Final answer:
The molecular reactions do not remain constant in a system at dynamic equilibrium. Changes in temperature affect the equilibrium constant (K), and pressure changes only affect systems involving gases and a change in the number of moles of gases.
Step-by-step explanation:
When a system is at dynamic equilibrium, its pH, pressure, and temperature usually remain constant. However, molecular reactions do not remain constant; instead, reactions continue to occur at equal rates in both the forward and reverse directions.
A change in temperature shifts the equilibrium constant, K. This can be understood by applying Le Chatelier's principle which states that the system will adjust to minimize the effect of the change.
It is essential to note that changes in pressure only have a significant effect if gases are involved and there is a change in the number of moles of gases during the reaction.