Calculate the equilibrium constant for each of the reactions in Problem 65.

Verified step by step guidance

1. Identify the balanced chemical equation for each reaction given in Problem 65. Ensure that the stoichiometric coefficients are correct as they will be used in the calculation of the equilibrium constant.
2. Write the expression for the equilibrium constant, $K$, for each reaction. The general form of the expression is $K = \frac{[\text{products}]^{\text{coefficients}}}{[\text{reactants}]^{\text{coefficients}}}$, where the concentrations of products and reactants are raised to the power of their respective stoichiometric coefficients in the balanced equation.
3. Gather the concentration data or partial pressures for each reactant and product at equilibrium. This information might be given directly in the problem or might need to be calculated based on other provided data.
4. Substitute the equilibrium concentrations or partial pressures into the equilibrium constant expression for each reaction. Ensure that the units are consistent and appropriate for the type of reaction (concentration in mol/L for solutions and pressure in atm for gases).
5. Calculate the numerical value of the equilibrium constant for each reaction. Remember that the equilibrium constant is dimensionless and provides a measure of the extent to which a reaction proceeds to completion under given conditions.

Key Concepts

Equilibrium Constant (K)

The equilibrium constant (K) is a numerical value that expresses the ratio of the concentrations of products to reactants at equilibrium for a given chemical reaction. It is temperature-dependent and provides insight into the extent of a reaction; a large K indicates a reaction that favors products, while a small K suggests a preference for reactants.

Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system will adjust itself to counteract the change and restore a new equilibrium. This principle helps predict how changes in concentration, pressure, or temperature will affect the position of equilibrium and, consequently, the value of K.

Reaction Quotient (Q)

The reaction quotient (Q) is a measure of the relative concentrations of products and reactants at any point in time during a reaction. It is calculated using the same formula as the equilibrium constant but with concentrations that are not necessarily at equilibrium. Comparing Q to K allows us to determine the direction in which a reaction will proceed to reach equilibrium.