A sample of zinc corrodes uniformly with a current density of 4.2 x 10® A/cm´ in an aqueous solution. (a) What is the corrosion rate of zinc in mg/dm/day? (b) What is the corrosion rate of zinc in mm/year? (a) Given current density, i = 4.2 x 10° A/cm? density, ame p= 7.1 g/cm3, n=2, F = 96 500 coulombs/mole. zinc atomic weight, M = 65.38 g/mol,

Q: (a) Write the half-reaction that occurs at a hydrogen electrode in acidic aqueous solution when it…

A: Concept introduction: Anodic reaction: It is the reaction that occurs at anode by loss of electrons…

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

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Q: Calculate the standard cell potential, E cell, for the following redox reaction. Ni(s) + Br2(1) →…

A: E 0  is the standard EMF of any cell. It is given by : E 0 cell = E 0red (cathode) - E 0 red (anode)…

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: 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: (19) Consider the following redox reaction that occurs in a voltaic cell: Cr2+ (aq) + Cu2+ (aq) →…

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Q: The following cell has a potential of 0.10 V at 25oC. Ni(s) | Ni2+(aq) (1.0 M) || H+ (? M) | H2(g)…

A: Ni(s)   +    2 H+(aq)     ⇔    Ni+2(aq)   +     H2 (g)    Ecello = 0.23…

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: The following redox reaction was performed under non-standard conditions. Zn(s) + Cu2*(aq) →…

A: The given redox reaction is, Zn (s) + Cu2+(aq)  →  zn2+ (aq) + Cu (s) Given that the concentration…

Q: (a) Draw a schematic representation of the galvanic (electrochemical) cell that is described by the…

A: A galvanic cell is defined as the electrochemical cell which converts chemical energy into…

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 5.99×104 A is passed through an electrolysis cell containing molten CaCl2 for 20.1…

A: Answers given as follows

Q: Determine the Ecell for the given redox reaction. Assume that the reaction reached equilibrium at…

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

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Q: O Fels) → Feo + 3e The balanced half-reaction occuring at the cathode in the redox reaction shown…

A: We have to predict balance reduction half reaction.

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

A: In this given question we have to find out standard emf of a cell made up of X and Y metal.

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: (a) In the electrolysis of aqueous NaCO3, how many liters of O₂(g) (at STP) are generated by a…

A: It is given that for an electrolysis reaction:current = 53.9 Atime = 73.9 minconvert min to sec.We…

Q: The voltage generated by the zinc concentration cell described by the line notation Zn(s)|Zn^ 2+…

A:

Q: The voltage generated by the zinc concentration cell described by the line notation Zn(s) | Zn²+…

A: It is a concentration cell in which standard electrode potential is zero. With the help of the…

Q: The cell potential of this electrochemical cell depends on the pH of the solution in the anode…

A:

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: 2 Magnesium and lead have similar first and second ionization energies, yet their reactivity with…

A: Only part (a) is mentioned to be solve. For the other parts to be solved available data is not…

Q: Consider the following half-reactions: Half-reaction E° (V) Br,(1) + 2e → 2Br (aq) |1.080V Co2+…

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Q: Write the balanced chemical equation for which the following shorthand notat Pt | Snt2 (aq), Sn+4…

A: For Sn4+/Sn2+, Ered = -0.15 V For Ag+/Ag Ered = +0.80 V Since E for Sn4+/Sn2+ is negative whereas R…

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

A:

Q: Use the following half-reactions to calculate the E0cell for the reaction and classify if the redox…

A: The reaction which involves both oxidation and reduction is called as the redox reaction. The…

Q: What mass of each of the following substances can be produced in 1.2 h with a current of 11 A? (a)…

A: Current = 11 ATime = 1.2 h

Q: (a) The standard reduction potential for X/X and Y/Y at 285 K are 0.52 V and 0.37 V respectively.…

A: Solution: In the given problem we have given reduction potential values and we have to represent the…

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

A:

Q: O Fe(ag) The balanced half-reaction occuring at the cathode in the redox reaction shown below is…

A: Redox reaction is a reaction in which both oxidation and reduction occurs simultaneously.  In…

Q: How long would it take to deposit 2.72 g of copper from an aqueous solution of copper II sulfate by…

A: Given that : Mass of copper to be deposited (w) = 2.72 g Current (i) = 2 amps

Q: A current of 8.46x1oʻ A is passed through an electrolysis cell containing molten KCi for 10.3 days.…

A: Given Current I = 8.46*104 A Time = 10.3 days Temperature = 273 K Pressure = 1 atm

Q: Metallic magnesium can be made by the electrolysis of molten MgCl2. (a) What mass of Mg is formed…

A: Given chemical reaction is :  MgCl2 (s)  ---------->  Mg(s)  +  Cl2 (g)  It is a thermal…

Q: 1.8107 g of steel are dissolved, treated so that Mn present is in the form Mn2+, and diluted to 500.…

A: Answer is explained below.

Q: A baby’s spoon with an area of 6.25 cm2is plated with silver from AgNO3 using a current of 2.00 A…

A: To calculate the mass of silver plated on the spoon first the charge that has passed will be…

Q: A current of 7.14×10“ A is passed through an electrolysis cell containing molten KCl for 13.9 days.…

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Q: A voltaic cell is constructed with two Zn2+ - Zn electrodes. The two half-cells have 3Zn2+4 = 1.8 M…

A: Given, The voltaic cell, Zn2+ - Zn When the two half-cells have [Zn2+] = 1.8 M     and[Zn2+] = 1.00…

Q: How many minutes will it take to electrodeposit 3.0 g of Cu (63.55 g/mol) on the surface of a…

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

Q: A pure organic acid sample (0.1516 g) is neutralized with OH- ions produced in a constant current of…

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.