How many amps are required to produce 59.6 g of aluminum metal from a sample of molten aluminum fluoride in 4.19 hours?

Q: When molten lithium chloride, LICI, is electrolyzed, lithium metal is liberated at the cathode. How…

A: To calculate mass of lithium liberated:   Molar mass of lithium = 7 g  So, it means 1F = 96500 C…

Q: The electrolysis of an aqueous solution of KBr has the overall reaction: 2H2O+2Br (aq) → H2(g) +…

A: The given balanced chemical equation is:              2H2O + 2Br-aq → H2g + Br2l + 2OH-aq Bromide…

Q: Calculate the charge, in coulombs, is required to deposit 1.5 g of solid magnesium from a solution…

A: The answer to the following question is- Given, mass of magnesium = 1.5 g  Molar mass of magnesium =…

Q: Determine the mass of Sodium( Na) produced when a 17 amp current flows for 9 hr through a cell…

A: The overall reaction in the cell: 2NaCl→2Na+Cl2 Cathode: Reduction Na++e−→ Na Anode: Oxidation 2Cl −…

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: What products are produced from the electrolysis of a solution of iron(II) bromide?

A: Electrolysis is a process in which an electrolyte in molten state or aqueous state is decomposed by…

Q: How many amperes of current needs to be passed through molten Sodium chloride to produce 2.4 g of…

A: Faraday's First law,           m α Q          m = eQ               = ect               = E96500ct…

Q: Convert 6.3 Faradays to Coulombs.

A: The question is based on concept of unit conversion. We have to convert given quantity of Faraday's…

Q: 5. The mass of metal deposited by the electrolysis of an aqueous solution of metal ions increases in…

A:

Q: Sodium metal is produced commercially by the electrolysis of molten sodium chloride. The by-product…

A: Sodium metal is commercially produced by electrolysis of molten sodium chloride.  Sodium metal was…

Q: What unit is used to measure the magnitude of electrical current? What unit is used to measure the…

A: The unit used to measure the magnitude of electrical current is Amperes.The unit used to measure the…

Q: B. Click on the left pop-out tab for metals and select silver (Ag). Click on the left pop-out tab…

A: Since you have posted multiple questions with multiple sub-parts, we will solve the first three…

Q: A steady current was passed through molten CoSO. until 2.35 g of metallic cobalt was produced.…

A:

Q: 17. What would be the products of a 0/1 single-replacement reaction between copper and zinc sulfate?…

A: Given :  To determine the products of a 0/1 single-replacement reaction between copper and zinc…

Q: What happens, when you add 3 electrons to Mn7+? O a. nothing has changed in the chemical character O…

A: if we add 3 electrons to Mn7+ then it will reduced.

Q: Convert 1.9 Faradays to Coulombs.

A: Faraday and Coulomb are units of electric charge. 1.9 Faraday = ? Coulomb

Q: The hydroperoxide ion, HO2–(aq), reacts with permanganate ion, MnO4–(aq) to produce MnO2(s) and…

A: The reactants given are HO2- and MnO4- ions. And the products given are MnO2 and O2. Hence the…

Q: 3. A proposed battery involves the reaction of Zn(s) and Cl2(g) to give ZnCl2. If you want such a…

A: The question is based on the concept of electrochemistry. It involves the application of  faraday's…

Q: How long would it take in minutes to plate 1.00 gram of silver to a watch when 9.2 amps are passed…

A: Mass of silver deposited = m = 1.00 g  Current passed I = 9.2 A Atomic mass of Silver M = 107.8682…

Q: 1 A sample of a Fe2+ solution requires 26 mL of 0.0200 M K2Cr2O7 for a reaction  in which Fe2+ is…

A: Normality and molarity are two unit of concentration. Here we required to find the  normality of…

Q: Assign an oxidation number to the element that is specified. S:SO32− P:Mg3(PO4)2 N:N2O3

A: The oxidation number of oxygen in oxides is -2.

Q: The reaction of magnesium metal (Mg) with oxygen (O 2) forms MgO. Write a balanced equation for this…

A: A redox reaction is a reaction in which the oxidation and reduction occurs simultaneously.

