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Chapter 17: Problem 59

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

Short Answer

Expert verified
At equilibrium, the rates of the forward and reverse reactions are equal.

Step by step solution

01

Understanding Reversible Reactions

A reversible reaction is one where the products can react to reform the reactants. This means the reaction can proceed in both directions, forward and backward.
02

Defining Equilibrium

Equilibrium in the context of a chemical reaction implies that the rate of the forward reaction is equal to the rate of the backward reaction. This dynamic state maintains a constant concentration of reactants and products.
03

Rates at Equilibrium

When a reversible reaction reaches equilibrium, the characteristic feature is that the forward and reverse reaction rates are equal. Although reactions continue to occur in both directions, there is no net change in the concentrations of reactants and products.

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Key Concepts

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

Reversible Reactions
In the world of chemistry, some reactions can go in both directions鈥攖hese are called reversible reactions. Simply put, in a reversible reaction, the products can transform back into the original reactants.
Reversible reactions are fundamental as they help explain many natural processes, where substances regularly convert back and forth. While a reaction is reversible, it does not mean both directions occur equally or spontaneously. The direction and extent depend on various factors like temperature, pressure, and concentration of substances involved.
However, understanding the reversible nature of reactions is key to predicting how reactions behave under different conditions.
Reaction Rate
The concept of reaction rate plays a crucial role in understanding chemical processes. The rate of a reaction tells us how quickly or slowly a reaction proceeds.
In reversible reactions, there are two ongoing reaction rates: the forward rate, where reactants form products, and the reverse rate, where products revert to reactants.
  • Forward Reaction Rate: As reactants convert into products, this rate initially might be fast but changes as the reaction proceeds.
  • Reverse Reaction Rate: As products start accumulating, they can react to form the original reactants at this rate.
These rates are not static and will adjust until equilibrium is reached. Monitoring reaction rates allows chemists to manage how quickly a system approaches equilibrium and how external changes affect the reaction process.
Dynamic Equilibrium
Reaching equilibrium doesn't mean a halt in chemical reactions. Instead, it introduces the idea of dynamic equilibrium, where reactions continue indefinitely but with balanced reaction rates.
At dynamic equilibrium, the forward and reverse reaction rates are equal, retaining consistent concentrations of both reactants and products.
This dynamic state is like a tug-of-war where neither side wins but both keep pulling. It鈥檚 important because it shows that equilibrium is not static but a continuous state of active processes balancing each other out.
  • Maintaining Equilibrium: Various factors, such as changes in temperature or pressure, can disturb the balance, but reactions will attempt to return to equilibrium.
  • Practical Implications: This principle is employed in industrial processes like the Haber process for ammonia production, balancing reaction conditions to maximize yield.
Understanding dynamic equilibrium allows us to appreciate the intricate balance present in chemical systems.

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Most popular questions from this chapter

The zinc ion concentration in a saturated solution of zinc phosphate, \(\mathrm{Zn}_{3}\left(\mathrm{PO}_{4}\right)_{2},\) is \(1.5 \times 10^{-7} \mathrm{M}\). Calculate the value for the equilibrium constant

Hydrofluoric acid, HF, is used in the manufacture of silicon computer chips. If the \(\mathrm{pH}\) of a \(0.139 \mathrm{M}\) solution is 2.00 , what is the ionization constant of the acid?

Write the solubility product expression for each of the following slightly soluble ionic compounds in a saturated aqueous solution: (a) \(\operatorname{AgI}(s) \rightleftarrows \operatorname{Ag}^{+}(a q)+\mathrm{I}^{-}(a q)\) (b) \(\mathrm{Ag}_{2} \mathrm{CrO}_{4}(s) \rightleftarrows 2 \mathrm{Ag}^{+}(a q)+\mathrm{CrO}_{4}^{2-}(a q)\) (c) \(\mathrm{Ag}_{3} \mathrm{PO}_{4}(\mathrm{~s}) \rightleftarrows 3 \mathrm{Ag}^{+}(a q)+\mathrm{PO}_{4}^{3-}(a q)\)

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.

Given the chemical equation for the ionization of acetic acid $$\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q) \rightleftarrows \mathrm{H}^{+}(a q)+\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}^{-}(a q)$$ Predict the direction of equilibrium shift for each of the following stresses: (a) increase \(\left[\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right]\) (b) increase \(\left[\mathrm{H}^{+}\right]\) (c) decrease \(\left[\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right]\) (d) decrease \(\left[\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}^{-}\right]\) (e) add solid \(\mathrm{NaC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) (f) add solid \(\mathrm{NaCl}\) (g) add solid NaOH (h) increase \(\mathrm{pH}\)
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