In the following chemical reaction A and B react within a closed system, reversi

Question

In the following chemical reaction A and B react within a closed system, reversibly, to form the products C and D. A state of dynamic equilibrium will eventually be established. a) Explain the concept of dynamic equilibrium and the significance of having a closed system. b) Write the equilibrium constant expression for this reaction. c) What is the significance of a "high" or "low" value for K_c? d) You start this reaction with ONLY the reactants A and B. Can dynamic equilibrium still be achieved (if yes, please explain why)?

Explanation / Answer

a) dynamic equilibrium is an equilibirum in which there is actually reactions between reactants and products, but since they react in the same rate, i.e. backward vs. forward is overall rate = 0; we consider this to be in euqilibrium

b)

K = [C][D]/([A][B])

c)

high K, means it favours products

low K, it favours reactants

d)

YES, since they will react to form some of product until K is achived

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