Question
Asked Mar 25, 2020
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The particulate model below represents the redox reactions that produce energy from fuel cells. Use the model to answer the following questions. 

 

Write a balanced half-cell equation for the reaction occurring at the anode. Ignore phases in the reaction.

 

Write a balanced half-cell equation for the reaction occurring at the cathode. Ignore phases in the reaction. 

 

Assuming excess oxygen, how many moles of electrons would be transferred if 22 moles of H2 were reacted. 

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sw5_23910_1.jpg (700x x
b My Questions | bartleby x
o Calculate the standard x
G How many liters of 02
х
A sw5.wwnorton.com/problemsets/filemanager/userfiles/ctcox@stanford.edu/sw5_23910_1.jpg
2:01 PM
O Type here to search
3/25/2020
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X For Life | Xfinity Stre x Smartwork5 sw5_23910_1.jpg (700x x b My Questions | bartleby x o Calculate the standard x G How many liters of 02 х A sw5.wwnorton.com/problemsets/filemanager/userfiles/ctcox@stanford.edu/sw5_23910_1.jpg 2:01 PM O Type here to search 3/25/2020

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Expert Answer

Introduction

Redox reactions possess two half-reactions in which one reaction occurs at anode named as oxidation reaction and another one reaction occurs at cathode named as reduction reaction.

Solution

The product formed in the reaction in the fuel cell is water.

The balanced half-cell equation taking place at the anode is shown below.

Chemistry homework question answer, step 2, image 1

In the above reaction, the oxidation state of hydrogen changes from 0 to +1. It is getting oxidized by releasing 2 electrons at the anode.  In the fuel cell, hydrogen molecules get oxidized to hydronium ions. Thus half-reaction is the oxidation reaction.

The balanced half-cell equation taking place at the cathode is shown below.

Chemistry homework question answer, step 2, image 2

In the above reaction, the oxidation state of oxygen changes from 0 to -2. In the fuel cell, the oxygen molecules are getting reduced at the cathode ...

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