Solve all parts otherwise I will downvote Part A: Spontaneity of redox reaction1. Use the standard electrode potentials to calculate the cell potential and determine whetherthe reaction is spontaneous or non-spontaneous. Explain your answers.a) Au3+ + 3 Fe2+ → 3 Fe3+ + Aub) Pb + So,2 + H20 → Pb2* + SO,2 + 2 OH-2. Given the following lab dataSn2* + NiSpontaneousNi2+FeSpontaneousCr2++ FeNon spontaneousa) Rank the oxidizing agents in decreasing order of strength.b) Rank the reducing agents in decreasing order of strength.c) Will Sn2* react with Cr? Explain?d) Will Fe2* react with Sn? ExplainPart B: Faraday's LawCalculate the time required to produce 23.0 g of nickel from the electrolysis of NiCl2tq) by usinga current of 15.0 A. Sketch this cell labeling the anode and the cathode and showing the flow ofions.

Since you've asked multiple questions with multiple sub-parts, we will solve first question (1,a and…

1. Use the standard electrode potentials to calculate the cell potential and determine whether the reaction is spontaneous or non-spontaneous. Explain your answers. a) Au3+ + 3 Fe2+ → 3 Fe3+ + Au b) Pb + SO,2 + H20 Pb2 + so, + 2 OH

1. Use the standard electrode potentials to calculate the cell potential and determine whether the reaction is spontaneous or non-spontaneous. Explain your answers. a) Au3+ + 3 Fe2+ → 3 Fe3+ + Au b) Pb + SO,2 + H20 Pb2 + so, + 2 OH

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 18.46QE

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Question

Solve all parts otherwise I will downvote

Part A: Spontaneity of redox reaction
1. Use the standard electrode potentials to calculate the cell potential and determine whether
the reaction is spontaneous or non-spontaneous. Explain your answers.
a) Au3+ + 3 Fe2+ → 3 Fe3+ + Au
b) Pb + So,2 + H20 → Pb2* + SO,2 + 2 OH-
2. Given the following lab data
Sn2* + Ni
Spontaneous
Ni2+
Fe
Spontaneous
Cr2+
+ Fe
Non spontaneous
a) Rank the oxidizing agents in decreasing order of strength.
b) Rank the reducing agents in decreasing order of strength.
c) Will Sn2* react with Cr? Explain?
d) Will Fe2* react with Sn? Explain
Part B: Faraday's Law
Calculate the time required to produce 23.0 g of nickel from the electrolysis of NiCl2tq) by using
a current of 15.0 A. Sketch this cell labeling the anode and the cathode and showing the flow of
ions.

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