At a certain temperature, nitogen and hydrogen react to form ammonia: N_2(g) + 3H_2(g)...


At a certain temperature, nitogen and hydrogen react to form ammonia:

{eq}N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) . {/eq}

When initial amounts of {eq}N_2 ,\ H_2 {/eq} ,and {eq}NH_3 {/eq} are mixed, the concentration of {eq}NH_3 {/eq} increases. Which statement below is TRUE?

A. {eq}K_c \gt Q {/eq}

B. {eq}K_c = Q {/eq}

C. {eq}K_c \lt Q {/eq}

D. More information is needed to make a statement about {eq}K_c {/eq}.

Relation Between the Equilibrium Concentrations

When a chemical system is in perfect equilibrium, it means that the reactants are continuously reacting to form products, and the products are simultaneously decomposing to form the reactants. The reversible arrow is used to depict such a scenario. The equilibrium constant, K, can be written for this system. However, any change in the concentrations of the species results in a shift from the equilibrium position. The reaction quotient, Q, is affected and, based on Le Chatelier's Principle, the direction of shift is such as to restore the value of Q to K.

Answer and Explanation: 1

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The equilibrium constant can be written as:

{eq}\displaystyle K_c = \frac{[products]}{[reactants]} {/eq}.

Now, we are told that for the given...

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Equilibrium Constant (K) and Reaction Quotient (Q)


Chapter 11 / Lesson 3

Understand equilibrium constant and reaction quotient and their definitions. Learn their symbols and differences, how to calculate Q and K, and see examples.

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