A technician is plating a faucet with 1.26 g of Cr from an electrolytic bath containing aqueous Cr2(SO4)3.  If 18.5 min is allowed for the plating, what current is needed? Faraday's constant = 96, 485 C/mol . Molar mass Ni = 51.9961 g/mol     Group of answer choices 2.10A 1.36A 3.16A 6.31A

Q: A galvanic cell is constructed with a copper electrode dipping into a 0.023 M solution of Cu2+ ions,…

A: Given that, Galvanic cell constructed with to half cells  Cu/Cu2+ is one electrode and Mg/Mg2+ is…

Q: Determine the molar mass (amu) of Metal (M) if it took 1.68 minutes for a current of 1.08 A to plate…

A: The metal will come out as M3++3e-= M . We can conclude from here that 3 moles of electrons are…

Q: 3. A technician is plating a faucet with 1.26 g of Cr from an electrolytic bath containing aqueous…

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Q: For the following half-reactions: Cr3-(aq) – Cr(s) Zn2«(aq) → Zn(s) a. What will be the overall…

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Q: The batteries used in automobiles are rechargeable and consist of Pb and PbO2 anodes and cathodes…

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Q: Chrome is plated from solutions of chromium (III) chloride. If a current of 4.57 A is passed through…

A: Given that: Mass of chromium deposited = 14.5 g Amount of current passed through solution = 4.57 A…

Q: Suppose a current of 690 mA is passed through an electroplating cell with an aqueous solution of…

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Q: Perchlorate is a serious problem in drinking water as it interfere with the functioning of thyroid…

A: Given information: Concentration of NaClO4 = 1.0*10-4 M Cell potential = -0.146 V After transferring…

Q: (a) One method to reduce the concentration of unwanted Fe3+(aq) in a                 solution of…

A: The half-reactions are oxidation or reduction reactions, which is useful in balancing redox…

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

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Q: 6. A 1M aqueous solution of chromium (I) bromide will be electrolyzed to "chrome plate" a faucet.…

A: As per the Faraday's 1st law of electrolysis: w=ZIt      ----(1)where,w = weight of the substance…

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 baby's spoon with an area of 6.25cm2 is plated with silver from a silver nitrate solution using a…

A: Calculation of Charge: Q=I×t                                 ...... (1)    where Q=charge, I =…

Q: 10

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Q: A common car battery consists of six identical cells each of which carries out the reaction:…

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Q: (a) How many moles of mercury will be produced by electrolysing 1.0 M Hg(N03)2 solution with a…

A: The quantity of charge passed is calculated as follows,                               Q=I×t Where,…

Q: Tin-plated steel is used for “tin” cans. Suppose that in the production of sheets of tin-plated…

A: Given: Current passed = 100.0 A. Time taken = 8 hours = 8 × 60 × 60 = 28800 s…

Q: What is the standard potential (E°) for the reaction below? Use the standard potentials in the Data…

A: Cathode :-  The electrode at which reduction reaction takes place is known as cathode Anode :-  The…

Q: Determine the molecular mass and identity of a +2 metal, X, that plates 46.3g of X in 6.75 hours at…

A: Note: As per our guidelines, we are supposed to answer only the first question (i.e. question number…

Q: How many minutes does it take to plate 164.8g of chromium onto a car part using 16.75 A of current…

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Q: Suppose a galvanic cell is established using the following cell reaction. Cu (s) + 2Ag^1 (0.100 M)…

A: Given the cell reaction is: Cu(s) + 2Ag+(aq) (0.100 M)  <-----> Cu2+(aq) (0.200 M) + 2Ag(s)…

Q: How long will it take to plate out 1.9 g Ni from aqueous Ni2+ with a current of 114.4 A? WHERE ARE…

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Q: A metal was galvanized with zinc using a solution of zinc nitrate, Zn(NO3)2. How much time was…

A: Answer :  We have to calculate time to plate zinc on the metal . Using Faraday laws of electrolysis…

Q: A galvanic cell using Mg|Mg2+ and Cu|Cu2+ half-cells operates under standard-state conditions at…

A: Given: Time passed = 31.5 hr = 31.5 × 3600 = 113400 s                             (Since 1 hr = 3600…

