A small part with a surface area of 2.62 cm2 is plated with a gold coating that is 5.00  10–4 mm thick. The density of gold is 19.32 g cm–3. (a) What mass of gold is in this coating? (b) If a barrel plating run has 5,000 of these parts in a single barrel, how long would the run take if the current was 15.0 A? (Gold is effectively plated from Au+(aq).)

Q: 6b. How long does it take to deposit a coating of gold 1.00 picometers thick on a disk-shaped…

A:

Q: When 0.60 A of electric current is passed through a 15.0 mL solution of permanganate ions for 11.7…

A: Given,  Current passed = I = 0.60 A  Volume in mL = 15.0 mL Time period = t = 11.7 min.  Equation is…

Q: What volumes of H₂ (9) and O₂ (g) at STP are produced from the electrolysis of water by a current of…

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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: (b) A constant current was passed through a solution of AuCl; between gold (Au) electrodes. After a…

A: Given, Mass of gold deposited = 2.628g Time = 20min = 1200 second

Q: Determine the molar mass (amu) of Metal (M) if it took 2.91 minutes for a current of 1.2 A to plate…

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Q: Determine the molar mass (amu) of Metal (M) if it took 1.57 minutes for a current of 1.09 A to plate…

A: First we would calculate the charge using formula : Q = I × t Then we would calculate the moles of…

Q: Mg(s) + Pb²*(aq) → Mg²*(aq) + Pb(s) If the above galvanic cell starts at standard state conditions,…

A: Option D When reactants decrease and product concentration increases the reaction quotient…

Q: Copper is electroplated from CuSO4 solution. A constant current of 4.28 A is applied by an external…

A:

Q: ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 2.54 minutes for a current…

A: Charge = current *time (in s)  Charge = 1*2.54*60 = 152.4 C

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

A:

Q: How many seconds are required to deposit 0.218 grams of tin metal from a solution that contains Sn2+…

A: F = 96500 C mol-1 Current = charge/time

Q: (c) (c) The magnitudes but not the signs of the standard electrode potentials of two metals, X and Y…

A: Given half-cell reactions are X2+  + 2e- →X;  E0 = 0.25  V  Y2+ + 2e-  → Y; E0 = 0.34  V Also given…

Q: How long would it take to deposit 3.75 g of iron from an aqueous solution of iron (III) sulfate by…

A: According to Faraday's First Law of Electrolysis, the chemical deposition due to flow of current…

Q: A current of 5.83 A is passed through a Fe(NO3)2 solution for 1.60 h. How much iron is plated out of…

A: According to Faraday's law of electrolysis, the amount of substance deposited on an electrode is…

Q: How long would it take to deposit 9.38 g of copper (molar mass 63.55 g/mol) at the cathode of an…

A: Faraday's law states that the amount of chemical change that is produced by passing a current to an…

Q: Semimetallic silicon can be made by the electrolysis of molten SiO2. (a) What mass of Si is formed…

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Q: Molten CaCl2 can be electrolyzed to form metallic Ca. For what duration should an electrolysis be…

A:

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: 2+ A current of 3.40 A is passed through a solution containing Cu²+ (aq) for 30.0 minutes, with…

A:

Q: A current of 9.22×104 A is passed through an electrolysis cell containing molten CaCl, for 10.9…

A: We will use relation of mass and gm equivalent

Q: Determine the sign of the electrodes in the cell. The left side half-cell is the and charged. The…

A: Answer: The left side of the half cell is the anode and negative charge.

Q: 12) What mass of silver can be plated onto an object in 67 minutes at 8.70 A of current? Ag'(aq) + e…

A: Given ->  Time (t) = 67 minutes = 67 × 60 seconds= 4020 s  (1minute = 60 seconds)  Current (i) =…

Q: Determine the molar mass (amu) of Metal (M) if it took 2.85 minutes for a current of 1.1 A to plate…

A: Molar mass can be calculated as:-

Q: Gold can be plated out of a solution containing Au3+ according to the half-reaction:Au3+(aq) + 3…

A: It is given that gold is plated for 25 minutes and the current is of 5.5 A and the half-reaction is…

Q: (a) Liquid H2O is subjected to electrolysis. One of the half-reactions is 2 H2O → O2 (g) + 4 H+(aq)…

A: We have to calculate the Faraday of electricity required and the time taken.

Q: ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 1.61 minutes for a current…

A:

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: ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 2.21 minutes for a current…

A: To solve this problem we will the formula  m = Z •i•t  Where ,  m = mass of metal  Z =…

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: Chromium can be electroplated from aqueous potassium dichromate, with the reduction shown below. If…

A: Given: Voltage = 11.6 V Current = 6.0 A mass of chromium (Cr) = 3.91 g molar mass of chromium =…

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: Molten CaCl₂ can be electrolyzed to form metallic Ca. For what duration should an electrolysis be…

A: For CaCl2 , the given data is- Current(I) = 2.06A Mass of Ca = 29.3g Atomic mass of Ca = 40.078 g…

Q: A current of 13.4A is passed through an electrolysis cell containing molten NaCl for 16.8 minutes.…

A: The objective of the question is to predict the products of electrolysis of molten NaCl and to…

Q: How many seconds are required to deposit 0.145 grams of zinc metal from a solution that contains Zn*…

A: Answer :-  t = 447 (s) The time required to deposit 0.145 g of Zn metal from a Zn2+ solution when…

Q: The surface area of an object to be gold plated is 49.8 cm?, and the density of gold is 19.3 g/cm?.…

A: Given: Surface area of gold (A) = 49.8 cm2                         Density of gold = 19.3 g/cm3…

Q: Determine the molar mass (amu) of Metal (M) if it took 2.54 minutes for a current of 1 A to plate…

A: From combination of first and second law of Faraday, we have :  M = n*F*m/(I*t) ....(1) Here, n =…

Q: Metallic iron can be made by the electrolysis of molten Fe2O3. (a) What mass of Fe is formed by…

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Q: (a) A student is required to construct a battery in the form of a galvanic cell using nickel (II)…

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Q: liters of Cl₂(g) is generated by this electrolysis. (b) How many moles of NaOH(aq) are formed in the…

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Q: Molten CaCl, can be electrolyzed to form metallic Ca. For what duration should an electrolysis be…

A: Given-> Current (I) = 2.99 ampere Weight of Ca= 23.5 gm

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.