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Questions and Answers
In chemical equilibrium, what does it mean when the equilibrium position is 'far to the right'?
In chemical equilibrium, what does it mean when the equilibrium position is 'far to the right'?
- Hardly any product is formed from the reactants at equilibrium
- Nearly all the reactants are consumed at equilibrium (correct)
- The forward reaction proceeds at a much faster rate than the reverse reaction
- The reverse reaction proceeds at a much faster rate than the forward reaction
What is the condition for a reaction mixture to exist at equilibrium?
What is the condition for a reaction mixture to exist at equilibrium?
- The forward reaction rate must be greater than the backward reaction rate
- The rates of the forward and backward reactions must be zero
- The rates of the forward and backward reactions must be equal (correct)
- The backward reaction rate must be greater than the forward reaction rate
What is the state of a system at chemical equilibrium?
What is the state of a system at chemical equilibrium?
- The reactants and products are absent
- The reverse reaction completely consumes the products
- No observable change in the properties of the system (correct)
- The forward reaction completely consumes the reactants
What did Berthollet discover that led to the development of the concept of chemical equilibrium?
What did Berthollet discover that led to the development of the concept of chemical equilibrium?
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What does it mean when the equilibrium position is 'far to the left'?
What does it mean when the equilibrium position is 'far to the left'?
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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.
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