Problem: At a particular temperature, K = 4.0 x 10 -7 for the reactionN2O4(g) ⇌ 2NO2(g)In an experiment, 1.0 mole of N2O4 is placed in a 10.0-L vessel. Calculate the concentrations of N2O4 and NO2 when this reaction reaches equilibrium.

FREE Expert Solution

We are asked to calculate the concentrations of N2O4 and NO2 when this reaction reaches equilibrium.


Step 1. Calculate molarity N2O4

M N2O4 = molLM N2O4 =1 mol N2O410 L

M  N2O4 = 0.1 M


Step 2. Set up ICE chart



Step 3. Calculate molarity in equilibrium


K = [NO2]2[N2O4]4.0 × 10-7 = [2x]2[0.1-x]

x is negligible in the denominator since K is very small. 


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Problem Details

At a particular temperature, K = 4.0 x 10 -7 for the reaction

N2O4(g) ⇌ 2NO2(g)

In an experiment, 1.0 mole of N2O4 is placed in a 10.0-L vessel. Calculate the concentrations of N2O4 and NO2 when this reaction reaches equilibrium.


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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 ICE Chart concept. You can view video lessons to learn ICE Chart. Or if you need more ICE Chart practice, you can also practice ICE Chart practice problems.

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 Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.