What is the Difference Between Equilibrium Constant and Reaction Quotient?
🆚 Go to Comparative Table 🆚The main differences between the equilibrium constant (K) and the reaction quotient (Q) are:
- Time: K represents the concentrations at equilibrium, while Q can use the concentrations at any given time during the reaction.
- Value: The value of Q changes during a reaction, whereas the value of K does not change unless the temperature changes.
- Equilibrium: Q can be calculated at any point during the reaction, whether it is at equilibrium or not. In contrast, K is calculated only when the reaction reaches equilibrium.
- Comparison: By comparing Q and K, we can determine in which direction the reaction will proceed initially.
In summary, the equilibrium constant (K) is a measure of the reaction's state at equilibrium, while the reaction quotient (Q) describes the state of the system with respect to equilibrium at any given time during the reaction. Comparing Q and K allows us to understand the direction in which the reaction will proceed.
Comparative Table: Equilibrium Constant vs Reaction Quotient
The equilibrium constant (K) and the reaction quotient (Q) are both used to describe the state of a chemical reaction with respect to equilibrium. However, they differ in several aspects:
Equilibrium Constant (K) | Reaction Quotient (Q) |
---|---|
Represents the ratio of products to reactants at equilibrium | Represents the ratio of products to reactants at any point during the reaction |
Unitless | Units may vary depending on the reaction |
Value does not change unless the temperature changes | Value changes during the reaction |
Helps determine the direction in which a reaction will shift to achieve equilibrium | Can be compared to K to determine if a reaction is at equilibrium or if it will shift to the right or left to reach equilibrium |
In summary, the equilibrium constant (K) is a constant value that represents the ratio of products to reactants at equilibrium, while the reaction quotient (Q) is a variable value that represents the ratio of products to reactants at any point during the reaction. Comparing Q and K can help determine the direction in which a reaction will proceed to reach equilibrium.
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