In an electroplating process, copper (ionic charge +2e, atomic weight 63.6 g/mol) is deposited using a...
Homework Answers
Here Charge passes, Q = It = 10*10*60
= 6000 C
1 atom require charge to Deposited = 2*1.6*10^-19
Therefore
No. of Atoms Deposited = (6000)/(2*1.6*10^-19)
= 1.875*10^22 atoms
Therefore
No. of Moles Deposited = (1.875*10^22)/(6.023*10^23)
= 0.03113 moles
1 mole of Copper has mass = 63.5 g
Therefore
Mass of Copper Deposited = 63.5*0.03113
= 1.98 g
So E option is Correct.
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In an electroplating process, copper (ionic charge +2e, atomic weight 63.6 g/mol) is deposited using a...
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Electroplating Postlab Questions 1. Suppose that you have the opportunity to be the first in the world to come up witha your data for the number of Coulombs of charge passed and the number of moles of value of Faraday's constant -never mind we al ready know it is 96485 C/mol e. Using copper actually lost from the copper electrode in your experiment, what would you predict for the value of Faradays constant? Show your work. What is the percent...
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Question 3 [20 points 1. Copper sulfide is produced when copper and sulfur are heated together Use the data below, obtained after the heating process, to determine the empirical formula of this compound. Molar masses (e/mol) c S 32.06. 18 points) befor 1 Mass of crucible cover copper (B) 2 Mass of crucible + cover (g) 3 Mass of copper (B) 4 Mass of crucible cover + copper sulfide at constant weight (8)40.23 S Mass of copper sulfide (8) 6...
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Please use railroad tracks for work, thank you.
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