Write the reaction quotients \(Q_{c}\) for (a) \(\mathrm{Fe}(\mathrm{OH})_{3}(\mathrm{~s}) \rightarrow \mathrm{Fe}^{3}(\mathrm{aq})+3 \mathrm{OH}^{-}(\mathrm{aq})\) (b) \(\mathrm{CuSO}_{4}(\mathrm{~s})+5 \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \rightarrow \mathrm{CuSO}_{4} \cdot 5 \mathrm{H}_{2} \mathrm{O}\) (s) (c) \(\mathrm{ZnO}(\mathrm{s})+\mathrm{CO}(\mathrm{g}) \rightarrow \mathrm{Zn}(\mathrm{s})+\mathrm{CO}_{2}(\mathrm{~g})\)

Chemical equilibrium is a state in a chemical reaction where the rate of the forward reaction equals the rate of the reverse reaction. In simpler terms, at equilibrium, the amounts of reactants and products remain constant over time, even though the reactions continue to occur. This balance does not mean that the reactants and products are present in equal amounts but rather that their concentrations have stabilized and are not changing with time.

Understanding chemical equilibrium is fundamental when studying reactions, as it can influence the outcome of a chemical process. In an equilibrium state, the reaction quotient (\(Q\textsubscript{c}\) or \(Q\textsubscript{p}\) for pressure) will equal the equilibrium constant (\(K\textsubscript{c}\) or \(K\textsubscript{p}\)) of the reaction. This equilibrium constant is a reflection of the ratio of the concentrations of products to reactants at equilibrium. Every different reaction at given conditions has a unique equilibrium constant that can indicate the position of the equilibrium and the extent to which reactants are converted to products.

Stoichiometry is a section of chemistry that involves the calculation of relative quantities of reactants and products in chemical reactions. It's grounded in the law of conservation of mass, where the total mass of reactants equals the total mass of products. In a balanced chemical equation, the stoichiometric coefficients represent the number of molecules (or moles) involved in the reaction for each substance.

To accurately calculate the reaction quotient (\(Q\textsubscript{c}\)) or the equilibrium constant (\(K\textsubscript{c}\)), one needs to apply the principles of stoichiometry. Each concentration (in mol/L) of a substance in the reaction quotient expression is raised to the power of its stoichiometric coefficient. It is crucial in computing the correct values for both equations and predictions regarding the direction of the reaction. Knowing the proper stoichiometry is essential for students in predicting product formation and for industries to optimize the production and yield of chemical processes.

The equilibrium constant, represented as (\(K\textsubscript{c}\) for concentrations or \(K\textsubscript{p}\) for pressures), is a number that expresses the relationship between the amounts of products and reactants at the point of chemical equilibrium for a reversible reaction at a constant temperature. The equilibrium constant provides insight into the position of equilibrium and the extent of the reaction: a large value of (\(K\textsubscript{c}\)) or (\(K\textsubscript{p}\)) indicates that, at equilibrium, a greater concentration of products is present compared to reactants, suggesting the reaction favors the production of products. Conversely, a small value points to a higher concentration of reactants.

Understanding how to calculate and apply the equilibrium constant is invaluable when predicting the outcome of a reaction. When you calculate the reaction quotient (\(Q\textsubscript{c}\)) during a reaction that hasn't yet reached equilibrium, you can predict which way the reaction will proceed to reach equilibrium; if \(Q\textsubscript{c} < K\textsubscript{c}\), the reaction will proceed forward to produce more products, and if \(Q\textsubscript{c} > K\textsubscript{c}\), the reaction will proceed in the reverse direction to produce more reactants.