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                                            THERMODYNAMICS

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                                            THERMODYNAMICS

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                                  So what is Thermodynamics?

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                                  So what is Thermodynamics?

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Thermodynamics is a branch of physics that explains the affect of work, heat, and energy on a system. It helps understand the relationship between heat and other forms of energy. The laws of Thermodynamics show us how the energy in a system changes and if the system can do work on its surrounds. 

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Thermodynamics is a branch of physics that explains the affect of work, heat, and energy on a system. It helps understand the relationship between heat and other forms of energy. The laws of Thermodynamics show us how the energy in a system changes and if the system can do work on its surrounds. 

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Before things get *heated*, lets go over some terminology to get some knowledge into our *systems* ;)

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Before things get *heated*, lets go over some terminology to get some knowledge into our *systems* ;)

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Energy being transferred from one system (ex. engine) to another

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Variables that make up the state of the system such as internal energy, enthalpy, entropy, and free energy...almost like ingredients.

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Reversible: when the system and environement are able to return to their previous state

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Irreversible: when the system and environment cannot return to their previous state

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System: the molecules that are reacting

Surroundings: Everything else around the system

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Measure of disorder in a system and amount of energy unavailable to do work.

More disorder = higher entropy

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Sum of internal energy and product of pressure and volume in a system.
H = E + PV. Reflects capacity to release heat

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Maximum amount of available work that can be take from a system under constant temperature and pressure.

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The Three Laws of Thermodynamics include:

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The Three Laws of Thermodynamics include:

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Also, known as the Law of Conservation of Energy states, energy cannot be created or destroyed but it can be transferred from one location to another and transformed into other forms of energy. The mathematical representation of this first law is   ΔU=q+w .

ΔU = total change in internal energy of a system

q = heat exchanged between system and surroundings

w = work done by or on the system

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The importance of this law is it applies to many aspects of our lives such as the air conditioning system, light bulbs, energy from food, etc.

The first example of how this law applies to real life is in our light bulbs. Light bulbs transform electrical energy into light energy. Electrical energy is also transformed into the energy used to light our computer screens and create sound energy to listen to music.

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In plants, the first law can also be applied because plants turns light energy from the sun into chemical energy which it uses to grow and make food.

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Second Law: Spontaneous and Non-Spontaneous process 

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Second Law: Spontaneous and Non-Spontaneous process 

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The second law of thermodynamics states that the entropy of any isolated system will always increase. Isolated systems spontaneously evolve towards thermal equilibrium which is the state of maximum entropy of the system.

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Second law of Thermodynamics is very important as it talks about entropy. We used the second law in our everyday life when using temperature and heat.
Example: Putting an ice cube into a cup with water at room temperature or leaving a cup of coffee out for more than 5 minutes. When both ice cubes start to melt and coffee gets cold the entropy will result in the water to decrease, therefore its entropy increases.

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       Spontaneous and Non-spontaneous relations 

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       Spontaneous and Non-spontaneous relations 

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•Spontaneous - the reaction which proceeds in the given direction without the need of outside force or energy is called spontaneous.

•Non spontaneous - the reaction which needs external force or energy in order to proceed in given direction is nonspontaneous reaction.

•To predict spontaneity, we check the Gibbs free energy if this is negative then the reaction is spontaneous. And if Gibbs free energy is positive then it is said to be non-spontaneous.

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The melting of ice into water happens spontaneously as soon as ice is left at room temperature. Ice is a solid with an ordered crystalline structure as compared to water, which is a liquid in which molecules are more disordered and randomly distributed.

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Spontaneous reaction example:                                                                                                                                                                                                          

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Spontaneous reaction example:                                                                                                                                                                                                          

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The rusting of iron is spontaneous and is accompanied by a decrease in the entropy of the system.

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-Reaction of atmospheric nitrogen and oxygen

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Definition of the "Third law of Thermodynamics"

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Definition of the "Third law of Thermodynamics"

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In simple terms ,the third law states that the entropy of a perfect crystal approaches zero as the absolute temperature approaches zero.This law provides an absolute reference point for the determination of entropy.

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How is the Third law of thermodynamics used in daily life?

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How is the Third law of thermodynamics used in daily life?

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The daily use of the Third law of thermodynamics allows us to define the sign of the entropy of any substance at temperatures above absolute zero and also it provides a fixed reference point that allows us to measure the absolute entropy of any substance at any temperature.

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Relationship between Enthalpy,Free Energy and Entropy.

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Relationship between Enthalpy,Free Energy and Entropy.

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Gibbs free energy combines enthalpy and entropy into a single value.

Gibbs free energy is the energy associated with a chemical reaction that can do useful work. It equals the enthalpy minus the product of the temperature and entropy of the system.

G = H – TS

At constant temperature

ΔG = ΔH – TΔS

ΔG predicts the direction of a chemical reaction. If ΔG is negative, then the reaction is spontaneous. If ΔG is positive, then the reaction is non-spontaneous.