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

Question

In the following chemical reaction A and B react within a closed system, reversbly, 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 foe K_o? d) You stort this reaction with ONLV the reactants A and B. Can dynamic equilibrium still be achieved (is yes. Please explain why)?

Explanation / Answer

A(aq) + B(aq) <------> C(aq) + D(aq)

In dynamic equilibrium, the rate of formation of reactants = rate of formation of products

Keq = {[C]*[D]}/{[A]*[B]}

Higher the value of Keq, greater is the concentration of products and vice-versa.

Yes, dynamic equilibrium will still be achieved when only the reactants are present initially as to reach the equilibrium state, A & B has to react to form C & D and all 4 has to achieve the equilibrium concentration.

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