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Equilibrium in Chemical Processes

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Questions and Answers

What is a characteristic of systems at chemical equilibrium?

Opposing processes occur at different rates.

Reactant concentrations are always higher than product concentrations.

One of the system's parameters has a constant value. (correct)

Measurable properties fluctuate continuously.

Why is chemical equilibrium described as dynamic?

The reaction stops after reaching equilibrium.

Forward and reverse reactions occur at different rates.

The reaction produces more products than reactants.

Reactants and products are continuously converting into each other. (correct)

In the Haber-Bosch process, what does the use of D₂ instead of H₂ demonstrate?

Different starting materials do not affect equilibrium composition. (correct)

Higher temperatures always shift equilibrium towards products.

Equilibrium is dependent on initial reactant concentration.

Equilibrium cannot be achieved with isotopes.

What does a leveling-off curve in a concentration versus time graph indicate?

<p>The system has reached a state of equilibrium.</p> Signup and view all the answers

Which condition is necessary for a system to reach chemical equilibrium?

<p>The temperature must remain constant in a closed system.</p> Signup and view all the answers

Study Notes

Equilibrium in Chemical Processes

Chemical reactions can reach equilibrium, a state where the rates of forward and reverse reactions are equal.
Equilibrium can be achieved starting with reactants or products.
Equilibrium is dynamic; both forward and reverse reactions continue, but at equal rates, maintaining constant concentrations of reactants and products.
Equilibrium is characterized by constant measurable properties at a given temperature.
The magnitude of these properties indicates the extent of the process's progression toward equilibrium.

Dynamic Equilibrium

Equilibrium is dynamic, meaning both forward and reverse reactions occur, but at equal rates.
The system is closed, preventing external influences.
Reactant and product concentrations remain constant.
The system exhibits constant, measurable properties.

Examples of Equilibrium

Haber-Bosch process: synthesis of ammonia.
The reaction in a closed system reaches equilibrium regardless of initial amounts of reactants or products.
The rate at which the products are produced is equal to the rate at which the reactants are used to make them.

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Description

This quiz explores the concept of equilibrium in chemical reactions, highlighting its dynamic nature and the conditions required for it to occur. Learn about the characteristics of equilibrium, the significance of constant measurable properties, and explore examples such as the Haber-Bosch process. Test your understanding of how reactions can reach equilibrium and the factors that influence it.