O iodeto de amônio dissocia-se reversivelmente em amônia e...

O iodeto de amônio dissocia-se reversivelmente em amônia e io. deto de hidrogēnio se for aquecido a temperatura suficientemente elevada. $$ \mathrm{NH}_4 \mathrm{I}(\mathrm{s}) \rightleftarrows \mathrm{NH}_3(\mathrm{~g})+\mathrm{HI}(\mathrm{g}) $$ Uma amostra de iodeto de amônio é colocada num balão e aquecida a $400^{\circ} \mathrm{C}$. Se a pressão total no balāo, atingido o equilibrio, for $705 \mathrm{~mm} \mathrm{Hg}$, qual o valor de $K_p$ (com as pressōes parciais em af. mosferas)?

O iodeto de amônio dissocia-se reversivelmente em amônia e io. deto de hidrogēnio se for aquecido a temperatura suficientemente elevada.
$$
\mathrm{NH}_4 \mathrm{I}(\mathrm{s}) \rightleftarrows \mathrm{NH}_3(\mathrm{~g})+\mathrm{HI}(\mathrm{g})
$$

Uma amostra de iodeto de amônio é colocada num balão e aquecida a $400^{\circ} \mathrm{C}$. Se a pressão total no balāo, atingido o equilibrio, for $705 \mathrm{~mm} \mathrm{Hg}$, qual o valor de $K_p$ (com as pressōes parciais em af. mosferas)?

Key Concepts

Chemical Equilibrium

Chemical equilibrium refers to the state in a reversible chemical reaction where the rate of the forward reaction equals the rate of the reverse reaction, and the concentrations (or partial pressures in the case of gases) of reactants and products remain constant over time. It involves dynamic processes, as reactants and products continue to form and convert, but overall, their amounts remain stable.

Equilibrium Constant (Kp)

The equilibrium constant, denoted as Kp when involving gaseous species, is defined as the ratio of the product of the partial pressures of the products to that of the reactants, each raised to the power of their stoichiometric coefficients. It provides a quantitative measure of the position of equilibrium and is dependent on temperature.

Partial Pressure

Partial pressure is the pressure exerted by an individual gas in a mixture of gases. It is especially important in equilibrium calculations involving gases, as these pressures are used in the expression for Kp. The individual partial pressures contribute to the total pressure observed in the system.

Reaction Stoichiometry

Reaction stoichiometry involves the quantitative relationships between reactants and products as defined by the balanced chemical equation. In equilibrium problems, stoichiometry is used to relate the changes in the amounts or pressures of gases produced or consumed during the reaction.

Unit Conversion in Gas Equilibrium

In gas equilibrium calculations, it is often necessary to convert pressure units (for example, from mm Hg to atmospheres) since the equilibrium constant Kp is typically expressed in terms of atmospheres. This conversion ensures that all terms in the equilibrium expression are consistent and correctly calculated.

Heterogeneous Equilibrium

Heterogeneous equilibrium refers to reactions where the reactants and products exist in different phases, such as a solid decomposing into gases. In such situations, the concentration (or activity) of the pure solid is taken as constant and does not appear in the equilibrium constant expression.

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