I mainly need the last one. The others I have right. The last one is not 1.55hrs so please find me the right answer. Thank you! for the electrolysis of molten chromium bromide (CrBr,). Identify the reaction that occurs at the anode and the cathode.anode: 2 BrBr2 + 2 e vcathode: Cr³ + 3 eCrDetermine the minimum voltage that must be applied to a cell containing molten CrBr, inorder for electrolysis to occur.1.83VIf 3.65 A is applied for 85 minutes, what mass of Cr(s) will be produced?3-3g CrIf 15.00 A of current is applied, how long would it take to produce 25.0 g of Cr(s)?hr

Given: Electrolysis of molten chromium bromide Current=15.00 A Mass of Cr=25.0 g To Find: Time…

Answered: If 15.00 A of current is applied, how…

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If 15.00 A of current is applied, how long would it take to produce 25.0 g of Cr(s)? hr

Introductory Chemistry: An Active Learning Approach

6th Edition

ISBN:9781305079250

Author:Mark S. Cracolice, Ed Peters

Publisher:Mark S. Cracolice, Ed Peters

Chapter19: Oxidation-reduction(electron Transfer) Reactions

Section: Chapter Questions

Problem 14E

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Question

I mainly need the last one. The others I have right. The last one is not 1.55hrs so please find me the right answer. Thank you!

for the electrolysis of molten chromium bromide (CrBr,).

Identify the reaction that occurs at the anode and the cathode.
anode: 2 Br
Br2 + 2 e v
cathode: Cr³ + 3 e
Cr
Determine the minimum voltage that must be applied to a cell containing molten CrBr, in
order for electrolysis to occur.
1.83
V
If 3.65 A is applied for 85 minutes, what mass of Cr(s) will be produced?
3-3
g Cr
If 15.00 A of current is applied, how long would it take to produce 25.0 g of Cr(s)?
hr

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