Equilibrium Constants and Reactions

Front

What is the equilibrium constant (K_eq)?

Back

The equilibrium constant (K_eq) is a numerical value that expresses the ratio of the concentrations of products to the concentrations of reactants at equilibrium for a reversible chemical reaction.

Front

How do you calculate K_eq for a reaction?

Back

K_eq = [products]^coefficients / [reactants]^coefficients, where the concentrations are at equilibrium.

Front

What does a large K_eq value indicate about a reaction?

Back

A large K_eq value (>>1) indicates that at equilibrium, the reaction favors the formation of products.

Front

What does a small K_eq value indicate about a reaction?

Back

A small K_eq value (<<1) indicates that at equilibrium, the reaction favors the formation of reactants.

Front

What is the difference between K_c and K_p?

Back

K_c is the equilibrium constant expressed in terms of molarity (concentration), while K_p is expressed in terms of partial pressures.

Front

How do you convert K_c to K_p?

Back

K_p = K_c(RT)^(Δn), where Δn is the change in moles of gas (moles of products - moles of reactants), R is the gas constant, and T is the temperature in Kelvin.

Front

What is the significance of the reaction quotient (Q)?

Back

The reaction quotient (Q) is a measure of the relative amounts of products and reactants at any point in time, used to predict the direction of the reaction.

Front

What does it mean if Q < K_eq?

Back

If Q < K_eq, the reaction will proceed in the forward direction to form more products.

Front

What does it mean if Q > K_eq?

Back

If Q > K_eq, the reaction will proceed in the reverse direction to form more reactants.

Front

What is the equilibrium expression for the reaction: 2A ⇌ B + C?

Back

K_eq = [B][C] / [A]^2.