(a) Metals may be coated or plated for a number of reasons – state three reasons. (b) In an electroplating operation, what volume (cm3 ) and weight (g) of zinc will be deposited onto a cathodic workpart if 10 A of current is applied for one hour? C = 4.75 x 10-2 mm3 /A-s, cathode efficiency E = 95%, density of zinc  = 7.15 g/cm3

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

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Q: impure

A: According to this law,  mass diposite on cathode is direactly proportion to the current.  So,…

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A:

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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: Question three on photo

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A:

Q: 4. Calculate the quantity indicated for each of the following electrolysis. a. The mass of Žn…

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Q: During an electrolysis process a current of 3.20 amperes was used for a period of 2 hours and 49…

A: The charge deposited is given by, Q=It where I is the current and t is the time.

Q: Calculate the quantity indicated for each of the following electrolysis. a. The mass of Zn deposited…

A: The mass of zinc can be calculated by using Faraday's law of electrolysis.

Q: How long will it take to plate 2.5 g of copper onto a light fixture using a solution of Cu(NO3)2 and…

A:

Q: It is desired to deposit 0.87 g of iron (MW = 55.85) from a FeCl3 solution by the passage of 2.5 A…

A: Given mass of of iron = 0.87 g MW for iron = 55.85 Current = 2.5 A Efficiency 85%

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A: We have to calculate the Faraday of electricity required and the time taken.

Q: A lead storage battery delivers a current of 6 A for one hour and 22 minutes at a voltage of 12 V.…

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Q: Gold can be plated out of a solution containing Au3+ according to the following half-reaction: Au 3+…

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Q: (a) How many minutes does it take to form 10.0 L of O₂ measured at 99.8 kPa and 28°C from water if a…

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Q: The electrolysis of AℓCℓ3 at high temperature produces aluminium metal. If a constant electrical…

A: Given:  Current (I) = 10 x 103 Amp  Time(t) = 1 hour = 3600 sec

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Q: Question attached

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

A: Given-> Current (I) = 2.99 ampere Weight of Ca= 23.5 gm

Q: An

A: We will calculate nfactor

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Q: A Zn Zn2 + Co 2+ Co  galvanic cell is constructed in which the standard cell potential is 0.48 V.…

A: Given: A galvanic cell :                    ZnZn2+Co2+Co                  E0cell = 0.48V = 0.48 JC-1…

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

A: Answer = 1268.9 min

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Q: Given the cell notation Pt /Cl2(g)/Cl¯(aq) // Zn+2(aq)/Zn. How long, in seconds, will it take for…

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Q: If a constant current of 7.3 amperes is passed through a cell containing Cu²+ for 1.5 hours, how…

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

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Q: A battery can provide a current of 3.80 A at 3.60 V for 8.00 hr. How much energy (in kJ) is…

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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: What mass of Molybdenum (Mo) could be deposited by electrolysis of an aqueous solution of Mo2(SO4)3…

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A:

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

A: Given: The amount of current passed through the solution for electrolysis is 1.44 A. The mass of Ca…

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.