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I know a negative delta g means the reaction is spontaneous. A positive delate g means the reaction is not spontaneous. But does a negative delta g means the reaction favors products and a positive delta g means the reaction favors reactants.
If you have a delta G that is negative which means that the reaction is spontaneous, then the reaction does not need energy to proceed. In other words, it will occur on its own without any external intervention. Because this reaction occurs spontaneously without the input of energy, this means that the products are more stable and thus favored than the reactants. So, this means that if you have a spontaneous reaction, the products are favored, whereas if you have a non spontaneous reaction where the delta G is positive, the reaction will not occur unless energy supplied, this means that the energy of the products is greater than the reactants and thus most likely less stable. The forward reaction will not be favorable in that case.
Yes because a spontaneous reaction means that the reaction is more likely to proceed and more products are likely to form. If a reaction is not spontaneous, the reactants are unlikely to form products, so the reverse reaction is favored.
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