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Chapter 17: Problem 60

With regard to concentration, what is characteristic of a reversible reaction at equilibrium?

Short Answer

Expert verified
At equilibrium, a reversible reaction has constant concentrations of reactants and products due to equal rates of forward and reverse reactions.

Step by step solution

01

Understanding the Concept of Equilibrium

A reversible reaction is one where the products can revert back to the original reactants. At equilibrium, the rate of the forward reaction equals the rate of the reverse reaction.
02

Defining Dynamic Equilibrium

In a chemical equilibrium state, reactants and products are formed at such rates that their concentrations remain constant over time, despite the ongoing reactions. This is known as dynamic equilibrium.
03

Analyzing Concentrations at Equilibrium

At equilibrium, the concentrations of reactants and products do not change because the rates of both the forward and reverse reactions are equal, leading to no net change in concentration.
04

Relationship Between Rates and Concentrations

For the overall reaction rate to stabilize, similar numbers of molecules are being converted in both directions, which keeps the concentrations of all substances constant, not necessarily equal.

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Key Concepts

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

Reversible Reaction
In chemistry, a reversible reaction is one where the products can change back into the reactants. Unlike reactions that go entirely in one direction, reversible reactions can proceed in both forward and reverse directions under the right conditions. Such reactions are characterized by the ability to reach a state of balance or equilibrium.

Key traits of reversible reactions include:
  • Possibility for both forward and backward reactions.
  • Products can react to form the original reactants.
  • Dynamic nature 鈥� they do not stop but continue in both directions at equilibrium.
This nature gives reversible reactions the flexibility to adjust according to changes in conditions, which is central to the concept of dynamic equilibrium.
Dynamic Equilibrium
Dynamic equilibrium is a fascinating concept within the context of reversible reactions. At this point, even though reactions continue to occur, the overall concentrations of reactants and products remain unchanged. This is because the rates of the forward and backward reactions are equal.

Key points about dynamic equilibrium:
  • The system is not static 鈥� reactions still happen continuously.
  • The concentrations of substances do not change over time.
  • Any change in conditions, like temperature or pressure, can shift the equilibrium point.
It鈥檚 important to understand that at dynamic equilibrium, chemical reactions are balanced in a way that maintains a constant concentration of all components involved.
Reaction Rates
When discussing chemical equilibrium, reaction rates provide a crucial understanding of how reactions proceed to reach equilibrium. Reaction rates refer to the speed at which reactants turn into products and vice versa. In a reversible reaction at equilibrium, these rates are equal in both directions.

Some important aspects of reaction rates include:
  • Forward and reverse reaction rates are equivalent at equilibrium.
  • Influenced by factors such as concentration, temperature, and catalysts.
  • Play a critical role in establishing and maintaining equilibrium.
By examining reaction rates, scientists can predict how a system behaves under various conditions and what measures can be taken to reach or modify equilibrium.

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Most popular questions from this chapter

The conditions for producing ammonia industrially are \(500^{\circ} \mathrm{C}\) and \(300 \mathrm{~atm}\). What happens to the ammonia concentration if (a) the temperature increases and (b) the pressure increases? $$\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \rightleftarrows 2 \mathrm{NH}_{3}(g)+\text { heat }$$

Explain why zinc carbonate, \(\mathrm{ZnCO}_{3}\), is more soluble in hydrochloric acid than in water

Write the solubility product expression for each of the following slightly soluble ionic compounds in a saturated aqueous solution: (a) \(\mathrm{Cu}_{2} \mathrm{CO}_{3}(s) \rightleftarrows 2 \mathrm{Cu}^{+}(a q)+\mathrm{CO}_{3}^{2-}(a q)\) (b) \(\mathrm{ZnCO}_{3}(s) \rightleftarrows \mathrm{Zn}^{2+}(a q)+\mathrm{CO}_{3}^{2-}(a q)\) (c) \(\mathrm{Al}_{2}\left(\mathrm{CO}_{3}\right)_{3}(s) \rightleftarrows 2 \mathrm{Al}^{3+}(a q)+3 \mathrm{CO}_{3}^{2-}(a q)\)

The Contact Process uses a metal catalyst to produce sulfur trioxide gas for the manufacture of sulfuric acid. Does the catalyst increase the amount of sulfur trioxide gas? Explain.

The \(K_{\text {sp }}\) values for \(\mathrm{CaCO}_{3}\) and \(\mathrm{CaC}_{2} \mathrm{O}_{4}\) are \(3.8 \times 10^{-9}\) and \(2.3 \times 10^{-9}\), respectively. In saturated solutions of \(\mathrm{CaCO}_{3}\) and \(\mathrm{CaC}_{2} \mathrm{O}_{4}\), which has the higher calcium ion concentration?
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