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wbrandi118
22.03.2021 •
Chemistry
QUESTION 6 Consider the following reaction between the diatomic and monatomic forms of iodine: I2 (g) <-> 2I (g) When 0.095 M I2 is initially placed in a previously empty container and sealed, the system slowly reaches equilibrium. When equilibrium is reached, it is found that there is an equilibrium concentration of 0.0055 M of the monatomic form of iodine. Calculate the (unitless) equilibrium constant Kc. Round your answer to two sig figs, and express it in scientific notation.
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Ответ:
The equilibrium constant is![3.3\times 10^{-4}](/tpl/images/1211/7332/b1ebc.png)
Explanation:
Initial concentration of
= 0.095 M
The given balanced equilibrium reaction is,
Initial conc. 0.095 M 0 M
At eqm. conc. (0.095-x) M (2x) M
Given : 2x = 0.0055
x = 0.00275
The expression for equilibrium constant for this reaction will be,
Now put all the given values in this expression, we get :
Thus the equilibrium constant is![3.3\times 10^{-4}](/tpl/images/1211/7332/b1ebc.png)
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