequivalent?

A: Faraday’s first law of electrolysis states that the mass of the substance accumulated or released at…

Q: In the commercial production of sodium metal by electrolysis, the cell operates at 7.0 V and a…

A: The faraday's first law explains that the quantity of any species deposited is directly proportional…

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: How long will an electrolytic cell containing a solution of cadmium(II) iodide need to run at a…

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Q: Given the standard cell potential for this cell is 0.115 V, and the measured cell potential is…

A: The standard reduction potential is measured under the following conditions as the 298 K…

Q: How long will it take to plate out 1.0 g Ni from aqueous Ni2+ with a current of 105.9 A? HOW DO WE…

A: Given: Mass of Ni to be plated out = 1.0 g. Current pass = 105.9 A.

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: Determine the current (in A) to produce 4.50 g Ag when Ag⁺(aq) is electrolyzed for 2.00 h. (F =…

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Q: a) In the electrolysis of aqueous NaNO2, how many liters of O2(g) (at STP) are generated by a…

A: Given data: Current = 67.8 A = 67.8 C/sec Time = 86.4 min = 86.4 x 60 sec Formula used: q = I x t

Q: Electrolysis of a solution of Zn(NO3)2 (aq) to give zinc metal is carried out using a current of…

A: The expression for the mass of metal deposited is given as:

Q: Calculate the mass of Li formed by electrolysis of molten LiCl by a current 6525 A flowing for a…

A: Given, Current = 6525 A or 6525 C/sTime = 50h = 50×3600 s = 180000seconds

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

A: It is given that MgCl2 is electrolysed and a current of 12.4 A is passed for 1h.

Q: Electrolysis of a solution of Zn(NO3)2(aq) to give zinc metal is carried out using a currentof 2.12…

A:

Q: Oxygen Supply in Submarines Nuclear submarines can stay under water nearly indefinitely because they…

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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 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: calculate the value of the electrode potential of hydrogen: a) in the 0.05 M solution of sulfuric…

A: a) Given : Concentration of sulfuric acid i.e H2SO4 = 0.05 M Since H2SO4 is a strong acid which will…

Q: How long ( hours) would it take to unload 0.433 moles of vibranium (Vb) metal during electrolysis of…

A: We have to calculate time needed for electrolysis  Molar mass of Tr not provided so only 1st…

Q: Over a period of time, the concentration of sulfuric acid in the lead storage battery of an…

A: Given data,Initial % by mass of H2SO4=38.0 %Final % by mass of H2SO4=26.0%Volume of H2SO4=734…

Q: What mass of aluminum metal can be produced per hour in the electrolysis of a molten aluminum salt…

A: The mass of aluminum metal calculated as follows

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: 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: Give the reason why it is necessary to use hydrogen as a standard to define the standard potential…

A: A standard electrode is an electrode used as a reference in electrochemical reactions and this…

Q: In an electroplating operation, the cell potential is sometimes 0 V. Why is zero potential possible…

A: In this question we need to illustrate the fact that cell potential for an electroplating cell can…

Q: 18. When pH = 7, p(O,) = 100 kPa, O, + 4H" + 4e calculate the electrode potential in according to…

A: 1 bar = 100 kPa [H+] = 10-pH = 10-7 M Nernst equation: EO2/H2O = EO2/H2O° -0.05914log1PO2×H+4…

Q: What mass of Sn(s) may be deposited from an aqueous SnCl, solution if a current of 2.50 A is applied…

A: Given,

Q: How long would it take to produce 3.6 g of platinum by passing a 2.0 ampere current through a…

A: The mass of the substance (m) deposited or liberated at any electrode is directly proportional to…

Q: what mass, in g, of copper will be deposited from a solution of Cu^2+ by a current of 2.43 A in 7.52…

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Q: In the electrolysis of water, how long will it take to produce 165.0 L of H2 at 1.0 atm and 273 K…

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Q: A current of 5.26 A is passed through a 2Sn(NO3)2 solution. How long, in hours, would this current…

A: In Sn(NO3)2 we have Sn in Sn2+ form  Hence to get tin that is Sn from Sn2+ the reaction will be Sn2+…

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

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

A: Given-> Current (I) = 1.48 ampere  Time (t) = 37.4 min = 37.5 × 60 second = 2250 seconds Weight…

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.