According to Faraday's equation, W = ItM nF , where w = weight of metal corroded or electroplated in aqueous solution in time t, /= current flow, M = atomic mass of the metal in g/mol, n = number of electrons produced/consumed in the process, and F = Faraday's constant. 1. The anodic reaction that occurs at the cadmium electrode is as follows: Cd → Cd2+ + 2e. A cadmium electroplating process uses 30 A of current to chemically corrode a cadmium anode. If it is assumed that there are no side reactions, how long will it take to corrode 9 g of cadmium from the anode? The atomic mass of cadmium is 112.414 g/mol. Assume F = 96,500 A s/mol. Calculate the time in minutes. The time taken to corrode the metal is (___) min. (*Show up to the 2nd decimal place) 신 2. A mild steel tank 60 cm high with a 30 cm x 30 cm square bottom is filled with aerated water up to the 45 cm level and shows a corrosion loss of 600 g over a four- week period. Assume that mild steel corrodes in the same way as pure iron, and the atomic mass of iron is 55.845 g/mol. 2-A. Convert the time in sec. t = [____] × 106 sec (*Show up to 4th decimal place) 2-B. Calculate the corrosion current. /= [___] A (*Show up to 4th decimal place) A 2-C. The surface area of the corroded surface is calculated as follows: Surface area of corroded surface = 4(S × H) + (S× S), where S refers to the side of the tank and H refers to the level of water in the tank. Calculate the current density associated with the corrosion current. Assume that corrosion occurs uniformly over all the surfaces of the steel tank. Surface area of corroded surface = [___] cm² Current density associated with the corrosion current = [_] × 10-4 A/cm² ("Show up to 4th decimal place) P
According to Faraday's equation, W = ItM nF , where w = weight of metal corroded or electroplated in aqueous solution in time t, /= current flow, M = atomic mass of the metal in g/mol, n = number of electrons produced/consumed in the process, and F = Faraday's constant. 1. The anodic reaction that occurs at the cadmium electrode is as follows: Cd → Cd2+ + 2e. A cadmium electroplating process uses 30 A of current to chemically corrode a cadmium anode. If it is assumed that there are no side reactions, how long will it take to corrode 9 g of cadmium from the anode? The atomic mass of cadmium is 112.414 g/mol. Assume F = 96,500 A s/mol. Calculate the time in minutes. The time taken to corrode the metal is (___) min. (*Show up to the 2nd decimal place) 신 2. A mild steel tank 60 cm high with a 30 cm x 30 cm square bottom is filled with aerated water up to the 45 cm level and shows a corrosion loss of 600 g over a four- week period. Assume that mild steel corrodes in the same way as pure iron, and the atomic mass of iron is 55.845 g/mol. 2-A. Convert the time in sec. t = [____] × 106 sec (*Show up to 4th decimal place) 2-B. Calculate the corrosion current. /= [___] A (*Show up to 4th decimal place) A 2-C. The surface area of the corroded surface is calculated as follows: Surface area of corroded surface = 4(S × H) + (S× S), where S refers to the side of the tank and H refers to the level of water in the tank. Calculate the current density associated with the corrosion current. Assume that corrosion occurs uniformly over all the surfaces of the steel tank. Surface area of corroded surface = [___] cm² Current density associated with the corrosion current = [_] × 10-4 A/cm² ("Show up to 4th decimal place) P
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...
Related questions
Question
![According to Faraday's equation, W =
ItM
nF
, where w = weight of metal
corroded or electroplated in aqueous solution in time t, /= current flow, M = atomic
mass of the metal in g/mol, n = number of electrons produced/consumed in the
process, and F = Faraday's constant.
1. The anodic reaction that occurs at the cadmium electrode is as follows: Cd →
Cd2+ + 2e. A cadmium electroplating process uses 30 A of current to chemically
corrode a cadmium anode. If it is assumed that there are no side reactions, how long
will it take to corrode 9 g of cadmium from the anode?
The atomic mass of cadmium is 112.414 g/mol. Assume F = 96,500 A s/mol.
Calculate the time in minutes.
The time taken to corrode the metal is (___) min.
(*Show up to the 2nd decimal place)
신
2. A mild steel tank 60 cm high with a 30 cm x 30 cm square bottom is filled with
aerated water up to the 45 cm level and shows a corrosion loss of 600 g over a four-
week period. Assume that mild steel corrodes in the same way as pure iron, and the
atomic mass of iron is 55.845 g/mol.
2-A. Convert the time in sec. t = [____] × 106 sec (*Show up to 4th decimal place)
2-B. Calculate the corrosion current. /= [___] A (*Show up to 4th decimal place)
A
2-C. The surface area of the corroded surface is calculated as follows:
Surface area of corroded surface = 4(S × H) + (S× S), where S refers to the side of
the tank and H refers to the level of water in the tank.
Calculate the current density associated with the corrosion current. Assume that
corrosion occurs uniformly over all the surfaces of the steel tank.
Surface area of corroded surface = [___] cm²
Current density associated with the corrosion current = [_] × 10-4 A/cm²
("Show up to 4th decimal place)
P](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F093e7116-3e01-49ad-9157-7a22a5caeb16%2F690e5782-6bd8-45f7-b3e3-d6d2b45ccea4%2Fjuqzig_processed.png&w=3840&q=75)
Transcribed Image Text:According to Faraday's equation, W =
ItM
nF
, where w = weight of metal
corroded or electroplated in aqueous solution in time t, /= current flow, M = atomic
mass of the metal in g/mol, n = number of electrons produced/consumed in the
process, and F = Faraday's constant.
1. The anodic reaction that occurs at the cadmium electrode is as follows: Cd →
Cd2+ + 2e. A cadmium electroplating process uses 30 A of current to chemically
corrode a cadmium anode. If it is assumed that there are no side reactions, how long
will it take to corrode 9 g of cadmium from the anode?
The atomic mass of cadmium is 112.414 g/mol. Assume F = 96,500 A s/mol.
Calculate the time in minutes.
The time taken to corrode the metal is (___) min.
(*Show up to the 2nd decimal place)
신
2. A mild steel tank 60 cm high with a 30 cm x 30 cm square bottom is filled with
aerated water up to the 45 cm level and shows a corrosion loss of 600 g over a four-
week period. Assume that mild steel corrodes in the same way as pure iron, and the
atomic mass of iron is 55.845 g/mol.
2-A. Convert the time in sec. t = [____] × 106 sec (*Show up to 4th decimal place)
2-B. Calculate the corrosion current. /= [___] A (*Show up to 4th decimal place)
A
2-C. The surface area of the corroded surface is calculated as follows:
Surface area of corroded surface = 4(S × H) + (S× S), where S refers to the side of
the tank and H refers to the level of water in the tank.
Calculate the current density associated with the corrosion current. Assume that
corrosion occurs uniformly over all the surfaces of the steel tank.
Surface area of corroded surface = [___] cm²
Current density associated with the corrosion current = [_] × 10-4 A/cm²
("Show up to 4th decimal place)
P
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by step
Solved in 2 steps
Recommended textbooks for you
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY