Dynamic equilibrium - <P> In the reaction of...

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<P> In the reaction of H<sub>2</sub> (g) + I<sub>2</sub>(g) ↔ 2 HI(g), one molecule of hydrogen reacts with another molecule of iodine to form hydrogen iodide, simultaneously one molecule of hydrogen iodide collides with another molecule of hydrogen iodide and reproduces the products. The red and yellow balls will denote any of the reactants, while the blue and green balls denote the one product. These reactions continue until the rate at which the products are formed equals the rate at which the reactants form, this is called dynamic equilibrium. At this point, the reaction does not stop, instead it continues but the forward and reverse reactions equal one another, and for the naked eye it appears the container is unchanged (for solutions only, gases are invisible).</P> <P> However, this situation of equilibrium can be observed through several variables that impact its attainment. The concentrations of the reactants, in this case the partial pressures, which are H<sub>2</sub> (g) and I<sub>2</sub>(g). As well as the partial pressures of the products, 2 HI(g). Besides the relative amounts which these species exist at equilibrium the rate at which either forms or breaks down is also crucial from our study of kinetics. In which at equilibrium, the K<sub>f</sub> equals the K<sub>r</sub>, therefore a shift in these two variables can have an impact on the establishment of the equilibrium.</P> <P> Several cases arise from this premise, of the many, one which we will be concerned with is keeping the initial concentrations of reactants and products equivalent,
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Dynamic equilibrium - &lt;P&gt; In the reaction of...

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