Problem: Consider the reaction2 NO2 (g) ⇌ N2O4 (g)For each of the following mixtures of reactants and products at 25°C, predict the direction in which the reaction will shift to reach equilibrium. c. PNO2 = 0.29 atm, PN2O4 = 1.6 atm

🤓 Based on our data, we think this question is relevant for Professor Castaneda's class at UMICH.

FREE Expert Solution

Recall that effect of the change in pressure to the equilibrium according to Le Chatelier's Principle:

  • Increasing the pressure → reaction towards the side with fewer moles of gas.
  • Decreasing the pressure → reaction towards the side with more moles of gas.


The reaction at equilibrium: 2 NO2(g) ⇌ N2O4(g)

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Problem Details

Consider the reaction

2 NO2 (g) ⇌ N2O4 (g)

For each of the following mixtures of reactants and products at 25°C, predict the direction in which the reaction will shift to reach equilibrium. 

c. PNO2 = 0.29 atm, PN2O4 = 1.6 atm

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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 Le Chatelier's Principle concept. You can view video lessons to learn Le Chatelier's Principle . Or if you need more Le Chatelier's Principle practice, you can also practice Le Chatelier's Principle practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Castaneda's class at UMICH.

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.