What equation is used to calculate the free change of a reaction?

Delta G (written triangle G) = Delta H -T Delta S

If you know the standard state free energy change, you can calculate the temperate and delta G of a reaction by doing the formula triangle G0 = -RT ln Keq.

It depends on if you are calculating the amount of usable energy from a reaction or the change in enthalpy. To calculate the Change in enthalpy of a chemical reation: ΔHreaction= ΣΔHfO (Products) - ΣΔHfO (Reactants) Which is the sum of the standard enthalpy change of formations of the products (multiplied by their balanced coefficients) minus the sum of the standard enthalpy change of formations of the reactants (also multiplied by their balanced coefficients). This is to say, in the equation: aA + bB -> cC + dD ΔHreaction = [( c x ΔHfO C) + (d x ΔHfO D) ] - [( a x ΔHfO A) + (b x ΔHfO B) ] However, the amount of usable of a reaction is given by ΔG or the change in Gibb's free energy. Gibb's free energy is the change in enthalpy minus the change in entropy multiplied by the temperature: ΔG = ΔH - TΔS Where T is the temperature in kelvin and ΔS is the change in entropy.

An exergonic reaction is a change in free energy to negative. It is a chemical reaction indicating a spontaneous reaction.

Gibbs free energy, DG, determines if a reaction is spontaneous or not at a certain temperature. A reaction is spontaneous if it occurs with no outside intervention. If the value of DG is negative, then the reaction is spontaneous. If DG is positive then the reaction is not spontaneous. The equation for Gibbs free energy has three components, the enthalpy change, DH, a Kelvin temperature, and the change in entropy, DS. DG = DH - TDS The enthalpy change represents the amount of thermal energy that a reaction either absorbs or releases to the environment. DH is the enthalpy of the products minus the enthalpy of the reactants. But keep in mind that we never now the actual beginning and ending enthalpy of a system, we only know the change in enthalpy

methane+oxygen ---> heat energy+carbon dioxide I think this is correct. Feel free to change it, if it is wrong!!

An endergonic reaction is a chemical reaction in which the standard change in free energy is positive.

Endergonic reaction is a chemical reaction in which the standard change in free energy is positive, and energy is absorbed. Exergonic reaction is a chemical reaction in which the free energy is negative.

If the free energy associated with a reaction is negative, that means the reaction is spontaneous in nature and is thermodynamically feasible.Such a reaction is exothermic and energy is released in it.

Positive (greater than 0).

Zero, if you mean what is the free energy change.

Yes. An exergonic reaction is a reaction with a negative change in Gibbs Free Energy. By definition, this is a spontaneous reaction.

she realizes she is free

Enthalpy is one of the factors involved in calculating the Gibbs free energy, which determines the spontaneity of a reaction. Gibbs free energy change = Enthalpy change - absolute temperature x entropy change. If the Gibbs free energy change is negative then the reaction is spontaneous. This depends on the balance between enthalpy and entropy changes, and also the temperature. The enthalpy change is negative when the reaction is exothermic, and this obviously favours spontaneity, but it is not sufficient alone.

The reaction is spontaneous below 743 K.

The reaction is spontaneous below 554.8/0.1975 K.

If the sign of ΔH is _______ and the sign of ΔS is _______ , then the magnitude of TΔS must be ________ than the magnitude of ΔH for the reaction to be spontaneous. The Gibbs free energy equation is ΔG = ΔH - TΔS. negative; negative; less

The symbol is delta (a triangle) and a capital G. This symbolizes Gibbs free energy. A negative sign means it's spontaneous; a positive sign means non-spontaneous.

Enzymes are biological catalysts. They speed up biochemical reaction. During the course of a reaction, the enzyme molecules do not get consumed. At the end of a reaction, the enzyme molecules are ready for another reaction. Enzymes are able to catalyze reactions by decreasing the free energy change (delta G) associated with a biochemical reaction. When the reactants have to go through a smaller free energy change, the products are formed faster.

endergonic is a reaction under which energy is stored in a chemical reaction in which the standard change in free energy is positive, and energy is absorbed. yourwelcome.<3

The reaction is spontaneous above 371 K.

If they are charged particles formed during a reaction the immediately form ethyl alcohol but the don't exist as free units, the reaction for formation of ethyl alcohol is as follows, C2H5-Cl + NaOH = C2H5-OH + NaCl

Endergonic means "absorbing energy in the form of work." Endergonic reactions are not spontaneous. An exergonic reaction is a chemical reaction where the change in the free energy is negative, indicating a spontaneous reaction.

δg = (-992.0) - (298)(-294.6)(1/1000)

the gibbs free energy for the reaction is positive