If an electrolysis plant operates its electrolytic cells at a total current of 150. A, how long, (in hours) will it take to produce 2.0 lbs of Mg(s) from seawater containing Mg2+? (1 faraday = 96,485 coulombs) %3D

Q: 7. A current of 1000. A flows for exactly 1 hour, through a cell in which the following reaction…

A: Electric current : It is defined as the rate at which a particular charge flows. It is represented…

Q: In the electrolysis of water, how long will it take to produce 95.00 L of H2 at 1.0 atm and 273 K…

A: Given Current = 249 mA Volume = 95 L Pressure = 1 atm Temperature = 273 K

Q: What mass of platinum could be plated on an electrode from the electrolysis of a Pt(NO3)2 solution…

A: Faradays first electrolysis Law states that the quantity of reaction taking place in terms of mass…

Q: 4. A metallurgist wants to gold-plate a thin sheet with the following dimensions: 1.5 in x 8.5 in x…

A: Given current = 7 A standard value  density of gold = 19.3 g/cm3

Q: A molten binary salt, Cal2, is electrolyzed. Write the half reactions that occur and identify which…

A: The binary salt given is CaI2  hence it has cation Ca2+ and anions I-

Q: Purification of copper can be achieved by electrorefining copper from an impure copper anode onto a…

A: Answer :- 337.7 h The time take to plate 14.0 kg of Cu onto the cathode when 35.0 A current passed…

Q: In an electrolysis of a solution containing Ni2+ (aq), metallic Ni(s) deposits on the cathode. Using…

A: (a) Current is the amount of charge flowing per unit time. If I is the current(in A) andt is 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: In the electrolysis of aqueous NaCl, how many grams of Cl2 are generated by a current of 4.65…

A: Question is based on first law Faraday's law of electrolytes. i.e., amount of substance deposited is…

Q: An electrolytic cell consists of a pair of inert metallic electrodes in a solution buffered to pH =…

A: Part a: The electrolytic cell consists of two electrodes, anode and cathode. Oxidation occurs at…

Q: If a water electrolysis cell operates at a current of 7.8 A, how longwill it take to generate 25.0 L…

A:

Q: Aluminum metal can be made from aluminum ions by electrolysis. What is the half-reaction at the…

A:

Q: Calculate the equilibrium constant, Keq, for each electrochemical cell given the following…

A: The equilibrium constant Keq can be calculated from the change in Gibb's free energy (∆G0) of the…

Q: A battery can provide a current of 2.20 A at 1.00 V for 8.00 hr. How much energy (in kJ) is…

A: Given information,Battery provides a current 2.20 A at 1.00 V for 8.00 hr.Calculate the power,

Q: a current of 5.79 A is passed over 500 seconds in 300 ml of aqueous solution of copper sulphate…

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

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: Copper can be electroplated at the cathode of an electrolysis cell by the half-reaction.…

A: In this question, we want to determine the time in second would it take for 320mg of copper metal…

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

A:

Q: A. Given that the electrochemical cell L gives a potential of 0.0570 V, determine the concentration…

A: A. Given a concentration cell L, in which the concentration of bromide ion in the anode is given to…

Q: In the electrolysis of aqueous NaCl, how many grams of Cl2 are generated by a current of 3.10…

A: Formation of Cl2 from NaCl is shown below,

Q: An electrochemical cell is made of theoretical metals Ma/Ma2+ and Mb/Mb2+. If the reduction…

A: Cell A: Ma/Ma2+       Ereduction= -0.19 V   Cell B: Mb/Mb2+        Ereduction = -0.85 V

Q: A solution of NaCl is neutral, with an expected PH of 7. If electrolysis was carried out on 500 mL…

A:

Q: A battery can provide a current of 2.40 A at 2.60 V for 4.50 hr. How much energy (in kJ) is…

A: Answer: If I Ampere current is generated by a battery for t seconds when it is operating at V…

Q: Calculate the amount of time it would take to collect 0.750L of hydrogen gas at the cathode of an…

A: Answer = 309 minutes

Q: Aluminum metal can be made from aluminum(III) ions by electrolysis. What is the half-reaction at the…

A:

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: Purification of copper can be achieved by electrorefining copper from an impure copper anode onto a…

A: Given that :  Mass of copper deposited = 18.5kg = 18.5kg×1000g/kg = 18500g  Current(I) = 40.5A =…

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: ) 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: In the electrolysis of aqueous NaCl, how many grams of Cl2 are generated by a current of 2.35…

A: moles of electrons  =6.2x1018 x2.35x140x60/6.022x1023 =20454 x 10-5 =0.2 Moles of electron = number…

Q: Question attached

A: Given that: ECell=0.64 VEoPb2+/Pbs=−0.1263 VPb2+=0.010 MVO2+=0.10 MV3+=1.0×10−5 M Cathode:…

Q: 6. Zinc (Zn) can be purified by the electrolysis of aqueous zinc sulfate. Suppose an electrolytic…

A: Given that, In the electrolytic cell : Molarity of ZnSO4 solution = 0.050 M Weight of zinc deposited…

Q: Enter your answer in the provided box. Copper is purified by electrolysis. A 4.75-kg anode is used…

A: Given:  Mass of anode = 4.75 kg = 4750 gm  Current (I) = 37.8 A

Q: 7. A current of 1000. A flows for exactly 1 hour, through a cell in which the following reaction…

A:

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: What mass of material will be deposited at the cathode when a current of 10.5 A is applied for 2.0…

A:

Q: The following figure represents an electrochemical cell at 25.00C with aqueous solutions that behave…

A:

Q: How long would it take to deposit 7.54 g of copper (molar mass 63.55 g/mol) at the cathode of an…

A: current = 15.9 A  (given) Molar mass of copper = 63.55 g/mol   (given) Cu is having n factor of 2…

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…

A: Given that a current of 3.80 A was provided by battery at 3.60 V. The power can be calculated as…

Q: In an electrolysis of a solution containing Ni2+ (aq), metallic Ni(s) deposits on the cathode. Using…

A: Given,  Current in ampere = I =  0.150 A  Electrolysis of Ni2+ (aq) ion  Time period in minutes = t…

Q: Consider the following electrochemical cell (battery): Mg(s) | Mg²“(aq) | Cr (aq) | Cl2 (g) | Pt(s)…

A: SOLUTION: Step 1: Given, Mg (s) │Mg2+(aq) ││Cl- (aq)│Cl2(g) │Pt(s) (a). In an electrochemical cell,…

Q: 5. How long would it take to deposit 15.0 g copper metal at the cathode of an electrolysis cell…

A: In this question, we want to determine the time taken for deposit 15.0g of Cu metal on Cathode.  You…

Q: 8) Consider the galvanic cell constructed with the following materials Zn electro Zn(NO3)2(aq), Fe…

A:

Q: Suppose the galvanic cell sketched below is powered by the following reaction: Cu(s)+2 A£NO3(aq) →…

A: Given thatthe cell reaction that takes place in the Galvanic cell is given by Cu(s)   + 2AgNO3(aq) →…

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…

A:

Q: 2. A galvanic cell consists of a lead anode immersed in a 1.00 M solution of Pb(NO3)2 and a platinum…

A:

Q: How many grams of copper are deposited on the cathode of an electrolytic cell if an electric current…

A: Faraday's law of electrolysisAsW= Ite/FF= 965900 Ct=20 x 60 sece for copper if taken in copper…

Q: 4. An electrolysis cell that deposits gold (from Au*(aq) operates for 15 minutes at a current of…

A:

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.