stability of reactants and products

[Cynthia Ulloa]

How do we describe the stability of reactants and products when we look at which reaction is favored?

[Neil Hsu 2A]

Whether the forward or reverse reaction is favored gives us a hint to the stability of the products: if the reaction is spontaneous, then the reaction will tend toward the product, so the product is more stable. On the other hand, if the reaction is not spontaneous, then the reaction will tend towards the reactants, which means that the reactants are more stable. You can see if the reaction is spontaneous by looking at delta G, E or K.

[Dayna Pham 1I]

If K is less than 10^-3, there are more reactants at equilibrium. Therefore, the reactants are strongly favored. The reactants are more stable than the products.

If K is greater than 10^3, there are more products at equilibrium. Therefore, the products are strongly favored. The products are more stable than the reactants.

[Mark 1D]

Spontaneous reaction means products are more stable whilst spontaneous means the reactants will be more stable