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∆G = ∆H - T∆S and for it to be spontaneous, ∆G should be negative. If both ∆H and ∆S are positive, in order to get a negative ∆H, the temperature needs to be elevated in order to make the ∆S term greater than the ∆H term. So, I guess the answer would be "the higher the temperature, the more likely will be the spontaneity of the reaction."
If G < 0, the reaction is spontaneous.
Delta G (written triangle G) = Delta H -T Delta S
Photosynthesis is a positive delta G as it produces more free energy than it uses. The overall result of the Gibbs equations shows that delta G is positive
The change in enthalpy between products and reactants in a reaction
∆G = ∆H - T∆S and for it to be spontaneous, ∆G should be negative. If both ∆H and ∆S are positive, in order to get a negative ∆H, the temperature needs to be elevated in order to make the ∆S term greater than the ∆H term. So, I guess the answer would be "the higher the temperature, the more likely will be the spontaneity of the reaction."
∆G = ∆H - T∆S and ∆G has to be negative for the reaction to be spontaneous. So, ultimately the effect of temperature will depend on the value of ∆H. If ∆H is negative, and ∆S is positive, then temperature won't matter, and reaction will be spontaneous. If ∆H is positive, and ∆S is positive, then a high temperature will favor spontaneity. If ∆H is negative and ∆S is negative, then a low temperature will favor spontaneity. So, the answer to your question is the higher the temperature the more likely the reaction will occur spontaneously.
If G < 0, the reaction is spontaneous.
enzymes dont affect the delta G, they only lower the activation energy. Therefore, the delta G stays the same
Delta G (written triangle G) = Delta H -T Delta S
The usable energy released or absorbed by a reaction.
Delta G (written triangle G) = Delta H -T Delta S
Delta G (written triangle G) = Delta H -T Delta S
When a chemical reaction has a negative delta G, the reaction is exothermic because delta G is the change in energy of a system and the change in its entropy. If the effect of a reaction is to reduce G, the process will be spontaneous so delta G is negative. Hope this helps :)
G is always positive when enthalpy increases and entropy decreases.
Photosynthesis is a positive delta G as it produces more free energy than it uses. The overall result of the Gibbs equations shows that delta G is positive
The change in enthalpy between products and reactants in a reaction