when h and s are both positive
To determine the temperature range at which the decomposition of KClO4 is spontaneous, you would need the values for the standard Gibbs free energy change (ΔG°) and the equilibrium constant (K). By using the equation ΔG = -RTlnK and taking into account that ΔG = 0 for a reaction at equilibrium, you can rearrange to solve for the temperature range where decomposition is spontaneous.
when H is negative and S is positive
Temperature and activation energy
The reaction will be spontaneous at high temperatures (T) where TΔS > ΔH, according to Gibbs free energy equation, ΔG = ΔH - TΔS. At high enough temperatures, the TΔS term can outweigh the positive ΔH term, leading to a negative ΔG value and a spontaneous reaction.
Temperature and activation energy - apex
The reaction is spontaneous below 743 K.
For some non-spontaneous reactions, you can change the temperature. For other non-spontaneous reactions, there is nothing you can do to make it spontaneous. Nature favors reactions that increase a system's entropy (disorder) and nature favors reactions that are exothermic (they release enthalpy). Any reaction that does both of these things is spontaneous at all temperatures. Any reaction that does neither of these things is never spontaneous. As far as this question is concerned, the interesting reactions are endothermic reactions that increase entropy and exothermic reactions that decrease entropy. Whether these reactions are spontaneous depends on the temperature. The first variety (endothermic, increase entropy) will be spontaneous at high temperatures; the second (exothermic, decrease entropy) will be spontaneous at low temperatures. To find the temperature at which a reaction becomes spontaneous, one may apply the Gibbs equation: DG = DH - TDS where capital Ds stand for the Greek capital delta.
The reaction is spontaneous below 554.8/0.1975 K.
The reaction is spontaneous above 371 K.
To determine the temperature range at which the decomposition of KClO4 is spontaneous, you would need the values for the standard Gibbs free energy change (ΔG°) and the equilibrium constant (K). By using the equation ΔG = -RTlnK and taking into account that ΔG = 0 for a reaction at equilibrium, you can rearrange to solve for the temperature range where decomposition is spontaneous.
-51 - -50.5
All nuclear decay is spontaneous.
when H is negative and S is positive
Temperature and activation energy
The reaction will be spontaneous at high temperatures (T) where TΔS > ΔH, according to Gibbs free energy equation, ΔG = ΔH - TΔS. At high enough temperatures, the TΔS term can outweigh the positive ΔH term, leading to a negative ΔG value and a spontaneous reaction.
Temperature and activation energy - apex
The change in Gibbs Free Energy (∆Gº) predicts if a reaction is spontaneous or not. The equation for this is ∆G = ∆H - T∆S where ∆H is the change in enthalpy, T is temperature in Kelvin, and ∆S in change in entropy.