Question

how do we determine if a reaction is at equilibrium? q = products/reactants 15) what does (q) represent in the mathematical equation? 16) if q = k: a) the reaction must shift to the right, producing more products. b) the reaction must shift to the left, producing more reactants. c) the reaction is already in a dynamic equilibrium. 17) if q > k: a) the concentrations of reactants and products are stabilized. b) the reaction must shift to the right, producing more products. c) q is larger than k. 18) if q < k:

Explanation:

Step1: Define reaction - quotient

The reaction - quotient $Q$ is the ratio of the concentrations of products to the concentrations of reactants at any given point in a reaction, calculated using the same formula as the equilibrium constant $K$.

Step2: Analyze when $Q = K$

When $Q = K$, the forward and reverse reaction rates are equal, and the reaction is in dynamic equilibrium. So for question 16, the answer is C.

Step3: Analyze when $Q>K$

When $Q>K$, there are too many products relative to reactants compared to the equilibrium state. The reaction will shift to the left to produce more reactants. But among the given options for question 17, the most appropriate answer based on the description is C (although it is more of a restatement of the condition).

Step4: Analyze when $Q

When $Q

Answer:

1. The reaction - quotient, which is the ratio of the concentrations of products to reactants at a particular moment in the reaction.
2. C. The reaction is already in a dynamic equilibrium.
3. C. $Q$ is larger than $K$.
4. A. The reaction must shift to the right, producing more products.