1. If a current of 3.80 A flows for 4.79 hr, then what quantity of charge (in C) has flowed? 2. If a current of 0.50 A flows for 10.40 hr, then how many moles of electrons have flowed? 3. In the reduction of aluminum ions to alumimum: Al3+(aq) + 3e- → Al(s) how many grams of alumimun are produced by a current of 6.75 A for 17.49 hr?

Q: The MnO2 used in alkaline batteries can be produced by an electrochemical process of which one…

A: Answer: 174.0

Q: Giorno Giovanna likes golden stuff. However, since he is currently broke, he has to settle for…

A: Gold ion gains 3 electrons to get reduced to gold as per below equation Au3+ + 3e-  --> Au

Q: How long will it take to plate out 3.9 g Ni from aqueous Ni2+ with a current of 108.2 A? HOW DO WE…

A: To plate Ni using the process of electrolysis, the reaction that needs to be employed on the…

Q: (a) In the electrolysis of aqueous NaNO2, how many liters of O2(g) (at STP) are generated by a…

A: Given, Current = 62.7 A Time = 81.9 min NaNO2 (aq) + H2O (l)     NO (g) + O2 (g) + NaOH (aq)…

Q: How many seconds will be required to produce 1.00 g of nickel metal (58.693 g/mol) by the…

A:

Q: How long will it take to plate out 3.0 g Ni from aqueous Ni2+ with a current of 113.1 A? HOW DO WE…

A:

Q: (a) In the electrolysis of aqueous NaCl, how many liters of Cl2(g) (at STP) are generated by a…

A: i = 81.2 A t = 59.2 min

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: se a current of 770. mA flows through a copper wire for 10.0 minutes. Calculate how many moles of…

A:

Q: A metal object is to be gold-plated by an electrolytic procedure using an aqueous AuCla solution.…

A: Given : Time = 3.0 min = 3.0 X 60 = 180 s                                              (Since 1 min…

Q: Q3/B: current of (0.5 ampere) was passed through a solution of (CUSO4) or (one hour).Calculate the…

A: Oxidation is associated with loss of electrons. Reduction is associated with gaining of electrons.

Q: 5. Consider the following reactions: 3 Ni 2"taq) + 2Cr(OH)3 (s) + 10 OH ¯ (aq) → 3 Ni (s) + 2 CrO4…

A:

Q: 1. a)How many grams of zinc metal will be deposited from a solution that contains Zn2+ ions if a…

A: Note - Since you have asked multiple questions, we are bound to solve only the first question for…

Q: How long must a current of 5 amperes (A) be maintained to electroplate 60 g of calcium from the…

A:

Q: Brass, an alloy of copper and zinc, can be produced by simultaneously electroplating the two metals…

A:

Q: 10

A:

Q: How long will it take to plate out 1.0 g Ni from aqueous Ni2+ with a current of 105.9 A? HOW DO WE…

A: Given: Mass of Ni to be plated out = 1.0 g. Current pass = 105.9 A.

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

A:

Q: a) In the electrolysis of aqueous NaNO2, how many liters of O2(g) (at STP) are generated by a…

A: Given data: Current = 67.8 A = 67.8 C/sec Time = 86.4 min = 86.4 x 60 sec Formula used: q = I x t

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…

A:

Q: Determining volume of a gas by electrolysis. What volume of chlorine gas at standard temperature and…

A: It is given that MgCl2 is electrolysed and a current of 12.4 A is passed for 1h.