Q: 2Al2O3 + 3C = 4Al +3CO2 If an elecltrolytic cell has a constant voltage of 4.4 V and produces a…

A: Given: 2Al2O3 + 3C = 4Al +3CO2 If an elecltrolytic cell has a constant voltage of 4.4 V and produces…

Q: Convert 6.9 Faradays to Coulombs.

A:

Q: How many grams of copper nitrate (Cu(NO3)2) should be added into 1000 ml water to produce a half…

A: Given data,Volume of water=1000mLElectric potential=0.32VNernst equation;E=Eo-0.0591nlogQ   ---at…

Q: What methods are used to reduce the corrosion of metals?

A: Corrosion is a naturally occurring process where a metal is converted into its metal oxide by…

Q: Convert 2.5 Faradays to Coulombs.

A: We know that 1 Faraday =96485.34  coulomb. Hence now we have to find what will be the value of 2.5…

Q: Determine the mass of Sodium( Na) produced when a 11 amp current flows for 4 hr through a cell…

A: We have given Determine the mass of Sodium(Na) produced when a 11 amp current flows for 4 hr through…

Q: Which of the following metals would NOT react with a strong acid to form hydrogen gas? A. Ca B. Sn…

A: Which of the following metals would NOT react with a strong acid to form hydrogen gas?

Q: In the thermite process, the reducing agent is:(a) Nickel(b) Zinc(c) Sodium(d) Aluminium

A: Thermite welding is a process that makes use of an exothermic reaction to create a high temperature.…

Q: Aluminum is produced commercially by the electrolysis of Al203 in the presence of a molten salt. If…

A: Total current, I = 1.09 million Ampere                           = 1.09×106 Ampere Time, t = 3 hr…

Q: Which products are obtained in the electrolysis of molten NaI?

A: Na metal produced at cathode and I2 produced at anode.

Q: Electrolysis of molten NaCl is done in a Downs cell operating at 7.0 volts and 4.0 x 10^4 A. How…

A: Molten NaCl electrolysis is given by the following expressions- At anode - 2 Cl- (aq) → Cl2(g) + 2…

Q: grams of iron

A:

Q: 0.115 V, what is the value of the standard free energy (in kJ) for this reaction?

A:

Q: 13.76 Chrome is plated from solutions of chromium(III) ions. If a particular application requires…

A:

Q: What is the oxidation number of the underlined element? K2SO3 A. –2 B. +4 C. +6 D. –4

A: A question based on structure of atoms that is to be accomplished.

Q: What current is used to liberate 213 grams of chlorine, Cl 2 from a solution NaCl if it take 2…

A: Faraday's 1st law of electrolysis is one of the most important law which explains that the quantity…

Q: What mass of gold is produced when 15.2 A of current are passed through a gold solution for 25.0 min

A: Given information: Current (I) = 15.2 A Time (t) = 25.0 min

Q: he Valve of trionde is Satlfer the mn f o. 2:+24+

A: Given reaction is: 2 e- + 2 H+ + S +O2  -----> SO3 + H2O                                  ΔH⁰ =…

Q: A factory wants to produce 1.00 x 10 kg barium from the electrolysis of molten barium chloride. What…

A:

Q: Considering the carrosion of ferrous metal (containing iron) metal, which of the following…

A: Corrosion is a reduction-oxidation process in which metal is oxidized by the oxygen in its…

Q: A factory wants to produce 1.00 x 103 kg barium from the electrolysis of molten barium chloride.…

A:

Q: Mention the reactions occurring at (i) anode, (ii) cathode, during working of a mercury cell. Why…

A: A voltaic cell is an example of electrochemical cell. It uses a chemical reaction to produce…

Q: How many coulombs will it take to deposit 8.97 g of metallic copper on the cathode from an aqueous…

A: The metal will be reduced at cathode as follows: Cu2+(aq)  +  2e-  ------------->  Cu(s).

Q: When 1.00 mole of chlorine gas is reduced to chloride ions in an electrolytic cell, what charge (in…

A: Reduction of 1 mol of chlorine is given below, Number of moles of electrons is 2.

Q: Would you expect a mercury cell to give a constant voltage and why?

A: Yes, mercury cell provides a constant voltage throughout life. This is because there are no ions…

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.