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2- Consider the following reaction at a certain temperature: 4Fe(s) + 302 (g)→2Fe2O3 (s) An equilibrium mixture contains 1.0 mole of Fe, 1.0 ×10³ mole of O2, and 2.0 moles of Fe2O; all in a 2.0-L container. Calculate the value of K for this reaction.

2- Consider the following reaction at a certain temperature: 4Fe(s) + 302 (g)→2Fe2O3 (s) An equilibrium mixture contains 1.0 mole of Fe, 1.0 ×10³ mole of O2, and 2.0 moles of Fe2O; all in a 2.0-L container. Calculate the value of K for this reaction.

Chemistry
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
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2- Consider the following reaction at a certain temperature: 4Fe(s) + 302 (g)→2Fe2O3 (s) An equilibrium mixture contains 1.0 mole of Fe, 1.0 ×10³ mole of O2, and 2.0 moles of Fe2O; all in a 2.0-L container. Calculate the value of K for this reaction.
Transcribed Image Text:2- Consider the following reaction at a certain temperature: 4Fe(s) + 302 (g)→2Fe2O3 (s) An equilibrium mixture contains 1.0 mole of Fe, 1.0 ×10³ mole of O2, and 2.0 moles of Fe2O; all in a 2.0-L container. Calculate the value of K for this reaction.
Expert Solution
Step 1

Given:

Number of moles of Fe= 1.0 mole

Number of moles of O2= 1.0 x 10-3 mole

Number of moles of Fe2O3= 2.0 moles

Volume of flask= 2.00 L

Chemistry homework question answer, step 1, image 1

 

Step 2

To calculate K for the reaction:

First we have to calculate concentration of Fe, O2 and Fe2O3,

Chemistry homework question answer, step 2, image 1

 

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