A piece of corroded steel plate was found in a submerged ocean vessel. It wasestimated that the original area of the plate was 13 in² and that approximately 3.8kg had corroded away during the submersion. Assuming a corrosion penetration rateof 200 mpy for this alloy in seawater, estimate the time of submersion in years. Thedensity of steel is 7.9 g/cm³. Calculating the submersion time from the corrosionpenetration rate (CPR).CPR ==ᏦᎳpAt

Step 1: First, list the given in the problem.CPR=200mpyA=13in2W=3.8kgρ=7.9g/cm3 Step 2: find the…

Answered: A piece of corroded steel plate was…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter17: Electrochemistry And Its Applications

Section: Chapter Questions

Problem 102QRT

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An engineer is designing a mirror for an optical system. A piece of metal that measures 1.3 cm by 0.83 cm will have a coating of rhodium plated on its surface to serve as the mirror. The rhodium thickness will be 0.00030 mm, and the electrolyte contains Rh3+ ions. If the operating current of the electrolysis is 0.10 A, how long must it be operated to obtain the desired coating? What mass of rhodium is deposited? (The density of rhodium is 12.4 g cm-3.)
An aqueous solution of an unknown salt of vanadium is electrolyzed by a current of 2.50 amps for 1.90 hours. The electroplating is carried out with an efficiency of 95.0%, resulting in a deposit of 2.850 g of vanadium. a How many faradays are required to deposit the vanadium? b What is the charge on the vanadium ions (based on your calculations)?
A silver coulometer (Study Question 106) was used in the past to measure the current flowing in an electrochemical cell. Suppose you found that the current flowing through an electrolysis cell deposited 0.089 g of Ag metal at the cathode after exactly 10 min. If this same current then passed through a cell containing gold(III) ion in the form of [AuCl4], how much gold was deposited at the cathode in that electrolysis cell?
You wish to electroplate a copper surface having an area of 1200 mm2 with a 1.0-m-thick coating of silver froma solution of Ag(CN)2 ions. If you use a current of150.0 mA, calculate how much electrolysis time youshould use. The density of metallic silver is 10.5 g/cm3.
If a plating line that deposits nickel (from NiCl2 solutions) operates at a voltage of 0.40 V with a current of 400.0 A and a total mass of 49.0 kg of nickel is deposited, what is the minimum number of kWh consumed in this process?
A current is passed through a solution of copper(II) sulfate long enough to deposit 14.5 g of copper. What volume of oxygen is also produced if the gas is measured at 24 °C and 0.958 atm of pressure?
In the electrolysis of a solution containing Ni2+(aq), metallic Ni(s) deposits on the cathode. Using a current of 0.150 A for 12.2 minutes, what mass of nickel will form?
Using values from the table of standard reduction potentials, calculate the cell potentials of the following cells. (a) Fe(s)|Fe2+(aq)Hg2+(aq)|Hg(l) (b) Pt(s)|Fe2+(aq),Fe3+(aq)MnO4(aq),H+(aq),Mn2+(aq)|Pt(s) (c) Pt(s)|Cl2(g)|Cl-(aq)Au+(aq)|Au(s)
How long would it take to electroplate a metal surface with 0.500 g nickel metal from a solution of Ni2+ with a current of 4.00 A?
Calculate the voltages of the following cells at 25°C and under the following conditions: (a) Cu|Cu+(0.80M)Hg22+(0.10M)|Hg|Pt (b) Cr|Cr3+(0.615M)Ni2+(0.228M)|Ni
Calculate the voltages of the following cells at 25°C and under the following conditions: (a) Zn|Zn2+(0.50M)Cd2+(0.020M)|Cd (b) Cu|Cu2+(0.0010M)H+(0.010M)|H2(1.00atm)|Pt
13.106 Hydrazine, N2H4 , has been proposed as the fuel in a fuel cell in which oxygen is the oxidizing agent. The reactions are N2H4(aq)+4OH-(aq)N2(g)+4H2O(l)+4eO2(g)+2H2O(l)+4e4OH-(aq) (a) Which reaction occurs at the anode and which at the cathode? (b) What is the net cell reaction? (C) If the cell is to produce 0.50 A of current for 50.0 h, what mass in grams of hydrazine must be present? (d) What mass in grams of O2 must be available to react with the mass of N2H4 determined in part (c)?

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