5 Questions
In chemical equilibrium, what does it mean when the equilibrium position is 'far to the right'?
Nearly all the reactants are consumed at equilibrium
What is the condition for a reaction mixture to exist at equilibrium?
The rates of the forward and backward reactions must be equal
What is the state of a system at chemical equilibrium?
No observable change in the properties of the system
What did Berthollet discover that led to the development of the concept of chemical equilibrium?
Some chemical reactions are reversible
What does it mean when the equilibrium position is 'far to the left'?
Hardly any product is formed from the reactants at equilibrium
Study Notes
Chemical Equilibrium
- When the equilibrium position is 'far to the right', it means the reaction has proceeded almost to completion, with nearly all reactants converted to products.
- A reaction mixture exists at equilibrium when the rates of forward and reverse reactions are equal, with no net change in composition.
- At chemical equilibrium, the state of a system is dynamic, with forward and reverse reactions occurring simultaneously, but at equal rates.
Development of Chemical Equilibrium Concept
- Berthollet discovered that some chemical reactions are reversible, leading to the development of the concept of chemical equilibrium.
Equilibrium Position
- When the equilibrium position is 'far to the left', it means the reaction has hardly proceeded, with most reactants remaining unreacted.
Test your knowledge of chemical equilibrium with this quiz. Explore the concepts of reactants, products, and the balance between forward and reverse reactions.
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