Zinc plating (galvanizing) is an important means of corrosion protection. Although the process is done customarily by dipping the object into molten zinc, the metal can also be electroplated from aqueous solution. How many grams of zinc can be deposited on a steel tank from ZnSO4 solution when a 0.755 A current flows for 2 days? Molar mass of zinc is 65.4 g/mol.

Q: An unknown metal M forms a soluble compound, M(NO3)3. A solution of M(NO3)3 is electrolyzed. When a…

A: The deposition is M+3 (aq) + 3e– ------> M (s)Number of moles of electrons = 3 × number of moles…

Q: How many seconds are required to deposit 0.274 grams of manganese metal from a solution that…

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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 metallic object to be plated with copper is placed in a solution of CuSO.. What mass of copper…

A: Given,  Current, I = 0.22 amp  Time, t = 1.5 hours               = 5400 sec  Molar mass of Cu =…

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

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Q: An aqueous solution of gold nitrate is electrolyzed with a current of 0.555 ampere until 1.32 g of…

A: The relationship between charge (q), time (t), and current (I) can be given as: q=I×t…

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: Electroplating is a way to coat a complex metal object with a very thin (and hence inexpensive)…

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Q: In the electrolysis of a 200 mL metal experiment, 0.0434 grams of cathode is applied when a current…

A: Given: weight of metal(w) = 0.0434  Current(I) = 0.50 A  Time(t) = 5 min = 300 sec  Valency factor =…

Q: Determine the molar mass (amu) of Metal (M) if it took 1.04 minutes for a current of 1.22 A to plate…

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

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Q: A laboratory was assigned the job of determining the copper(II) ion concentration in thousands of…

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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: To determine which electrode will be positive and the voltage that the voltmeter will show, we need…

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: 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: Electroplating is a way to coat a complex metal object with a very thin (and hence inexpensive)…

A: Mole is the amount of the substance that contains the same number of particles or atoms or…

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

A: Given: Current = 2.96 A Time = 33.4 min Mass of V deposited at cathode = 0.784 g Molar mass of V =…

Q: an irregularly shaped metal part was made from a particular alloy was galvanized with zinc using a…

A: Given The amount of current (I) is 2.15 A The time is 2.2 hours The density of zinc is 7.410 g/cm3…

Q: A proposed battery involves the reaction of Zn(s) and Cl2(g) to give ZnCl2. If you want such a…

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

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

A: As per the given information, this is basically concentration cell,where all the cell working due to…

Q: A steady current of 10 A maintained for 1 hr deposits 12.2 g of zinc at the cathode. What is the…

A: Given,  I = 10 A.  t = 1 hr.  m = 12.2 gm.

Q: Rhodium is a bright, hard, and highly reflective metal. It is most commonly used to plate white gold…

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Q: Electroplating is a way to coat a complex metal object with a very thin (and hence inexpensive)…

A: We have given that Current (I) = 240 mA = 0.24 A Time (t) = 55 sec Equivalent weight of silver =…

Q: Rhodium is a bright, hard, and highly reflective metal. It is most commonly used to plate white gold…

A: To find out the oxidation state, first find out the moles of e- and the moles of the rhodium. Then…

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: Metallic magnesium can be made by the electrolysis of molten MgCl2 What mass of Mg is formed by…

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Q: If a constant current of 115 A is applied for 15.0 hours to the plating of cobalt from a cobalt(III)…

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Q: How many seconds are required to deposit 0.128 grams of magnesium metal from a solution that…

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

A: Mass can be calculated as:-

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

A: Given ,

Q: Nickel can be produced when a current is passed through an aqueous solution of nickel (II) acetate.…

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Q: Determine the molar mass (amu) of Metal (M) if it took 1.29 minutes for a current of 1.48 A to plate…

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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: How many seconds are required to deposit 0.136 grams of copper metal from a solution that contains…

A: Given, mass of Cu deposited = 0.136 g Current passed = 0.913 A 1 Faraday is the magnitude of charge…

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: A current of 4.63 A4.63 A is passed through a Pb(NO3)2Pb(NO3)2 solution for 1.30 h1.30 h. How much…

A: Amount of substance deposited at electrode during electrolysis can be calculated as follows

Q: An electrolytic cell for depositing copper from copper sulfate solutions is placed in series with…

A: We use the formula below to find the weight of a metal(W) deposited in an electrode during…

Q: Giorno Giovanna likes golden stuff. However, since he is currently broke, he has to settle for…

A: According to electro-chemistry  W = zCt W= mass of Metal deposited in grams C= current  t = time in…

Q: How many seconds are required to deposit 0.177 grams of manganese metal from a solution that…

A: Approach to solving the question: Detailed explanation: Examples: Key references:

Q: Calculating standard reaction tree ing standard reduction potentials from the ALEKS Data tab,…

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Q: the intention of protecting the steel material (mainly Iron and other elements) of an industry,…

A: Given: Some electrode reduction potentials are: E°(Sn+2(aq) / Sn(s)) = -0.14 V E°(Zn+2(aq)/Zn(s)) =…

Q: Electroplating is a way to coat a complex metal object with a very thin (and hence inexpensive)…

A:

Q: many grams of cobalt metal will be deposited from a solution that contains Co2+ ions if a current of…

A: Given:  Current = 0.974 A  Time = 67.4 min = 67.4 x 60 = 4044 sec

Q: How long would it take to deposit 2.72 g of copper from an aqueous solution of copper II sulfate by…

A: Given that : Mass of copper to be deposited (w) = 2.72 g Current (i) = 2 amps

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.