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Answer: B. the products have a smaller number of available energy microstates than the reactants
Explanation:
Entropy [tex]S[/tex] is a thermodynamic quantity defined as a criterion to predict the transformation of thermodynamic systems.
In other words: Entropy is the measure of the disorder (or randomness) of a system and is a function of state. That is, it depends only on the state of the system.
However, as there is chaos that threatens to destroy a system, there are also self-regulation mechanisms, which allow the level of disorder to drop or remain balanced, so that the existence of the system remains; this is known as negative entropy.
To undersand it better:
In the specific case of a reaction, its variation in entropy [tex]\Delta S[/tex] is matematically expressed as:
[tex]\Delta S=S_{products}-S_{reactants}[/tex] (1)
Where:
[tex]S_{products}[/tex] is the entropy of the products of the reaction
[tex]S_{reactants}[/tex] is the entropy of the reactants of the reaction
Now, remembering entropy is a function of the state of the system, if [tex]S_{reactants}[/tex] have a greater amount of available energy microstates than [tex]S_{products}[/tex], the variation in entropy of the system [tex]\Delta S[/tex] will be negative.
B. the products have a smaller number of available energy microstates than the reactants
Further Explanation
The second law of thermodynamics is expressed more in other state functions, namely entropy (S), entropy in the second law is allowed to recognize the spontaneous change.
Second law: Entropy of an isolated system increases as long as there is a spontaneous change with the formula: ∆Stot> 0
A static definition of entropy is formulated: S = k ln W
With k as the boltzman constant with the value k = 1,318 x 10 ^ 23 J / K, and W is the number of ways that the energy of the system is the arrangement of atoms in the existing state.
In a heat-isolated system, entropy runs only in one direction (not a reversible process).
The entropy of a system needs to be measured to determine that energy cannot be used to do business on thermodynamic processes. These processes can only be carried out by energy that has been transformed, and when energy is converted into work/effort, it theoretically has a certain maximum efficiency. During the work/effort, entropy will accumulate in the system, which is then dissipated in the form of waste heat.
In classical thermodynamics, the concept of entropy is defined in the second law of thermodynamics, which states that the entropy of an isolated system always increases or remains constant. Thus, entropy can also be a measure of the tendency of a process, whether the process tends to be "entroped" or will take place in a certain direction. Entropy also shows that heat energy always flows spontaneously from areas of higher temperature to areas of lower temperature.
Thermodynamic entropy has an energy dimension divided by temperature, which has an International Unit of joules per kelvin (J / K).
To carry out this kind of process the system is connected to a different temperature reservoir. If a hot current flows into the system, then Qr is positive and the entropy of the system increases. If the heat flow out of the Qr system is negative and the entropy of the system drops. If in a process there is a reversible heat flow between the system and its environment, then essentially the system temperature and ambient temperature are the same. The amount of this heat flow that enters the system or enters the environment at each point is the same, but must be marked opposite. Therefore the change in environmental entropy is equal but opposite the sign with the change in system entropy and the number becomes zero. Because the system together with its environment forms the world, it may be said that the entropy of the world is permanent. It should be remembered that this statement applies to the reversible process only.
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Grade: High School
Subject: Physics
keywords: entropy
