Chapter 07 Equilibrium Vocabulary

Vocabulary flashcards covering key terms, definitions, equations, and principles from Chapter 07 Equilibrium.

Irreversible Reactions

Reactions that proceed only in one direction (forward), represented by a single arrow ($\rightarrow$).

Reversible Reactions

Reactions that can proceed in both forward and backward directions simultaneously, represented by a double or equilibrium arrow ($\rightleftharpoons$ or $\Leftrightarrow$).

Equilibrium State

A state in which the rates of the forward and backward reactions are equal and dynamic in nature, meaning the reaction processes continue occurring at the exact same rate to keep net concentrations constant.

Physical Equilibrium

An equilibrium involving physical processes such as a change of state or phase, such as the melting of ice ($H_2O(s) \rightleftharpoons H_2O(l)$ at $0\,^\circ\text{C}$) or evaporation of water ($H_2O(l) \rightleftharpoons H_2O(g)$ at $100\,^\circ\text{C}$).

Chemical Equilibrium

An equilibrium associated with chemical reactions where the concentrations of both reactants and products remain constant over time (e.g., $N_2 + 3H_2 \rightleftharpoons 2NH_3$).

Law of Chemical Equilibrium

The law stating that at a constant temperature, the ratio of the product of concentrations of the products to that of the reactants, with each concentration term raised to a power equal to its stoichiometric coefficient in the balanced chemical equation, has a constant value.

Equilibrium Constant ($K_c$)

The ratio defined by $K_c = \frac{[C]^c[D]^d}{[A]^a[B]^b}$ for a general reversible reaction $aA + bB \rightleftharpoons cC + dD$.

Reverse Reaction Equilibrium Constant ($K'$)

The equilibrium constant for a reverse reaction, which is the reciprocal of the forward reaction constant ($K' = \frac{1}{K}$).

Gaseous Equilibrium Constant ($K_p$)

The equilibrium constant for reactions involving gases, where concentration terms are replaced by their respective partial pressures ($P$).

$K_p$ and $K_c$ Relationship Equation

The expression $K_p = K_c(RT)^{\Delta n}$, derived from the Ideal Gas Equation $P = \text{[Concentration]} \cdot RT$.

$$\Delta n$$

The difference calculated as $\Delta n = (c + d) - (a + b) = n_P - n_R$, representing the number of moles of gaseous products minus the number of moles of gaseous reactants.