This is part of the HSC Chemistry course under the topic of Static and Dynamic Equilibrium, focusing on models. In this post, we model static and dynamic equilibrium and analyse the differences between open and closed systems.
Modelling Open and Closed Systems
In this video, it models dynamic equilibrium by transferring water from one container into another.
In chemistry, equilibrium refers to a state where the rate of a forward reaction is equal to the rate of the reverse reaction. There are two main types of equilibrium: static and dynamic equilibrium.
Static equilibrium occurs when there is no net movement of reactants or products in a reaction. This can occur when a system is closed, and there is no exchange of matter or energy with the surroundings. In a static equilibrium, the concentrations of the reactants and products remain constant over time.
An example of static equilibrium is the dissolution of a sparingly soluble salt, such as calcium sulphate, in water. Once the maximum amount of the salt has dissolved, the concentration of the ions in the solution remains constant.
This video compares the features of static and dynamic equilibrium, running through the properties and differences.
Dynamic equilibrium occurs when the rate of the forward and reverse reactions are equal, and there is a continuous exchange of reactants and products. This type of equilibrium is more common in chemical reactions, where there is an ongoing exchange of matter and energy with the surroundings.
In a dynamic equilibrium, the concentrations of the reactants and products do not remain constant, but their ratio does. An example of dynamic equilibrium is the Haber process, which involves the production of ammonia from nitrogen and hydrogen gas. In this reaction, the forward and reverse reactions occur simultaneously, and the concentration of reactants and products remains constant over time.
In summary, static equilibrium occurs when there is no net movement of reactants or products, while dynamic equilibrium occurs when the rate of the forward and reverse reactions are equal and there is a continuous exchange of reactants and products.
Open and Closed Systems
This video goes through the differences in the properties between open, closed and isolated systems.
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