This relation is NOT valid in general at all.mjbm0720 said:Hi
I am new in thermodynamics , and I thought you can help me
If it is valid dG=dW
seems to be correct, assuming that the work done is fully resisted.dG=-Pdv
P=-dG/dv?
siddharth said:Hi mjbm0720, and welcome to the forums.
This relation is NOT valid in general at all.
However, assuming that the relation is valid in a specific situation,
seems to be correct, assuming that the work done is fully resisted.
Is there anything specific you are trying to show?
Gibbs free energy, also known as free enthalpy, is a thermodynamic potential that measures the amount of energy in a system that is available to do useful work.
Gibbs free energy is a fundamental concept in thermodynamics, which is the study of energy and its transformations in systems. It is used to determine whether a chemical reaction will occur spontaneously at a given temperature and pressure.
The Gibbs free energy of a system is calculated using the equation G = H - TS, where G is the Gibbs free energy, H is the enthalpy, T is the temperature in Kelvin, and S is the entropy. It can also be calculated using the equation G = U + PV - TS, where U is the internal energy and PV is the product of pressure and volume.
Gibbs free energy is significant in chemical reactions because it helps determine the spontaneity of a reaction. If the Gibbs free energy is negative, the reaction is spontaneous and can occur without the need for external energy. If the Gibbs free energy is positive, the reaction is non-spontaneous and will not occur without the input of external energy.
Yes, Gibbs free energy can be used to predict the direction of a reaction. If the Gibbs free energy is negative, the reaction will proceed in the forward direction, while a positive Gibbs free energy indicates that the reaction will proceed in the reverse direction. A reaction is at equilibrium when the Gibbs free energy is zero.