What is the equilibrium constant for each of the reactions mentioned in Problem 66?

Verified step by step guidance

insert step 1> Identify the reactions mentioned in Problem 66.

insert step 2> Write the balanced chemical equation for each reaction.

insert step 3> Use the balanced equations to write the expression for the equilibrium constant (K) for each reaction.

insert step 4> Determine the concentrations or partial pressures of the reactants and products at equilibrium, if provided.

insert step 5> Substitute the equilibrium concentrations or partial pressures into the equilibrium constant expression to solve for K.

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

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 the equilibrium constant.

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 helps determine the direction in which a reaction will proceed to reach equilibrium.

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Reaction Quotient Q

Related Practice

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Use tabulated electrode potentials to calculate ∆G°rxn for each reaction at 25 °C. a. 2 Fe³⁺(aq) + 3 Sn(s) → 2 Fe(s) + 3 Sn²⁺(aq) b. O₂(g) + 2 H₂O(l) + 2 Cu(s) → 4 OH^–(aq) + 2 Cu²⁺(aq) c. Br₂(l) + 2 I^–(aq) → 2 Br^–(aq) + I₂(s)

Textbook Question

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

Textbook Question

Calculate the equilibrium constant for the reaction between Fe²⁺(aq) and Zn(s) (at 25 °C).