Q: 1.Chrome is plated from solutions of chromium (III) ions. If a particular application requires 13.7…

A: Since you have asked multiple questions in a single upload, if you want the second question to be…

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

A: According to the first law of Faraday, the mass of a metal deposited on the anode during…

Q: How many grams of copper metal can be deposited from Cu²⁺(aq) when a current of 2.50 A is run for…

A: By using Faraday law, we can find mass of Cu deposited at respective electrode.   The following…

Q: One of the half-reactions for the electrolysis of water is: 2H2O (l) -----> O2 (g) + 4H+ (aq) + 4e-…

A: According to the ideal gas equation, PV=nRT where P, V, n, R and T are the pressure, volume, number…

Q: Determining volume of a gas by electrolysis. What volume of chlorine gas at standard temperature and…

A: Given information: Current = 12.4 A Time = 1.0 h Charge flown:  Q = It= 12.4×60×60= 44640 C For the…

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 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:

Q: What mass of Ba(s) may be deposited from an aqueous BaCl2 solution if a current of 2.50 A is applied…

A: Mass of electrodeposited species can be calculated from the amount of charge passed.

Q: How long will it take to plate out 1.0 g Ni from aqueous Ni2+ with a current of 105.9 A? HOW DO WE…

A: Given: Mass of Ni to be plated out = 1.0 g. Current pass = 105.9 A.

Q: (a) In the electrolysis of aqueous Na2O2, how many liters of H2(g) (at STP) are generated by a…

A: The reaction taking place is given as, => Na2O2 (aq) + H2O (l) ↔ H2 (g) + O2 (g) + NaOH (aq)…

Q: Over a period of time, the concentration of sulfuric acid in the lead storage battery of an…

A: Given data,Initial % by mass of H2SO4=38.0 %Final % by mass of H2SO4=26.0%Volume of H2SO4=734…

Q: Copper from a 200.0 mL solution of copper (II) sulfate is plated on to the cathode of an…

A:

Q: • Part A A lead-acid battery uses a redox reaction in which lead(0) and lead(IV) are both converted…

A: The reaction given is, => Given: Time passed = 5.00 hours = 5 × 60 × 60 = 18000 s…

Q: Determine the current (in A) to produce 3.00 g Ag when Ag⁺(aq) is electrolyzed for 2.00 h. (F =…

A: The half reaction when Ag+ (aq) is electrolyzed.                                           Ag+ (aq)…

Q: Electrolysis of an aqueous solution of sodium chloride produces chlorine, Cl, (g). The reaction that…

A:

Q: 2. Tin-plated steel is used for tin cans. If the production of sheets of tin-plated steel requires…

A: Formulas used : I = q/t     where I is the current in amperes                            q is the…

Q: 4. A copper rod was purified by using it as the anode in the electrolysis of a 1.0 M copper (II)…

A: Anode is the electrode on which oxidation takes place and Cathode is the electrode where reduction…

Q: An electrical engineer is analyzing an electroplating run and wants to calculate the charge that has…

A:

Q: Calculate the value of the faraday if electrolysis of a NaCl solution with a current of 1.60 A for a…

A:

Q: How long will it take to plate out 4.9 g Ni from aqueous Ni2+ with a current of 113.1 A? HOW DO WE…

A: Given:: Mass of Ni= 4.9 g molar mass of Ni=58.6934 g mol-1 charge = ?

Q: If in using a lead-acid battery to start a car, 1.00 gram of Pb (207.2 g/mol) is consumed on the…

A: Given:  m = 1 g of Pb MW = 207.2 mol = 1207.2= 0.004826 mol of Pb I = 0.5 C/s

Q: How long would it take a current of 1 ampere to reduce completely 80 cm3 of 0.10 M Fe2(SO4)3 to…

A: We can solve this problem by using the faraday law of electrolysis  W= (E×i×t)/96500 W= mass of a…

Q: (a) In the electrolysis of aqueous Naz2C204, how many liters of H2(9) (at STP) are generated by a…

A: The balanced chemical reaction can be written as follows: Na2C2O4 (aq) +  2H2O (l)  →  2CO2 (g) + H2…

Q: How long must a current of 0.25 A pass through a sulfuric acid solution to liberate 0.400 L of H2…

A: We have to determine how long must a current of 0.25 A pass through a sulfuric acid solution to…

Q: How long will it take to plate out 4.2 g Ni from aqueous Ni2+ with a current of 112.3 A? HOW DO WE…

A:

Q: When a suspected drunk driver blows 182 ml. of his breath through the fuel cell breathalyzer, the…

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.