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Answers
Explanation:
Systems in equilibrium are balanced. For example, if you are running on a treadmill you are in constant motion. However, you are not moving forward or backwards. As fast as you run forward the treadmill is moving you backwardsh. You are in equilibrium with the treadmill.
In the same way chemical reactions can be in equilibrium (the products and reactants are produced at the same rate). We will begin by exploring chemical equilibrium in more detail. Ways of measuring equilibrium and the factors that affect equilibrium will be covered.
haemoglobin(aq) + \(4\text{O}_{2}(\text{g})\) \(\rightleftharpoons\) haemoglobin(\(\text{O}_{2})_{4}\)(aq)
Answer:
Chemical equilibrium refers to the state of a system in which the concentration of the reactant and the concentration of the products do not change with time and the system does not display any further change in properties.
There are two types of chemical equilibrium:
☆Homogeneous Equilibrium
☆Heterogeneous Equilibrium
Homogenous Chemical Equilibrium
In this type, the reactants and the products of chemical equilibrium are all in the same phase. Homogenous equilibrium can be further divided into two types: Reactions in which the number of molecules of the products is equal to the number of molecules of the reactants. For example,
H2 (g) + I2 (g) ⇌ 2HI (g)
N2 (g) + O2 (g) ⇌ 2NO (g)
Reactions in which the number of molecules of the products is not equal to the total number of reactant molecules. For example,
2SO2 (g) + O2 (g) ⇌ 2SO3 (g)
COCl2 (g) ⇌ CO (g) + Cl2 (g)
Heterogeneous Chemical Equilibrium
In this type, the reactants and the products of chemical equilibrium are present in different phases. A few examples of heterogeneous equilibrium are listed below.
CO2 (g) + C (s) ⇌ 2CO (g)
CaCO3 (s) ⇌ CaO (s) + CO2 (g)
Thus, the different types of chemical equilibrium are based on the phase of the reactants and products.
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