How is the reaction quotient used to determine whether a system is at equilibrium?
The reaction is at equilibrium when Q > Keq.
At equilibrium, the reaction quotient is undefined.
The reaction quotient must be satisfied for equilibrium to be achieved.
The reaction is at equilibrium when Q < Keq.
The reaction is at equilibrium when Q = Keq.
I think the answer is when reaction is at equllibrium when they = each other
You are right.
You are correct! The reaction is at equilibrium when the reaction quotient (Q) is equal to the equilibrium constant (Keq). To determine whether a system is at equilibrium, you compare the values of Q and Keq.
The reaction quotient (Q) is calculated using the same formula as the equilibrium constant (Keq), but it is calculated at any given point in time during the reaction, not just at equilibrium. Q is found by substituting the concentrations (or pressures for gaseous species) of the reactants and products into the equilibrium expression.
There are three possible cases:
1. If Q is greater than Keq (Q > Keq), it means that there is an excess of products compared to the equilibrium state, suggesting that the reaction is not yet at equilibrium and will proceed in the reverse direction to reach it.
2. If Q is less than Keq (Q < Keq), it means that there is an excess of reactants compared to the equilibrium state, suggesting that the reaction is not yet at equilibrium and will proceed in the forward direction to reach it.
3. If Q is equal to Keq (Q = Keq), it means that the system is already at equilibrium. The concentrations (or pressures) of the reactants and products are already in their equilibrium proportions, and there is no net change in concentration over time.
So, in summary, when Q is equal to Keq (Q = Keq), the system is at equilibrium.