Enter your answer in the provided box. The MnO, used in alkaline batteries can be produced by an electrochemical process of which one half reaction is Mn2*(aq) + 2H,0(1) → MnO2(s) + 4H*(aq) + 2e If a current of 25.0 A is used, how many hours are needed to produce 1.23 kg of MnO2?

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2vo; (aq)…

A:

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

A: Answer: 174.0

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: 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: 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: (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: Copper metal can be purified electrolytically according to the following arrangement. The anode is…

A: W = I × t × M / n × F Where ; W = mass of  purified Cu = ? I = current = 15 A  t = time = 8.5 hours…

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: A battery can provide a current of 4.00 A at 1.60 V for 1.00 hr. How much energy (in kJ) is…

A: Given that a current of 4.00 A was provided by battery at 1.60 V. The power can be calculated as…

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

A:

Q: Use a table of Standard Reduction Potentials to predict if a reaction will occur between Hg metal…

A: We will write reaction first , then using standard reduction potentials, we will predict whether…

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: In the commercial production of sodium metal by electrolysis, the cell operates at 7.0 V and a…

A: The faraday's first law explains that the quantity of any species deposited is directly proportional…

Q: What mass of zinc (in grams) is deposited at the cathode when a current of 8.3 amperes passes…

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: 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: 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: (Q98) Electrolysis is being used to plate chromium onto a large plastic surface. If a total of 3.77…

A: Given, mass of Chromium (Cr) = 3.77 g Current (I) = ? Time (t) = ? min Note: molar mass of Cr = 52.0…

Q: Tin-plated steel is used for "tin" cans. Suppose that in the production of sheets of tin-plated…

A:

Q: The electrolysis of AℓCℓ3 at high temperature produces aluminium metal. If a constant electrical…

A: Given: current = 10 × 103 mA Or current = 10 × 103 × 10-3 A Or current = 10 A And time = 1 hour =…

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: Consider the following electrochemical cell reaction:   Pb2+(aq)  +  2 Cr2+(aq)  →  Pb(s)  +  2…

A: We will calculate cell potential using nernst equation.

Q: How long ( hours) would it take to unload 0.433 moles of vibranium (Vb) metal during electrolysis of…

A: We have to calculate time needed for electrolysis  Molar mass of Tr not provided so only 1st…

Q: A lead storage battery delivers a current of 6 A for one hour and 22 minutes at a voltage of 12 V.…

A: The discharging reaction if lead storage battery is given as:Pb (s) + PbO2 (s) + 2SO42- (aq) + 4H+→…

Q: VOLTAIC CELL AND ELECTROLYSIS 1. Fischl, a scientist from Mondstadt specializing in…

A: Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: A gold (III) chloride solution was electrolyzed using a current of 13.5 amperes for four hours. How…

A: Mass deposit or plated  = Z.i.t

Q: many grams of cobalt metal will be deposited from a solution that contains Co2+ ions if a current of…

A: Given:  Current = 0.974 A  Time = 67.4 min = 67.4 x 60 = 4044 sec

Q: Write the balanced equation for the overall reaction that occurs in the cell. Calculate E ̊ for the…

A: The reaction with smaller standard electrode potential, that reaction occurs at anode and reaction…

Q: How many amperes of current needs to be passed through molten Sodium chloride (NaCl) to produce 2.1…

A: We have given that during the electrolysis of molten Sodium chloride 2.1 g of Sodium is produced at…

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: Suppose that a machine part requires 400 mg of copper to provide a coating that is thick enough for…

A: Given data,Current=0.5ATime=10min=10×60s=600s

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

A:

Q: a) A proposed battery involves the reaction of Zn(s) and Cl2(g) to give ZnCl2. If you want such a…

A: Hii there, since there are multiple questions posted. We are answering first question. If you need…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3Cu*…

A:

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

A: Interpretation -  In the electrolysis of aqueous NaNO2, how many liters of O2(g) (at STP) are…

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

A:

Q: Copper metal (63.55 g/mol) is purified by electrolysis. How much copper metal (in grams) could be…

A:

Q: Electroplating is a way to coat a complex metal object with a very thin (and hence inexpensive)…

A: Electroplating is a process of coating layer of metal over another metal by the process of…

Q: Weighing a copper atom in an electrolysis experiment. A standard experiment involves passing a…

A: Electrolysis is the process through which electrical energy is converted into the chemical energy…

Q: If an electrolysis plant operates its electrolytic cells at a total current of 150. A, how long, (in…

A: According to Faraday's First Law of Electrolysis, The amount of product deposited is directly…

Q: If a constant current of 7.3 amperes is passed through a cell containing Cu²+ for 1.5 hours, how…

A:

Q: In the electrolysis of molten MgCl 2, what mass of Mg metal is deposited by a current of 16 amperes…

A: Electrolysis is the process of conversion of electrical energy to chemical energy. This reaction…

Q: How much Beryllium metal can be deposited from a solution of BeCl2 by a current of 5.0 Amperes that…

A:

Q: An aqueous solution of an unknown salt of ruthenium is electrolyzed by a current of 3.00 A passing…

A: Given Current (I) = 3A Given mass = 1.572g Time = 25min = 1500s Molecular weight = 101.07g

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

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.