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Chapter 12: Problem 82

What types of reactions are classified as homogeneous equilibria?

Short Answer

Expert verified
The types of reactions classified as homogeneous equilibria are those in which all reactants and products are in the same physical state. These can include gas-phase reactions, reactions in solution, and solid-state reactions.

Step by step solution

01

Understanding Homogeneous Equilibria

Homogeneous equilibrium is when all the reactants and products are in the same physical state. These states can be solid, liquid, gas, or a solution.
02

Classifying Reaction Types

Under homogeneous equilibria, we can classify various types of reactions. These include: \[1) Gas-phase reactions - where all reactants and products are gases. For example: N_2(g) + 3H_2(g) 鈬� 2NH_3(g)\] \[2) Reactions in solution - where all reactants and products are in the same solution. For example: AgNO_3(aq) + NaCl(aq) 鈬� AgCl(s) + NaNO_3(aq)\] \[3) Solid-state reactions - where all reactants and products are in solid state. Though less common, these reactions do exist. An example: Fe_3O_4(s) 鈬� 3FeO(s) + 1/2O_2(g)\]

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Key Concepts

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

Gas-phase reactions
Gas-phase reactions occur when all the reactants and products are gases. These reactions are an excellent example of homogeneous equilibria. One common occurrence of gas-phase reactions is in the synthesis of ammonia. Consider the reaction:

\[\text{N}_2(g) + 3\text{H}_2(g) \rightleftharpoons 2\text{NH}_3(g)\]

In this reaction, nitrogen and hydrogen gases react together to form ammonia gas. All participants are in the gaseous state.
  • This uniform state helps ensure that the particles can freely mix and react efficiently.
  • Equilibrium in this context refers to the balance between the forward and reverse reactions, maintaining constant concentrations over time.
Gas-phase reactions are important in both industrial and natural processes. Their study is crucial for applications like the Haber process for ammonia production.
Reactions in solution
Reactions that occur in solution are another form of homogeneous equilibria. In these processes, reactants and products are dissolved in a solvent, usually a liquid such as water. A classic example involves silver nitrate and sodium chloride solutions:

\[\text{AgNO}_3(aq) + \text{NaCl}(aq) \rightleftharpoons \text{AgCl}(s) + \text{NaNO}_3(aq)\]

Here, while silver chloride precipitates out, the dissolved ions initially react in an aqueous environment.
  • Since all reactive species are in the same solution, molecular interactions are facilitated.
  • These reactions are crucial in analytical chemistry and biological systems where solutions provide a medium for metabolic processes.
The concept of equilibrium is crucial in predicting the direction and extent of the reaction.
Solid-state reactions
Solid-state reactions involve reactants and products all in the solid phase. These are less common compared to their gas and solution counterparts but are essential in fields like materials science. An example is:

\[\text{Fe}_3\text{O}_4(s) \rightleftharpoons 3\text{FeO}(s) + \frac{1}{2}\text{O}_2(g)\]

In this reaction, magnetite can decompose into ferrous oxide and oxygen under certain conditions.
  • These reactions occur at interfaces or grain boundaries, where the solid structures can interact.
  • Solid-state reactions are fundamental in processes such as the formation of ceramics and metal alloys.
Understanding these reactions requires knowledge of crystal structures and lattice dynamics, differentiating them from more common reaction types.

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Most popular questions from this chapter

What is the chemical species that exists temporarily during a multistep reaction?

If the initial concentrations of reactants and products are substituted into the equilibrium constant expression, and the value obtained is greater than the equilibrium constant, is the system in a state of equilibrium? If not, in which direction will the reaction shift to reach equilibrium? Explain.

Consider the following factors: increase in temperature, increase in concentration, and addition of a catalyst. Which increases the average kinetic energy of the reactants?

Draw a generic energy diagram that shows the energies of reactants, products, and the activated complex. Label the activation energy.

Consider the vaporization of bromine in a closed container: $$ \mathrm{Br}_{2}(l) \rightleftharpoons \mathrm{Br}_{2}(g) $$ What kinds of measurements could you make to determine if this physical change has reached a state of equilibrium?
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