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Chapter 38: Problem 6

Use a grammatically correct English sentence to describe the relationship between the forward rate and reverse rate at equilibrium.

Short Answer

Expert verified
At equilibrium, the forward rate of a reaction equals the reverse rate. This means that the formation of products from reactants occurs at the same rate as the reformation of reactants from products.

Step by step solution

01

Understand chemical equilibrium

To begin, one must comprehend the concept of chemical equilibrium. This is a state in a chemical reaction where the amounts of the reactants and products do not change over time. This happens when the rate of the forward reaction is equal to the rate of the reverse reaction.
02

Analyze forward and reverse rates

In a chemical reaction, the forward rate is the speed at which the reactants produce the products, while the reverse rate is the speed at which the products revert back to being reactants. These rates can be influenced by different factors including concentration, temperature, and presence of a catalyst.
03

Describe the relationship at equilibrium

At equilibrium, the forward rate of reaction and the reverse rate of reaction are equal. This means that the amount of reactants being converted into products is the same as the amount of products being converted back into reactants. Therefore, on a macroscopic level, it appears as if the reaction has stopped as the concentrations of reactants and products remain steady though the reactions are still taking place.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Forward and Reverse Rates
In the realm of chemical reactions, the terms "forward rate" and "reverse rate" are crucial in understanding the dynamic nature of equilibrium. The forward rate refers to the speed at which reactants transform into products. Conversely, the reverse rate is how quickly products transform back into reactants. This constant interplay is what keeps reactions in balance.
  • Forward Rate: The speed of the tenacious journey of reactants turning into products.
  • Reverse Rate: The rate at which products retrace their steps to become reactants again.
  • Equilibrium: Occurs when these two rates are equal, giving the illusion of stillness as changes occur invisibly at the molecular level.
Factors such as concentration and temperature can influence these rates, nudging the equilibrium point in one direction or another. Understanding these rates is key to predicting how a reaction mixture reacts under various conditions.
Reactants and Products
Reactants and products form the basic vocabulary in the chemistry of reactions. Reactants are the starting substances in a chemical reaction; they undergo transformation to form products. The journey from reactants to products and possibly back is what defines a chemical reaction.
  • Reactants: Starting materials that undergo change in a chemical reaction.
  • Products: New substances formed as a result of the reaction.
At equilibrium, the amounts of reactants and products remain constant, not because they cease changing but because their transformation rates are balanced. This underlying balance plays a fundamental role in the stability and predictability of chemical processes.
Concentration
The concentration of reactants and products is a vital factor in determining the pace of a chemical reaction. Concentration refers to the amount of a substance present in a certain volume of solution. As concentration of reactants increases, the forward rate generally increases because more molecules are available to collide and react.
  • High concentration of reactants usually speeds up the forward reaction.
  • Increasing concentration of products can slow down the forward reaction and enhance the reverse reaction.
At equilibrium, the concentration of reactants and products remains constant. Despite this unchanging outward appearance, the molecules continue to react with one another at a fixed rate.
Catalysts
Catalysts are substances that increase the rate of a chemical reaction without being consumed in the process. They offer a unique pathway with a lower activation energy, making it easier for a reaction to take place. Importantly, catalysts affect both the forward and reverse rates equally, meaning they help achieve equilibrium faster but do not change the position of the equilibrium.
  • Speed up reaction rates by providing an alternative pathway with a lower activation energy.
  • Do not alter the equilibrium concentrations of reactants or products, simply help reach equilibrium more quickly.
Catalysts play a crucial role in industrial applications, allowing reactions to proceed under milder conditions and saving energy in processes ranging from manufacturing to biochemical systems.

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Most popular questions from this chapter

(B) In what region (kinetic or equilibrium) is the quantity \(\frac{(D)}{(A)}\) a constant?
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