Anonymous

Question description

The equilibrium constant for HI decomposition at 500 °C is 5.8×10-3.
2HI(g)  H2(g) + I2(g)
At that temperature reactants and products are gaseous. (There is no change in the total number of moles, so Kc = Kp.)
A sample of 0.43 mol of HI is placed in a 1.00 L vessel which is then heated to 500 °C. When equilibrium is reached, what is the molar concentration of H2? (Give units).
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Iodine is sparingly soluble in pure water. However, it does `dissolve' in solutions containing excess iodide ion because of the following reaction:

 I-(aq) + I2(aq) I3-(aq) K = 710

For each of the following cases calculate the equilbrium ratio of [I3-] to [I2].

5.00×10-2 mol of I2 is added to 1.00 L of 5.00×10-1 M KI solution.

The solution above is diluted to 12.00 L.

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