How long will it take to plate out each of the following with a current of 100.0 A?  1.0 kG Al from aqueous Al3+   (book answer: 30 hours) 1.0 g Ni from aqueous Ni2+     (book answer: 33 s)

Q: Using a library or the Internet, research a fuel cell that usesmethanol for fuel. What is the…

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Q: Which of the following statements is/are TRUE about standard electrode potentials? I. EO is measured…

A: To determine the true statements , we would use some facts about standard electrode potential (E°) .

Q: How much time in minutes would it take to deposit 1.74 grams of X (MW = 133.98 g/mol) on a cathode…

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Q: ctrolyzed by passing a current of 0.500 A through 1.00 L 22SO4 solution for 120 minutes. Determine…

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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: 1) Molten metal chloride (MC13) subjected to a current of 6.50 A for 0.388 hours deposits 1.41g of…

A: It is given that current = and time for which it flows Charge,

Q: Assume the specifications of a Ni-Cd voltaic cell include delivery of 0.46 A of current for 1.00 h.…

A: Oxidation takes place at anode.  So, metal will be eroded from anode.  Thus, minimum mass of anode…

Q: Answer the following question for marking • What is the effect of [KI]? • What is the effect of…

A: In this question, we have to find out the correct answer of given problem by the help of THE…

Q: A metallurgist wants to gold-plate a thin sheet with the following dimensions: 1.5in x 8.5in x…

A: first we have to find the volume,volume=length ×width×heightthen we know,density=massvolumeby…

Q: Assume the specifications of a Ni-Cd voltaic cell include delivery of 0.32 A of current for 1.00 h.…

A: Answer: According to the current value and time duration, charge required is…

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: How long would it take to reduce 1 mole of each of the following ions using the current indicated?…

A: Since you have posted question with multiple sub-parts, we are entitled to answer the first 3 only.…

Q: Assume the specifications of a Ni-Cd voltaic cell include delivery of 0.37 A of current for 1.00 h.…

A: Given I = 0.37 A t = 1 hr = 60*60 S Minimum mass of Cadmium = ? g

Q: Fischl, a scientist from Mondstadt specializing in electrochemistry, performed an electrolytic cell…

A: Given Amount of metal deposited = 15.73 g Current = 1.5 A Time = 5 hours n = 2

Q: 10

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Q: Copper is electroplated from CuSO4 solution. A constant current of 4.06 A is applied by an external…

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Q: How many milliliters of oxygen gas is generated from electrolysis of water performed at 25°C using a…

A: The balanced reaction taking place is given as, => 2 H2O (l) -------> 2 H2 (g) + O2 (g) Given:…

Q: A 1.00 g of metal sample took 31.05 minutes to be consumed in the anode to recharge a battery using…

A: According to Faraday's first law of electrolysis, the mass of a substance deposited on the electrode…

Q: current of 0.500 A flows through a cell containing Cd(II) for 10.0 minutes. Calculate the maximum…

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Q: What mass of copper could be deposited from a copper(II) sulfate solution using a current of0.50 A…

A: The given problem can be solved by using the formula as; Q=I×t…

Q: A sample of 25 mL prepared for an electrolysis experiment has a zinc concentration of approximately…

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Q: Show your work with tables 1 Amp means 1 C/1 sec 5 amp means 5C per 1 sec Faraday’s…

A: Given current is 15A.  Farady constant is given as 96,485 C.  Time for which the current is passed…

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: charge

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Q: How many grams of copper metal can be deposited from Cu²⁺(aq) when a current of 2.50 A is run for…

A: By using Faraday law, we can find mass of Cu deposited at respective electrode.   The following…

Q: A zinc-copper battery is constructed at follows at 25°C: Zn /  Zn2+(0.10M) // Cu2+(2.50 M) / Cu The…

A: Note: “Since you have posted a question with multiple sub-parts, we will solve the first three…

Q: Please help me with this. The lesson is all about Electrochemistry..   *If the standard reduction…

A: redox  process is process where oxidation and reduction occur simultaneously

Q: How long (in minutes) should a current of 6 amperes be applied through a solution of silver nitrate…

A: It is an application of Faraday  first law of electrolysis

Q: ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 1.39 minutes for a current…

A: According to the first law of Faraday, the mass of a metal deposited on the anode during…

Q: A current of 5.90 A is passed through a Sn(NO3)2 solution. How long, in hours, would this current…

A: The solution is having salt Sn(NO3)2 which contains ion Sn2+  Hence on passing the current, below…

Q: A battery can provide a current of 2.20 A at 1.40 V for 10.0 hr. How much energy (in kJ) is…

A: GIVEN: Current = 2.20 A Voltage = 1.40 V Time= 10.0 hr To CALCULATE: Energy (kJ)

Q: A certain half-reaction has a standard reduction potential E =+0.43 V. An engineer proposes using…

A: An electrochemical cell is one that converts chemical energy to electrical energy. The cell is…

Q: 13.72 A metallurgist wants to gold-plate a thin sheet with the following dimensions: 1.5 in x 8.5 in…

A: We have find out the answer.

Q: ) Show the equation and describes Faradays law which relates moles of analyte to charge in coulombs…

A: #(d): Faraday's first law describes the relation between the moles of the analyte deposited at the…

Q: One of the half-reactions is 2 N3- → N2 + 6 e How many faradays of electricity are required to…

A: For one mole of N2, 6 mole of electron or 6 Faraday electricity is required.

Q: If a water electrolysis cell operates at a current of 7.9 AA , how long will it take to generate…

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Q: A current of 0.80 A was applied to an electrolytic cell containing molten CdCl2 for 2.5 hours.…

A: Given: Current, i=0.80 A Time, t=2.5 hours Molar mass of cadmium=112.40 One Faraday=96,500 coulombs

Q: alculate the value of the faraday if electrolysis of a NaCl solution with a current of 1.60 A for a…

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Q: An electrolytic cell involving aluminium species is set up. The balanced reaction equation was…

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Q: current of 5.79 amps passes over 500 seconds in 300ml aqueous solution of CuSO4 copper…

A: Faraday's laws of electrolysis were proposed to solve such problems. According to the first law of…

Q: A constant current of 0.800 A was used to deposit copper at the cathode and oxygen at the anode of…

A: The half-reactions that will occur are as follows:

Q: During electrorefining of Cu from CUSO4, how much time (in hours) is needed to produce 250 g Cu on…

A: When a charge Q passes through a circuit the current through that circuit can be calculated by the…

Q: How many grams of copper metal can be deposited from Cu²⁺(aq) when a current of 2.50 A is run for…

A: Given data Time : t=1.45 hr Current : i=2.50 A Faraday constant : F=96500 C/mole Mass of Cu…

Q: How many grams of Ca metal (atomic mass = 40.08 g/mol) are produced by the electrolysis of CaBr,…

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Q: A 0.04 M sulfuric acid solution was electrolyzed using copper electrodes. A constant current of 3.36…

A: The reaction at cathode is: H+ + e-  → 1 2 H2 (g) 1F = 96485C electricity is required for 0.5 mol of…

Q: AG", rzn =-474 kJ/mol Electrode Half-Reaction Standard Reduction Cathode O2(9) + 4 H* (aq) + 4 e → 2…

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Q: 2. A spoon of surface area 20.0 cm² needs to be electroplated with silver to a thickness of 100 µm.…

A: The question has asked to calculate the time for which current will flow to deposit the required…

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

A: In this question, we have to find out the correct answer of given problem by the help of 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.