Write the balanced chemical equation for the reaction/equilibrium between hydrogen gas and nitrogen gas to produce gaseous ammonia.Write the Qc, Kc , and Kp expressions for above equilibrium and briefly explain the difference between the three.Recall that temperature (T) is a measure of kinetic energy. With respect to gases, this refers to the frequency of the collisions between gaseous particles. Compare the kinetic energy of the reactants to the products in this equilibrium. Which side has the greater or lesser kinetic energy based on the total number of gas particles? Recall that LeChatelier’s principle states that an equilibrium will respond to an external change/force/stress to maintain the equilibrium. Let’s look at two examples.If the T (thus KE) is increased, in which direction would the equilibrium shift?The reaction is exothermic (DH = -92.2 kJ which you could calculate) and, thus, heat is treated as a product. Thus, is it better to heat or cool the reaction to produce more ammonia?In what ways are the above two effects complementary or contradictory?

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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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Write the balanced chemical equation for the reaction/equilibrium between hydrogen gas and nitrogen gas to produce gaseous ammonia.
Write the Q_c, K_c , and K_pexpressions for above equilibrium and briefly explain the difference between the three.
Recall that temperature (T) is a measure of kinetic energy. With respect to gases, this refers to the frequency of the collisions between gaseous particles. Compare the kinetic energy of the reactants to the products in this equilibrium. Which side has the greater or lesser kinetic energy based on the total number of gas particles?
Recall that LeChatelier’s principle states that an equilibrium will respond to an external change/force/stress to maintain the equilibrium. Let’s look at two examples.
- If the T (thus KE) is increased, in which direction would the equilibrium shift?
- The reaction is exothermic (DH = -92.2 kJ which you could calculate) and, thus, heat is treated as a product. Thus, is it better to heat or cool the reaction to produce more ammonia?
- In what ways are the above two effects complementary or contradictory?

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