How do you calculate the Keq of a reaction?

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How do you calculate the Keq of a reaction?

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Answer 1 · 2017-06-17T17:38:23

These are not $calculated$ $"calculated"$ , but $MEASURED$ $"MEASURED"$ .

Explanation:

For the reaction........

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

There is a $rate forward$ $"rate forward"$ , $k_{f} [A] [B]$ $k_f[A][B]$ , where $k_{f}$ $k_f$ is some constant....

And a $rate backwards$ $"rate backwards"$ , $k_{r} [C] [D]$ $k_r[C][D]$ , where $k_{r}$ $k_r$ is some other constant....

Now, by definition, a condition of $chemical equilibrium$ $"chemical equilibrium"$ occurs not when chemical change ceases, but when there is equality of forward and reverse rates, and thus.........

$rate backwards$ $"rate backwards"$ , $k_{r} [C] [D] \equiv rate forwards$ $k_r[C][D]-="rate forwards"$ , $k_{f} [A] [B]$ $k_f[A][B]$ . And so we take the quotient......

$\frac{k_{r}}{k_{f}} = \frac{[C] [D]}{[A] [B]}$ $k_r/k_f=([C][D])/([A][B])$

We more commonly call the quotient $\frac{k_{r}}{k_{f}}$ $k_r/k_f$ , $K_{c}$ $K_c$ , the thermodynamic equilibrium constant.

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How do you calculate the Keq of a reaction?

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