Example 9 A copper surface area, A=100 cm², is exposed to an acid solution. After 24 hour, the loss of copper due to corrosion (Oxidation) is 15*10* gram. Calculate: (a) The current density in µA/cm². (b) The corrosion rate in mm/y Given that: molar mass for copper = 63.54 g/mc p = 8.96 g/cm

Example 9 A copper surface area, A=100 cm², is exposed to an acid solution. After 24 hour, the loss of copper due to corrosion (Oxidation) is 1510 gram. Calculate: (a) The current density in µA/cm². (b) The corrosion rate in mm/y Given that: molar mass for copper = 63.54 g/mc p = 8.96 g/cm

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: Complete and balance the following redox reaction in acidic solution NO2(g) - NO, (aq) + NO(g)…

A: Redox reaction is a reaction in which one element undergoes oxidation while another element…

Q: 7. Solutions A and B are separated by a membrane that is permeable to Ca²+ and impermeable to Cl¯.…

A: b

Q: Considering an experiment of using electrolysis to make bleach: (a) What would the effect be of…

A: Bleach is sodium hypochlorite NaOCl , widely used as a disinfectant or a bleaching agent. this…

Q: 2Cr(OH)3 + 3CI→2Cr+ 3CIO+ 3H2O In the above reaction, the oxidation state of chromium changes from |…

A: Given equation: 2Cr(OH)3 + 3Cl- → 2Cr + 3ClO- + 3H2O We have to find how the oxidation state of…

Q: In the electrolysis of an aqueous AGNO3 solution, 0.49 g of Ag is deposited after a certain period…

Q: In an electrochemical cell, a metal anode lost 0.187 g while a total volume of 0.08633 L of hydrogen…

A: The pressure of dry hydrogen gas can be determined as, Barometric Pressure = Pressure of water vapor…

Q: A 1.00-L solution contains 2.00×104 M Cu(NO3)2 and 2.40x10-3 M ethylenediamine (en). The Kf for…

A: Given that : The volume of the solution = 1.00 L The concentration of Cu(NO3)2 = 2.00 x 10-4 M The…

Q: a) Write the definition of reduction and oxidation.

Q: In aqueous solution, bromine oxidises sulfur dioxide, SO,, to sulfate ions, So,²- (i) Deduce the…

A: Answers are explained below. Deduction of oxidation state of sulfur is as follows:

Q: 18.15 Consider the following half-reactions: MnO, (aq) + 8H*(aq) + 5e¯ - Mn²*(aq) + 4H,O(1) NO, (aq)…

A: The standard reduction potential ( Eo) value for the 1st reaction is 1.512V and for the second…

Q: (a) What is corrosion?(b) How is corrosion caused

A: (a) Metals react with the atmospheric oxygen to form the metal oxide. This metal oxide is also known…

Q: 2+ If the anode of a galvanic cell is composed of Fe/Fc" (, which of the following should be used as…

A: Welcome to bartleby ! We have to tell which one of them is best for cathode cell so that voltage…

Q: In an electrochemical cell, a metal anode lost 0.125 g while a total volume of 0.09055 L of hydrogen…

A: In an electrochemical cell, a metal anode lost 0.125 g while a total volume of 0.09055 L of hydrogen…

Q: A total of 1.569 F of electricity (1 F = 1 mol e¯) was required to electrodeposit all of the Zn and…

A: Answer: This question is based on Faraday's law of electrolysis. To deposit each mole of Zinc ion…

Q: Calculate the grams of nickel (58.69 g/mol) can be electroplated from a solution of Ni(NO3)2(aq)…

Q: a) (i) Write a half equation to show the conversion of MnO4 toMn2+. (ii) Write a half equation to…

A: Hello. Since your question has multiple parts, we will solve first question for you. If you want…

Q: A total of 1.707 F of electricity (1 F = 1 mol e¯) was required to electrodeposit all of the Zn and…

A: Answer:This question is based on Faraday's law of electrolysis. To deposit each mole of Zinc ion and…

Q: What is(are) the product(s) formed at the cathode in the electrolysis of aqueous MGB1, Br2(4) O…

A: Given : We have to tell what are the electrolysis product of MgBr2 at cathode.

Q: 21.28 A voltaic cell is constructed with an Ag/Ag* half-cell and a Pb/Pb²* half-cell. The silver…

A: Voltaic cell involves conversion of chemical energy into electrical energy through redox reaction.

Q: (b) A zinc plate is then electrically connected to the carbon steel plate and both are immersed in…

A: (b) The metal which have more oxidation potential is anode and which have less is cathode So Zn is…

Q: complete and blance the following oxidation-reduction reactions, which give the highest…

Question

Example 9
A copper surface area , A=100 cm², is exposed to an acid solution. After 24 hour, the loss
of copper due to corrosion (Oxidation) is 15*10 gram. Calculate:
(a) The current density in µA/cm?.
(b) The corrosion rate in mm/y
Given that: molar mass for copper = 63.54 g/n
8.96 g/cm³

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Extraction of Crude Metal from Concentrated Ore

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

When a solution of NaI in water was electrolyzed with graphite electrodes, a gas was evolved at the cathode and a yellow-brown color was observed around the anode. The solution became basic. Which one of statements (a) - (d) is not correct? If all are correct, select option (e). Please see the data page for relevant electrode potentials for the half reactions.a) OH- ions were formed at the cathode.b) I- ions were oxidizedc) The gas, which was evolved, was O2.d) Water was reducede) Statements (a) - (d) are all correct
part 2
How long will it take in hours to create 1.026 grams of Cr at the cathode of an electrolytic cell if 265.8 mA of current is passed through a solution containing Cr(NO3)6 molar mass of Cr is 51.9901
(b) A zinc plate is then electrically connected to the carbon steel plate and both are immersed in seawater. Which material will form the anode and which the cathode in the resulting galvanic couple? Justify your answer. (c) Write down the relevant anodic and cathodic reactions for (b).
Which of the following is not a method that can be taken to prevent, or at least reduce, corrosion? anodic protection application of coatings use of inhibitors environmental alteration
Chromium plating is applied by electrolysis to objects suspended in a dichromate solution, according to this half-reaction: Cr2O7^2- (aq) + H^+ (aq) + e^- —> Cr(s) + H20(l) (unbalanced) The same amount of electrical energy was applied to a solution containing X^n+, After 2 hours, 40.15 g of solid X was deposited. If the atomic weight of X is 64.56, what is the charge of X^n+?
Please don't provide hand writtin solution....
question 26
(B) Sample of Zinc have dimensions 10mm x 20mm x 2mm is at one sides of the sample are exposed to a corrosive environment. Calculate corrosion rate in mm/y? M=65g/ mole, density-7.14g/cm³, Ian-1.12 10³ A/cm², t-3.1536 x10' sec/year, n=2
10. In our discussion of anode reservoirs for Li-Ion batteries, which elemental solid was identified as the best reservoir? (a) Si (b) C/graphite (c) Sn (d) Li-Sn alloy
Answer my question please
A current of 5.65×104 A is passed through an electrolysis cell containing molten KCl for 12.8 days.(a) How many grams of potassium are produced? ____________g(b) How many liters of chlorine are collected, if the gas is at a temperature of 273 K and a pressure of 1.00 atm? _____________L