From the result above, the cell potentialfor the corrosion of copper is very lowcompared to iron. Theoxidation/corrosion of copper is a LESSspontaneous reaction compared to theRESULT FOR NAIL Aoxidation/corrosion of iron. Therefore,ironmore prone to oxidationcompared to copper. We can say thatiron is a more active metal than copper.Using the result for Nail C:From the result above, the cell potentialThe added potassium ferricyanidefor the corrosion of Zinc is higher thaniron. The oxidation/corrosion of copper(Fe(CN)6³) in the agar turns Prussianblue when it reacts with Fe2+ in theis a MORE spontaneous reactioncompared to the oxidation/corrosion ofiron. Therefore, zinc is more prone tosolution to produce iron (II)oxidation compared to iron. We can sayhexacyanoferrate (III):that zinc is a more active metal thaniron.Fe 2* (aq)Fe(CN),³-(aq)+Fez[Fe(CN)6]2 (Prussian blue)Using the result for Nail D: Arrange the following ions in terms ofincreasing strength as an oxidizingagent.Arrange the three metals in termsof increasing strength as a reducingO Fe2+ < Cu²+ < Zn²+agent.Cu2+ < Zn²+ < Fe2+Recall:O Fe2+ < Zn²+ < Cu²+O Cu²+ < Fe2+ < Zn²+ARALEO - Anode: Reducing AgentLosses Electron, process is calledO Zn²+ < Fe²+ < Cu²+OxidationO Zn2+ < Cu2+< Fe2+COAGER - Cathode: Oxidizing AgentGains Electron, process is calledReductionArrange the three metals in terms ofincreasing ability to undergo oxidationO Fe < Cu < Znbased on the observations in nails A, Cand D.O Fe < Zn < CuO Cu < Zn < FeO Cu < Fe < ZnO Zn < Fe < CuくO Fe < Cu < ZnO Cu < Zn < FeO Fe < Zn < CuO Zn < Cu < FeO Zn < Cu < FeO Zn < Fe < CụO Cu < Fe < Zn

Answered: Image /qna-images/answer/0800c348-b5a0-4033-990f-c935d96524eb.jpg

Arrange the following ions in terms of increasing strength as an oxidizing agent. Arrange the three metals in terms of increasing strength as a reducing O Fe2+ < Cu2+ < Zn2+ く agent. O Cu2+ < Zn2+ < Fe2+ Recall: O Fe2+ < Zn2+ < Cu²+ O Cu2+ < Fe2+ < Zn²+ ARALEO - Anode: Reducing Agent Losses Electron, process is called OZn2+ < Fe2+ < Cu²+ Oxidation O Zn2+ < Cu2+< Fe2+ COAGER - Cathode: Oxidizing Agent Gains Electron, process is called Reduction Arrange the three metals in terms of increasing ability to undergo oxidation O Fe < Cu < Zn based on the observations in nails A, C and D. O Fe < Zn < Cu Cu < Zn < Fe O Cu < Fe < Zn Zn < Fe < Cu O Fe < Cu < Zn O Cu < Zn < Fe O Fe < Zn < Cu Zn < Cu < Fe O Zn < Cu < Fe O Zn < Fe < Cu O Cu < Fe < Zn

Arrange the following ions in terms of increasing strength as an oxidizing agent. Arrange the three metals in terms of increasing strength as a reducing O Fe2+ < Cu2+ < Zn2+ く agent. O Cu2+ < Zn2+ < Fe2+ Recall: O Fe2+ < Zn2+ < Cu²+ O Cu2+ < Fe2+ < Zn²+ ARALEO - Anode: Reducing Agent Losses Electron, process is called OZn2+ < Fe2+ < Cu²+ Oxidation O Zn2+ < Cu2+< Fe2+ COAGER - Cathode: Oxidizing Agent Gains Electron, process is called Reduction Arrange the three metals in terms of increasing ability to undergo oxidation O Fe < Cu < Zn based on the observations in nails A, C and D. O Fe < Zn < Cu Cu < Zn < Fe O Cu < Fe < Zn Zn < Fe < Cu O Fe < Cu < Zn O Cu < Zn < Fe O Fe < Zn < Cu Zn < Cu < Fe O Zn < Cu < Fe O Zn < Fe < Cu O Cu < Fe < Zn

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...

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Concept explainers

Potentiometric Titrations

Potentiometric titration is one of the important titration methods and is mainly carried out to characterize acid solutions. It follows a method similar to that of the normal titration technique, but the main difference is that there is no indicator used in the potentiometric titrations. Instead of using an indicator, electrodes are employed for monitoring the whole titration process. A scientist named Robert Behrend did the potentiometric titration for the first time, and it was done using the mercurous solution and potassium chloride.

Question

From the result above, the cell potential
for the corrosion of copper is very low
compared to iron. The
oxidation/corrosion of copper is a LESS
spontaneous reaction compared to the
RESULT FOR NAIL A
oxidation/corrosion of iron. Therefore,
iron
more prone to oxidation
compared to copper. We can say that
iron is a more active metal than copper.
Using the result for Nail C:
From the result above, the cell potential
The added potassium ferricyanide
for the corrosion of Zinc is higher than
iron. The oxidation/corrosion of copper
(Fe(CN)6³) in the agar turns Prussian
blue when it reacts with Fe2+ in the
is a MORE spontaneous reaction
compared to the oxidation/corrosion of
iron. Therefore, zinc is more prone to
solution to produce iron (II)
oxidation compared to iron. We can say
hexacyanoferrate (III):
that zinc is a more active metal than
iron.
Fe 2* (aq)
Fe(CN),³-
(aq)
+
Fez[Fe(CN)6]2 (Prussian blue)
Using the result for Nail D:

Arrange the following ions in terms of
increasing strength as an oxidizing
agent.
Arrange the three metals in terms
of increasing strength as a reducing
O Fe2+ < Cu²+ < Zn²+
agent.
Cu2+ < Zn²+ < Fe2+
Recall:
O Fe2+ < Zn²+ < Cu²+
O Cu²+ < Fe2+ < Zn²+
ARALEO - Anode: Reducing Agent
Losses Electron, process is called
O Zn²+ < Fe²+ < Cu²+
Oxidation
O Zn2+ < Cu2+< Fe2+
COAGER - Cathode: Oxidizing Agent
Gains Electron, process is called
Reduction
Arrange the three metals in terms of
increasing ability to undergo oxidation
O Fe < Cu < Zn
based on the observations in nails A, C
and D.
O Fe < Zn < Cu
O Cu < Zn < Fe
O Cu < Fe < Zn
O Zn < Fe < Cu
く
O Fe < Cu < Zn
O Cu < Zn < Fe
O Fe < Zn < Cu
O Zn < Cu < Fe
O Zn < Cu < Fe
O Zn < Fe < Cụ
O Cu < Fe < Zn

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