If the ∆H is positive and the ∆S is positive, then the reaction is entropy driven. If the ∆H is negative and the ∆S is negative, then the reaction is enthalpy driven. If ∆H is positive and ∆S is negative, then the reaction is driven by neither of these. If ∆H is negative and ∆S is positive, then the reaction is driven by both of these.
An exergonic reaction will usually give off heat while endergonic will get colder. Exergonic reactions give off energy in the form of heat (prefix "ex"=outward) while endergonic reactions absorb energy, giving the products of the reaction more energy than the reactants.
Exothermic, because the reaction enthalpy must be negative. With polymerization, the entropy decreases. The Gibbs energy has to be negative. Thus negative reaction enthalpy. Gibbs energy = reaction enthalpy - temperature*entropy
Stability of the products as compare to stability of reactants.
Enthalpy is the amount of energy released or used when kept at a constant pressure. Entropy refers to the unavailable energy within a system, which is also a measure of the problems within the system.
S > 0 contributes to spontaneity.
The change in enthalpy between products and reactants in a reaction
Exothermic, because the reaction enthalpy must be negative. With polymerization, the entropy decreases. The Gibbs energy has to be negative. Thus negative reaction enthalpy. Gibbs energy = reaction enthalpy - temperature*entropy
Stability of the products as compare to stability of reactants.
True, a large positive value of entropy tends to favor products of a chemical reaction. However, entropy can be offset by enthalpy; a large positive value of enthalpy tends to favor the reactants of a chemical reaction. The true measure to determine which side of a chemical reaction is favored is the change in Gibbs' free energy, which accounts for both entropy and enthalpy, as calculated by: Change in Gibbs = Change in Enthalpy - Temp in Kelvin * Change in Entropy A negative value of Gibbs free energy will always favour the products of a chemical reaction.
Temperature and energy are two of the variables included when graphing enthalpy and entropy. Enthalpy is made up of the energy, pressure, and volume of a system. Entropy is a way to determine the different ways energy can be arranged.
To feed the rise in Entropy. Enthalpy is a constant, but Entropy is always increasing.
Enthalpy is the amount of energy released or used when kept at a constant pressure. Entropy refers to the unavailable energy within a system, which is also a measure of the problems within the system.
Synthesis reactions such as dehydration synthesis. For a reaction to proceed the there must be a net decrease in the Gibbs Free Energy of the system. The Gibbs Free Energy is made up of two terms: Enthalpy or Heat Content H Entropy S For a reaction in which the entropy is increasing to proceed there would have to be a sufficient release of heat content (enthalpy) such that Change in Free Energy G would be negative, ie decrease...
Enthalpy- positive Entropy- decreasing Free energy- negative
S > 0 contributes to spontaneity.
The change in enthalpy between products and reactants in a reaction
Chemical reactions are driven by the amount of energy used to break the bonds in the reactants ( the activation energy) and the energy released by making new bonds in the products. The stronger the forces holding together the molecules of products, the more readily the reaction takes place. The difference between the energy produced in making the bonds and breaking the bonds is called ENTHALPY. The reaction can also be driven if the products have a greater degree of disorder (ENTROPY) than the reactants.
An increase in entropy.