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
If G < 0, the reaction is spontaneous.
To become spontanious,energy should be released.
This is a spontaneous reaction.
a non spontaneous reaction is a reaction that doesnt occur naturally and it normally tends to favor the reactants of a chemical reaction. Another thing is that it doesnt really produce free energy
The first of two factors that determine whether a reaction is spontaneous or non-spontaneous is entropy. The second is energy. For a reaction to be spontaneous, it must have both of these factors.
The reaction is spontaneous below 743 K.
The reaction is spontaneous below 554.8/0.1975 K.
The reaction is spontaneous above 371 K.
when H is negative and S is positive
a spontaneous reaction
If G < 0, the reaction is spontaneous.
It tells if the reaction will process spontaneously or not
To become spontanious,energy should be released.
it doesn't its energy releasing reaction
An exothermic reaction (often a spontaneous one)
Reactions are described by this equation: GD = HD - TDS where D = delta for change in values. GD < 0 spontaneous HD < 0 exothermic ; HD > 0 endothermic The first equation is Gibbs free energy. When G is negative, the reaction is spontaneous. In contrast, a positive number G is non spontaneous. The interesting thing is that spontaneous reactions can be EITHER exothermic and endothermic. Lets look at this: lets assume HD has a value of 100. This means TDS would have to be bigger than 100 in order to make GD a negative number. An endothermic reaction which has a positive H can still be exothermic. Here's another way to pose your question: Is an exothermic reaction spontaneous? Always. Is an endothermic reaction spontaneous? This can be either.
It predicts whether or not a reaction will be spontaneous.