When the following reaction comes to equilibrium, will the concentrations of the reactants or products be greater? does the answer to this question depend on the initial concentrations of the reactants and products? a(g)+b(g)⇌2c(g)kc=1.4×10−5 match the words in the left column to the appropriate blanks in the sentences on the right. the value of the equilibrium constant is relatively ; therefore, the concentration of reactants will be the concentration of products. this result is the initial concentration of the reactants and products.

At equilibrium, the concentration of the reactants will be greater than the concentration of the products. This does not depend on the initial concentrations of the reactants and products.

Explanation:

The value of Kc gives us an idea of the extent of the reaction. A big Kc (Kc > 1) means that in the equilibrium there are more products than reactants, and the opposite happens for a small Kc (Kc < 1). The equilibrium is reached no matter what the initial concentrations are.

The value of the equilibrium constant is relatively SMALL; therefore, the concentration of reactants will be GREATER THAN the concentration of products. This result is INDEPENDENT OF the initial concentration of the reactants and products.

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explanation:

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the answer is the first option

explanation:

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