Q: What is the standard potential (E°) for the reaction below? Use the standard potentials in the Data…

A:

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

A: Given: Time = 3.3 hours Current = 17.8 A Atomic mass of copper = 63.5 g/mol

Q: In an electrolytic cell, silver is deposited at the cathode when a current of 2.75 A is passed for…

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Q: 4. What current is required to deposit on the cathode 5.00 g gold/h from a solution containing a…

A: Current = Charge/Time  Q = I/t  1F =96500 C/mol  Mass of 1 mole =Molar mass

Q: How many grams of chromium metal are plated out when a constant current of 8.00 A is passed through…

A: We have, Cr3+ needs 3 Faradays to plate 1 mole This means that for every 3 moles of electron…

Q: A galvanic cell using Mg / Mg*" and Cu / Cu" half-cells operates under standard-state conditions at…

A: Cell delivers = 0.31 A or 0.31 C/sec In 1 sec charges delivered = 0.31 C  32.1 hr = 3600 sec × 32.1…

Q: How many amperes of current needs to be passed through molten Sodium chloride (NaCl) to produce 2.1…

A: We have given that during the electrolysis of molten Sodium chloride 2.1 g of Sodium is produced at…

Q: galvanic cell is made using 0.25M ZnSO4 and an unknown amount of CuSO4. The cell potential is 105V…

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Q: How long will it take to plate out 1.2 g Ni from aqueous Ni2+ with a current of 112.4 A? WHERE ARE…

A: Given,   1.2 g Ni plate out from aq Ni2+ with a current of 112.4 A

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

A:

Q: At 25C and pH 7, a solution containing compound A and its reduced form AH2 has standard electrode…

A: (i) The standard potentials are given for A and B which can be represented as;   A+2H++2e-→AH2…

Q: A baby's spoon with an area of 6.25cm2 is plated with silver from a silver nitrate solution using a…

A: Given: Area = 6.25 cm2Current = 2.00 ATime = 2 hours 25 minutesCurrent efficiency = 82% Density of…

Q: Weighing a copper atom in an electrolysis experiment. A standard experiment involves passing a…

A: Electrolysis is the process through which electrical energy is converted into the chemical energy…

Q: Calculate the standard free energy, ∆G°, for a galvanic cell represented by the following notation:…

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Q: Cr3+(aq) → Cr(s) Zn2+(aq) → Zn(s) a. What will be the overall balanced reaction if you want to make…

A: The answer is discussed below, Oxidation occurs at the anode and reduction occurs at the cathode.

Q: decided to deposit 55.00 g of gold over an iron medallion by electroplating it from a solution…

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Q: Consider these two entries from a fictional table of standard reduction potentials.…

A: X3+ +3e- ⟶ X(s) , Eo =−1.63 V (anode) Y3+ +3e−⟶Y(s), Eo =−0.41 V (cathode)

Q: (c) For the electrochemical cell: Cd (s) / Cd Cl2 (aq, 0.0538 M) // Ag NO, (aq, 0.0320M) / Ag (s) i)…

A:

Q: Consider these two entries from a fictional table of standard reduction potentials. X3++3e−⟶X(s)…

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Q: A galvanic cell is constructed with a copper electrode dipping into a 0.023 M solution of Cu²+ ions,…

A: Given, Ecell= 2.86V at 25oC[Cu2+]=0.023MMg(s)   +  Cu2+(aq) → Mg2+(aq)  +  Cu(s)Since we know that…

Q: Cr3+(aq) → Cr(s) Zn2+(aq) → Zn(s) a. What will be the overall balanced reaction if you want to…

A: The two half reactions are as follows: The oxidation half reaction is, Zn(s)------>Zn2+(aq) +2 e-…

Q: How many minutes would be required to electroplate 20 g of chromium (52.00 g/mol) by passing a…

A: Let t be the time required in seconds than total charge passed in t seconds = current in ampere…

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…

Q: 1) What is measured in Volts? a) how many electrons are passing through a system b) how many…

A: "To get remaining sub-parts solved please repost the complete question and mention the sub-parts to…

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.