an irregularly shaped metal part was made from a particular alloy was galvanized with zinc using a Zn(NO3)2 solution. When a current of 2.15 A was used, it took exactly 2.2 hours to deposit a 0.018-mm layer of zinc on the part. What was the total surface area of the part? The density of zinc is 7.410 g/cm^3. Assume the efficiency is 100%. Calculate your answer to at least 2 decimal places.

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

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

Q: A certain half-reaction has a standard reduction potential Ed=+0.42 V. An engineer proposes using…

A: The standard reduction potential of E°red = + 0.42 V is used as the cathode half-cell reaction of…

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

A: At cathode reduction takes place while at anode oxidation takes place.  Current (I) = 1.55 A  Time…

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

A:

Q: When a lead acid car battery is recharged by the alternator, it acts essentially as an electrolytic…

A:

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: Three electrochemical cells were connected in series so that the same quantity of electrical current…

A: Concept introduction: Faradays second law of electrolysis is explained as when the same quantity of…

Q: Chlorine, Cl2, is produced commercially by the electrolysis of aqueous sodium chloride. The anode…

A: Current =5.00×10^2A Mass of chlorine=4.18kg=(4.18×1000)g=4180g

Q: How long in seconds would it take to deposit 59.07 g of Pt from an aqueous solution of Pt 2+ with a…

A:

Q: A certain metal M forms a soluble nitrate salt MNO3. Suppose the left half cell of a galvanic cell…

A: left half cell concentration = 3.00MRight half cell concentration = 15mMTemperature T= C + 274 =…

Q: A certain metal M forms a soluble nitrate salt MNO3. Suppose the left half cell of a galvanic cell…

A:

Q: Electrolysis was performed to determine the identity of an unknown metal X. It was determined that 3…

A:

Q: A galvanic cell with a voltage of 1.3 V utilises the reaction: Zn + Cu2+ →→ Cu + Zn2+, as a source…

A: Given: The cell voltage is 1.3 V. The amount of Cu and Zn used is 6.3 g and 11 g, respectively.

Q: A certain half-reaction has a standard reduction potential Ered =-0.96 V. An engineer proposes using…

A:

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

A:

Q: A 215-mL sample of a 0.500 M NaCl solution with an initial pH of 7.00 is subjected to electrolysis.…

A: Gien: Volume of a sample = 215 mL NaCl = 0.500M pH = 7 After 15 minutes, Volume removed = 10 mL HCl…

Q: According to the reaction, Ag+ (aq) + e- --> Ag(s), silver is deposited. For 30.0 minutes, a 0.800A…

A:

Q: Consider these two entries from a fictional table of standard reduction potentials. X3+ + 3 e- »…

A:

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: 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 Cr3+1aq2 solution is electrolyzed, using a current of 7.60 A. What mass of Cr(s) is plated out…

A: Charge flowing per unit time is known as current which may be expressed mathematically as :…

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: When a lead acid car battery is recharged by the alternator, it acts essentially as an electrolytic…

A: Given data,Current=29.0ATime=69.0sReaction at cathode;Pb2++2e-→Pb(s)

Q: An electroplating solution contains vanadium (50.9415 g/mol), which is a metallic element that can…

A:

Q: A current of 2.90 A was applied to an electrolytic cell containing molten CdCl2 for 54 minutes.…

A: We have to calculate the mass of cadmium metal deposited when current passed is 2.90 A for 54…

Q: When lead acid car battery is recharged by the alternator, it acts essentially as an electrolytic…

A:

Q: Masakatsu plans to create counterfeit gold badges through electroplating. In a filled 500-mL tub, A…

A: Given: Current passed = 875 mA = 0.875 A                                 (Since 1 A = 1000 mA) And…

Q: Determine the molar mass (amu) of Metal (M) if it took 2.95 minutes for a current of 1.8 A to plate…

A:

Q: Aluminum(III) ion (Al 3+) is reduced to solid aluminum at an electrode. If a current of 2.75 amperes…

A:

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

A:

Q: How many grams of nickel metal can be plated from 1.00M NISO4(aq), using a current of 3.00 A for…

A: Here mass of metal is calculated by using faraday's law

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: An aqueous copper (II) chloride solution is electrolyzed for a period of 156 minutes. Using a…

A: We have given that  An aqueous copper (II) chloride solution is electrolyzed for a period of 156…

Q: A current of 4.05 A is passed through a Cu(NO3)2 solution for 1.70 h. How much copper is plated out…

A:

Q: When a lead acid car battery is recharged by the alternator, it acts essentially as an electrolytic…

A:

Q: Chromium can be plated from solution of CrCl3(aq) according to the following half reaction. How many…

A:

Q: When a lead acid car battery is recharged by the alternator, it acts essentially as an electrolytic…

A:

Q: An electrochemical cell is constructed by dipping a zinc rod in a solution of Zn(NO3)2(aq), dipping…

A: The equilibrium constant can be written as the ratio of concentration of products to the…

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

A:

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

Q: What constant current would be needed for a copper cathode to accumulate 3.06 g of copper in 30 min.…

A: given- mass = 3.06 g. time = 30 min = 30 x60 = 1800 sec electrochemical equivalent of copper = 3.29…

Q: A current 6.0 amperes is passed for 10 hours between copper electrodes in 800 ml of copper nitrate…

A: The charge carried by one electron is 96500 C. The electrode reaction: Given that current passed is…

Q: A certain half-reaction has a standard reduction potential Ered=+0.90 V. An engineer proposes using…

A: It is given that E°cell ≥ 0.70  E°cat = 0.90 V

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

A: Current I = 1.46 A  time t = 23.1 minutes = 23.1 * 60 s = 1386 s Mass of vanadium deposited = 0.534…

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.