Reversible reactions

Definition

Reversible reactions are chemical reactions where the reactants can form products, which can then revert back into the original reactants. These reactions reach a state of dynamic equilibrium where the rate of the forward reaction equals the rate of the reverse reaction.

5 Must Know Facts For Your Next Test

1. Reversible reactions do not go to completion; instead, they reach an equilibrium state.
2. At equilibrium, the concentrations of reactants and products remain constant over time.
3. The direction of reversible reactions can be influenced by changes in temperature, pressure, and concentration.
4. Le Chatelier's principle describes how a system at equilibrium responds to external changes.
5. In biological systems, reversible reactions are crucial for metabolic pathways and homeostasis.

Review Questions

• What happens to the concentrations of reactants and products in a reversible reaction at equilibrium?
• How does Le Chatelier's principle apply to reversible reactions?
• Why are reversible reactions important in biological systems?

Related terms

Dynamic Equilibrium: A state in which the forward and reverse rates of a chemical reaction are equal, resulting in no net change in concentrations.

Le Chatelier's Principle: A principle stating that if a system at equilibrium is disturbed, it will adjust to counteract the disturbance and restore equilibrium.

Metabolic Pathways: Series of interconnected biochemical reactions that convert substrates through multiple steps into final products; often involve reversible steps.