
What is Gibbs free energy in Electrochemistry?
Answer
417.3k+ views
Hint: First we know electrochemistry is the study of chemical processes that cause electrons to move. The Gibbs free energy is the available energy of a substance that can be used in a chemical reaction. Substances tend to transform into other substances that have less Gibbs free energy. The change of Gibbs free energy predicts whether a chemical reaction will occur spontaneously.
Complete answer:
The Gibbs free energy is the energy associated with a chemical reaction and is equal to the difference between the enthalpy (\[\Delta H\]) of a system and the product of its entropy (\[\Delta S\]) and absolute temperature( \[T\]).
At constant temperature and pressure, the change in Gibbs free energy is defined as \[\Delta G = \Delta H - T\Delta S\] .
Reactions that have a negative \[\Delta G\] release free energy and are called exergonic reactions. A negative \[\Delta G\] means that the reactants (initial state), have more free energy than the products (final state).
Gibbs free energy is a derived quantity that combines enthalpy and entropy into a single value. If the free energy is negative, we are looking at changes in enthalpy and entropy that favour the process and it occurs spontaneously. A spontaneous reaction is one that releases free energy, and so the sign of \[\Delta G\] must be negative.
Note:
Note that the movement of electrons in chemical processes is called electricity, which can be generated by movements of electrons from one element to another in a reaction known as redox (an oxidation-reduction) reaction. Exergonic means energy is exiting the system.
Complete answer:
The Gibbs free energy is the energy associated with a chemical reaction and is equal to the difference between the enthalpy (\[\Delta H\]) of a system and the product of its entropy (\[\Delta S\]) and absolute temperature( \[T\]).
At constant temperature and pressure, the change in Gibbs free energy is defined as \[\Delta G = \Delta H - T\Delta S\] .
Reactions that have a negative \[\Delta G\] release free energy and are called exergonic reactions. A negative \[\Delta G\] means that the reactants (initial state), have more free energy than the products (final state).
Gibbs free energy is a derived quantity that combines enthalpy and entropy into a single value. If the free energy is negative, we are looking at changes in enthalpy and entropy that favour the process and it occurs spontaneously. A spontaneous reaction is one that releases free energy, and so the sign of \[\Delta G\] must be negative.
Note:
Note that the movement of electrons in chemical processes is called electricity, which can be generated by movements of electrons from one element to another in a reaction known as redox (an oxidation-reduction) reaction. Exergonic means energy is exiting the system.
Recently Updated Pages
Master Class 12 Business Studies: Engaging Questions & Answers for Success

Master Class 12 English: Engaging Questions & Answers for Success

Master Class 12 Social Science: Engaging Questions & Answers for Success

Master Class 12 Chemistry: Engaging Questions & Answers for Success

Class 12 Question and Answer - Your Ultimate Solutions Guide

Master Class 12 Economics: Engaging Questions & Answers for Success

Trending doubts
Give 10 examples of unisexual and bisexual flowers

Draw a labelled sketch of the human eye class 12 physics CBSE

Differentiate between homogeneous and heterogeneous class 12 chemistry CBSE

Differentiate between insitu conservation and exsitu class 12 biology CBSE

What are the major means of transport Explain each class 12 social science CBSE

Franz thinks Will they make them sing in German even class 12 english CBSE
