The reaction of hydrogen gas and nitrogen gas to form ammonia is a well-known process that is an important reaction in industry. The equilibrium reaction is shown below. 2 NO2) N2O4 (2) AH=-57 kJ (colorless) (brown) 1. If more NO2 is added to the system, how will that affect the concentration of N204? Support your explanation using Le Chatelier's principle. 2. If the temperature is increased, how will that affect the concentration of the product, N204? What observations would you expect to see if you performed this experiment in the laboratory. Support your explanation using Le Chatelier's principle. 3. If the pressure on the system is increased, how will that affect the concentration of the product, N2O4? 4. Besides changing temperature, pressure, or NO2 concentration, what is another way to get this reaction to produce more N204?

The reaction of hydrogen gas and nitrogen gas to form ammonia is a well-known process that is an important reaction in industry. The equilibrium reaction is shown below. 2 NO2) N2O4 (2) AH=-57 kJ (colorless) (brown) 1. If more NO2 is added to the system, how will that affect the concentration of N204? Support your explanation using Le Chatelier's principle. 2. If the temperature is increased, how will that affect the concentration of the product, N204? What observations would you expect to see if you performed this experiment in the laboratory. Support your explanation using Le Chatelier's principle. 3. If the pressure on the system is increased, how will that affect the concentration of the product, N2O4? 4. Besides changing temperature, pressure, or NO2 concentration, what is another way to get this reaction to produce more N204?

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

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Concept explainers

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Exergonic Reaction

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Question

The reaction of hydrogen gas and nitrogen gas to form ammonia is a well-known process that is
an important reaction in industry. The equilibrium reaction is shown below.
2 NO2@) N204 ()
AH= -57 kJ
(colorless)
(brown)
1. If more NO2 is added to the system, how will that affect the concentration of N2O4?
Support your explanation using Le Chatelier's principle.
2. If the temperature is increased, how will that affect the concentration of the product,
N2O4? What observations would you expect to see if you performed this experiment in
the laboratory. Support your explanation using Le Chatelier's principle.
3. If the pressure on the system is increased, how will that affect the concentration of the
product, N2O4?
4. Besides changing temperature, pressure, or NO2 concentration, what is another way to get
this reaction to produce more N2O4?

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