Which of the following relative values of kf and kr results in an equilibrium mixture that contains large amounts of reactants and small amounts of products? (a) kf 7 kr (b) kf = kr (c) kf 6 kr

Verified step by step guidance

Identify the meaning of kf and kr: kf represents the forward reaction rate constant, and kr represents the reverse reaction rate constant.

Understand the relationship between kf, kr, and the position of equilibrium: If kf > kr, the reaction favors the formation of products. If kf < kr, the reaction favors the formation of reactants.

Analyze the given options to determine which scenario leads to a reaction favoring the formation of reactants: (a) kf > kr, (b) kf = kr, (c) kf < kr.

Compare the options to the desired condition of having large amounts of reactants and small amounts of products, which indicates that the equilibrium should lie towards the reactants.

Conclude that the correct option where kf < kr (option c) will result in an equilibrium mixture containing large amounts of reactants and small amounts of products.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Video duration:

Was this helpful?

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 reaction at a specific temperature. It is defined as K = [products]^[coefficients] / [reactants]^[coefficients]. A large K value indicates that products are favored at equilibrium, while a small K value suggests that reactants are favored.

Forward and Reverse Rate Constants (kf and kr)

The forward rate constant (kf) and the reverse rate constant (kr) are parameters that describe the speed of the forward and reverse reactions, respectively. The relationship between these constants determines the position of equilibrium. If kf is much smaller than kr, the reaction favors the formation of reactants, leading to a higher concentration of reactants at equilibrium.

Le Chatelier's Principle

Le Chatelier's Principle states that if a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the system will adjust to counteract that change and restore a new equilibrium. This principle helps predict how changes in conditions will affect the concentrations of reactants and products, providing insight into the behavior of the equilibrium mixture.

Recommended video:

Guided course

07:32

Le Chatelier's Principle

Related Practice

Textbook Question

For the reaction A2 + 2B ∆ 2 AB, the rate of the for- ward reaction is 18 M/s and the rate of the reverse reaction is 12 M/s. The reaction is not at equilibrium. Will the reaction pro-ceed in the forward or reverse direction to attain equilibrium?

Textbook Question

Consider a general, single-step reaction of the type A + B ∆ C. Show that the equilibrium constant is equal to the ratio of the rate constants for the forward and reverse reactions, Kc = kf>kr.

Textbook Question

Consider the reaction of chloromethane with OH- in aque- ous solution: CH Cl1aq2 + OH-1aq2 ∆kf CH OH1aq2 + Cl-1aq2 At 25 °C, the rate constant for the forward reaction is 6 * 10-6 M-1 s-1, and the equilibrium constant Kc is 1 * 1016. Calculate the rate constant for the reverse reac- tion at 25 °C.

Textbook Question

In automobile catalytic converters, the air pollutant nitric oxide is converted to nitrogen and oxygen. Listed in the table are forward and reverse rate constants for the reac- tion 2 NO1g2 ∆ N21g2 + O21g2. Temperature (K) kf1M — 1 s-12 kr1M-1 s — 121400 0.29 1.1 * 10-61500 1.3 1.4 * 10-5Is the reaction endothermic or exothermic? Explain in terms of kinetics.