How can one tell a reaction has reached equilibrium?

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How can one tell a reaction has reached equilibrium?

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Answer 1 · 2017-03-09T22:22:30

When the rate of forward reaction is equal to the rate of reverse reaction.

Explanation:

For the generalized equilibrium we have:

$A + B ⇌ C + D$ $A+BrightleftharpoonsC+D$

Now we have a rate forward,

$k_{f} [A] [B]$ $k_f[A][B]$ , and a rate backwards, $k_{r} [C] [D]$ $k_r[C][D]$ .

$k_{f}$ $k_f$ and $k_{r}$ $k_r$ are unspecified rate constants, whose ratio must be determined by measurement.

The condition of chemical equilibrium is reached when,

$rate forward \equiv rate backwards$ $"rate forward "-=" rate backwards"$ ,

i.e. $\frac{[C] [D]}{[A] [B]} = \frac{k_{f}}{k_{r}} = K_{eq}$ $([C][D])/([A][B])=k_f/k_r=K_"eq"$ .

$K_{eq}$ $K_"eq"$ is the thermodynamic equilibrium constant, WHICH must be measured for a given reaction, and for a given temperature. Because chemical change is conceived to continue even after equilibrium is reached, even tho $net chemical change$ $"net chemical change"$ is nil, this is labelled as $dynamic chemical equilibrium.$ $"dynamic chemical equilibrium."$ After equilibrium is reached, NO NET CHEMICAL CHANGE OCCURS.

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How can one tell a reaction has reached equilibrium?

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