5. Consider the following reactions: 3 Ni 2"taq) + 2Cr(OH)3 (s) + 10 OH ¯ (aq) → 3 Ni (s) + 2 CrO4 -2 (aqg) + 8 H2O (1) A) What is the value for n for this reactions? B) Calculate the standard Gibbs Free-Energy C) How long does it take a current of 5 A to deposit 95 g of nickel?

Q: An unknown metal M forms a soluble compound, M(NO3)3. A solution of M(NO3)3 is electrolyzed. When a…

A: The deposition is M+3 (aq) + 3e– ------> M (s)Number of moles of electrons = 3 × number of moles…

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

A:

Q: What is the electrical current, in Amperes, that must be applied if 6.50 g Ag is deposited at the…

A:

Q: A current of 4.89 A is passed through a Pb(NO3)2 solution. How long, in hours, would this current…

A:

Q: A solution of NaCl in water was electrolyzed with a current of 6.51 A for 23.0 min. How many…

A: Answer:Here:

Q: How much time (in hours to two decimal places) must pass to produce 50 grams of gold using a 6.50 A…

A: Use the given quantities carefully to solve for time taken by gold.

Q: A current of 4.21 A is passed through a N i ( N O 3 ) 2 solution. How long, in hours, would this…

A: Current (I) = 4.21 A  Mass of nickel deposited (m) = 4.50 g

Q: A current of 5.26 A is passed through a Pb(NO3)2 solution for 1.20 h. How much lead (in g) is plated…

A:

Q: A current of 11.3 A is applied to 1.25 L of a solution of 0.552 M HBr converting some of the H+ to…

A: Equivalents of H+ ions reduced = QF=I×t96500=11.3 ×73 ×6096500= 0.513 Total equivalents of H+ ions…

Q: Consider the following cell reaction: Fe(s) + 2 H+(? M) →→→Fe²+(1.00 M) + H₂(g) (1.00 atm) If the…

A: The given cell reaction is Fe(s)  + 2H+ (? M) →  Fe2+ (1.00 M) + H2 (g) (1.00 atm) The concentration…

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: How long must a current of 20.0 amps be applied to a solution of CrCl3 to produce 175 g of Cr (s)…

A:

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

A: According to the Faraday's electrolysis law -  W = Zit  W is the weight in grams.  Z = E/96500 where…

Q: your answer in the provided box. A constant current is passed through an electrolytic cell…

A: Given,produced volume of Cl2 gas at anode ( at STP ) = 4.18 Ltime taken = 16 h.

Q: How many grams of silver will be obtained when the aqueous silver nitrate solution is electrolyzed…

A:

Q: How long (in hours) must a current of 4.61 amps be passed to produce 79.5 g of copper metal from a…

A: Given:: Current i= 4.61 A  Mass of Cu = 79.5 g  Molar mass of Cu= 63.55 g mol-1 Time t= ?

Q: Determine the current (in A) to produce 6.50 g Ag when Ag⁺(aq) is electrolyzed for 2.00 h. (F =…

A: Given information  Mass of Ag = 6.50 g Time = 2.00 h To calculate: Current

Q: Manganese dioxide (MnO2) for use in dry cell batteries is made by electrolyzing solutions of Mn2*…

A:

Q: What mass of gold can be plated onto an object in 9.18 minutes at 4.91 A of current ? Au^3^+…

A:

Q: A silver material is to be plated with gold using an aqueous solution of Au*3. How many moles of…

A: we have to calculate moles of gold deposited

Q: A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is…

A: The Nernst equation is a mathematical relationship used in electrochemistry that relates the…

Q: 6. Consider the following cell. Al(s) | Al³* (1 M) || OH- (1 M) | Al(OH)3(s), Al(s) Given the Ksp…

A:

Q: Consider the following cell reaction: Fe(s) + 2 H*(? M) Fe2*(1.00 M) + H2(g)(1.00 atm) If the cell…

A: By applying formula Ecell = E•cell - 0.0591/2 . Log[Fe2+]| [H+]2  At 25 degree Celsius

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: Brass, an alloy of copper and zinc, can be produced by si-multaneously electroplating the two metals…

A:

Q: An aqueous solution of a platinum salt is electrolyzed for 1.00 hour using a current of 1.50 A to…

A: According to Faraday's law when a solution of an element is electrolysed then it will deposited.…

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: Determine the current (in A) to produce 4.50 g Ag when Ag⁺(aq) is electrolyzed for 2.00 h. (F =…

A:

Q: In the electrolysis of an acid solution, oxygen can be produced by the following half-reaction:…

A:

Q: A current of 3.38 A3.38 A is passed through a Pb(NO3)2Pb(NO3)2 solution. How long, in hours, would…

A: Ans is 40.8min

Q: What mass of zinc metal can be produced per hour in the electrolysis of a molten zinc salt by a…

A: Current (I) = 84 ATime (t) = 1 hour = 3600 s mass of Zinc metal produced = ?Note:Molar mass of Zinc…

Q: Calculate the mass in grams of a metal Q ( Molar mass= 88.23 g/mol) that will be deposited from a…

A:

Q: How many grams of silver metal are produced from Ag⁺(aq) in 2.00 h with a current of 3.50 A? (F =…

A:

Q: How much time would it take for 325 mg of copper solid (atomic molar mass = 63.546 g/mol) to be…

A: Two moles of electrons give one mole of copper atom. Number of electrons required is determined as…

Q: In the electrolysis of an acid solution, oxygen can be produced by the following half-reaction:…

A:

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: An aqueous solution of an unknown salt of molybdenum is electrolyzed by a current of 2.50 A passing…

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: 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: A current of 4.63 A4.63 A is passed through a Pb(NO3)2Pb(NO3)2 solution for 1.30 h1.30 h. How much…

A: Amount of substance deposited at electrode during electrolysis can be calculated as follows

Q: A current of 3.27 A is passed through a Pb(NO3)2 solution. How long, in hours, would this current…

A:

Q: How many hours are required to plate 12.00 g of nickel metal from 1.00 M NİSO4(aq), using a current…

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.