Reaction Quotient
Definition
The Reaction Quotient (Q) measures the relative amounts of products and reactants present during a reaction at a particular point in time.
Analogy
Think of Q as taking a snapshot of a race between two runners (reactants turning into products). It doesn't tell us who will win eventually (that's K, or equilibrium constant), but it gives us an idea about who's leading at that specific moment.
Related terms
Equilibrium Constant (K): This tells us what the ratio of products to reactants is when a chemical reaction reaches equilibrium.
Le Chatelier’s Principle: As mentioned above, this principle states that if an external stress is applied to a system at equilibrium, the system adjusts in a way that minimizes the stress.
Shifts in Equilibrium: Changes in concentration, temperature, or pressure can cause a shift in equilibrium. Depending on the change, the reaction may shift to favor either the reactants or products.
"Reaction Quotient" appears in:
Study guides (4)
Practice Questions (2)
In a reaction with an equilibrium constant K = 10^-3, if the reaction quotient Q = 10^-4, what can be said about the direction of the reaction?
A reaction has an equilibrium constant K of 2.5 x 10^-3 at a certain temperature. If the reaction quotient Q is calculated to be 8.0 x 10^-4, what can be said about the direction of the reaction?
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