Write the reaction quotients \(Q_{c}\) for (a) \(\mathrm{Cu}(\mathrm{s})+\mathrm{Cl}_{2}(\mathrm{~g}) \rightarrow \mathrm{CuCl}_{2}(\mathrm{~s})\) (b) \(\mathrm{NH}_{4} \mathrm{NO}_{2}\) (s) \(\rightarrow \mathrm{N}_{2} \mathrm{O}\) (g) \(+2 \mathrm{H}_{2} \mathrm{O}\) (g) (c) \(\mathrm{MgCO}_{3}(\mathrm{~s}) \rightarrow \mathrm{MgO}\) (s) \(+\mathrm{CO}_{2}\) (g)

Chemical equilibrium is a state of a chemical reaction at which the concentrations of reactants and products remain constant over time, indicating a balance between the forward and reverse reactions. This does not mean the reactions have ceased, but rather that their rates are equal, effectively making the observable properties of the system constant. At equilibrium, the reaction quotient \(Q_c\) is equal to the equilibrium constant \(K_c\), an important figure that can be used to predict the direction of the reaction. It is crucial to assess how the system might respond to changes in concentration, pressure, or temperature, applying Le Chatelier’s principle.

For instance, if an equilibrium system is exposed to a change, say an increase in concentration of a product, the system will adjust to counteract that change, often by increasing the rate of the reverse reaction. This adjustment works to re-establish equilibrium conditions, hence maintaining the balance of reactant and product concentrations.

Stoichiometric coefficients in a balanced chemical reaction indicate the relative quantities of each substance involved. They play a pivotal role in determining the proportions of reactants consumed and products formed during a reaction. In the context of the reaction quotient, \(Q_c\), stoichiometric coefficients determine the exponents to which the concentrations of substances are raised in the quotient's calculation.

For example, in the provided solution for reaction (b), the balanced equation \(\mathrm{NH}_{4}\mathrm{NO}_{2}\) (s) \(\rightarrow\) \(\mathrm{N}_{2}\mathrm{O}\) (g) \(+2 \mathrm{H}_{2}\mathrm{O}\) (g) shows a stoichiometric coefficient of 1 for \(\mathrm{N}_{2}\mathrm{O}\) and 2 for \(\mathrm{H}_{2}\mathrm{O}\), giving us a \(Q_c\) that considers the concentration of \(\mathrm{N}_{2}\mathrm{O}\) to the first power and \(\mathrm{H}_{2}\mathrm{O}\) to the second power. Understanding these coefficients is essential for properly writing out the reaction quotient expression and predicting the extent of a reaction.

The concentration of reactants and products is a measure of the amount of a substance in a given volume of solution. It's typically expressed in molarity (moles per liter). In chemical kinetics and equilibrium, the concentrations of the reactants and products at any point in time can predict the direction and extent of the reaction. In the reaction quotient \(Q_c\), the concentrations of gaseous and aqueous species are used to gauge how far a system is from reaching equilibrium.

It’s essential to recognize that in the \(Q_c\) expression, the concentration of pure solids and liquids, as shown in the reactions (a) and (c), are omitted because their concentrations remain constant. Gaseous substance concentrations, as in reaction (c) with \(\mathrm{CO}_{2}\) gas, are included in the \(Q_c\) expression. Calculating accurate concentrations of the reactive species involved is fundamental to predicting the behavior of a chemical system under various conditions and is one of the foundational concepts in the study of chemical equilibria.