#Chemical Equilibrium: Calculating Equilibrium Constants

#Introduction

Now that you're familiar with the concepts of $K_c$ and $K_p$, let's dive into how to calculate them! This guide will help you master these calculations, ensuring you're ready for anything the AP Chemistry exam throws your way. Remember, equilibrium is all about the balance between reactants and products. Let's get started!

Equilibrium calculations are a cornerstone of AP Chemistry. Expect to see them in both multiple-choice and free-response questions. Mastering this topic is crucial for a strong exam performance.

#Equilibrium Constant Formulas

#Key Concepts

• Equilibrium: A state where the rate of forward and reverse reactions are equal, and the concentrations of reactants and products remain constant.

• $K_c$ (Equilibrium Constant in terms of concentration): Relates the concentrations of reactants and products at equilibrium.

• $K_p$ (Equilibrium Constant in terms of pressure): Relates the partial pressures of gaseous reactants and products at equilibrium.

#Formulas

Both $K_c$ and $K_p$ follow the same basic formula: products over reactants, each raised to the power of their stoichiometric coefficients. The difference lies in whether you're using concentrations (for $K_c$) or partial pressures (for $K_p$).

#$K_c$ Formula

latex
<math-block>K\_c = \frac{[C]^c[D]^d}{[A]^a[B]^b}</math-block>

Where:

• [A], [B] are the equilibrium concentrations of reactants.
• [C], [D] are the equilibrium concentrations of products.
• a, b, c, d are the stoichiometric coefficients from the balanced chemical equation.

#$K_p$ Formula

latex
<math-block>K\_p = \frac{P\_C^cP\_D^d}{P\_A^aP\_B^b}</math-block>

Where:

• $P_A$, $P_B$ are the partial pressures of reactants at equilibrium.

• $P_C$, $P_D$ are the partial pressures of products at equilibrium.

• a, b, c, d are the stoichiometric coefficients from the balanced chemical equation.

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