Problem: Consider the following reaction at a certain temperature:4Fe(s) + 3O2(g) ⇌ 2Fe2O3(s)An equilibrium mixture contains 1.0 mole of Fe, 1.0 x 10-3 mole of O2, and 2.0 moles of Fe2O3 all in a 2.0-L container. Calculate the value of K for this reaction.

🤓 Based on our data, we think this question is relevant for Professor Raja's class at STATEN ISLAND CUNY.

FREE Expert Solution

Recall that the equilibrium constant is the ratio of the products and reactants


We use Kp when dealing with pressure and Kc when dealing with concentration:


Kp=PproductsPreactants     Kc=[products][reactants]


Note that solid and liquid compounds are ignored in the equilibrium expression.


Molarity(M)=moles of soluteLiters of solution


The Kc expression for the reaction is:


Kc=[products][reactants]=1[O2]3


[O2]=1.0×10-3 mol O22.0 L5.0 x 10-4 M


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Problem Details

Consider the following reaction at a certain temperature:

4Fe(s) + 3O2(g) ⇌ 2Fe2O3(s)

An equilibrium mixture contains 1.0 mole of Fe, 1.0 x 10-3 mole of O2, and 2.0 moles of Fe2O3 all in a 2.0-L container. Calculate the value of K for this reaction.

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Equilibrium Expressions concept. If you need more Equilibrium Expressions practice, you can also practice Equilibrium Expressions practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Raja's class at STATEN ISLAND CUNY.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl 2nd Edition practice problems.