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In the Gibbs free energy equation ( G = H - TS ), a reaction can become spontaneous at high temperatures if the entropy change (( \Delta S )) is positive and the enthalpy change (( \Delta H )) is either positive or less negative. As the temperature (( T )) increases, the ( -TS ) term becomes more significant, potentially outweighing a positive ( \Delta H ) and resulting in a negative ( \Delta G ). This indicates that at sufficiently high temperatures, the increased disorder associated with the reaction can drive the process forward, making it spontaneous.
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Ask us anythingAccording to the Gibbs free energy equation G H - TS when could a high temperature make a reaction that was nonspontaneous at low temperature spontaneous?
A reaction that is nonspontaneous at low temperatures can become spontaneous at high temperatures if the entropy change (ΔS) is positive and the enthalpy change (ΔH) is either positive or less negative. In the Gibbs free energy equation (G = H - TS), as temperature (T) increases, the term -TS becomes more negative, which can lower the Gibbs free energy (G). If the increase in entropy at high temperatures outweighs the enthalpic costs, G can turn negative, indicating spontaneity.
On what conditions does a spontaneous reaction become spontaneous?
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.
When could a high temperature make a reaction that was non spontaneous at a low temperature spontaneous?
A high temperature can make a reaction that is non-spontaneous at low temperatures spontaneous if the reaction has a positive entropy change (ΔS > 0) and a negative enthalpy change (ΔH < 0). According to the Gibbs free energy equation (ΔG = ΔH - TΔS), increasing the temperature (T) can make the term -TΔS more significant, potentially turning ΔG negative and indicating spontaneity. This is particularly relevant for reactions that are endothermic (positive ΔH) but have a large increase in disorder.
The equation G equals H-TS predicts that?
the Gibbs free energy (G) of a system is equal to the enthalpy (H) minus the temperature (T) multiplied by the entropy (S). This equation is used to determine whether a reaction is spontaneous (ΔG < 0) or non-spontaneous (ΔG > 0) at a given temperature.
When is a reaction always spontaneous according to Gibbs free energy equation?
A reaction is always spontaneous when the change in Gibbs free energy (ΔG) is negative (ΔG < 0). This occurs when the system's enthalpy change (ΔH) is negative and the entropy change (ΔS) is positive, or when the temperature is sufficiently low to make the term TΔS (where T is temperature) less significant compared to ΔH. In summary, spontaneous reactions can be identified by a negative ΔG value, indicating that they can occur without external input.
According to the Gibbs free energy equation G H - T S when could a high temperature make a reaction that was nonspontaneous at low temperature spontaneous?
A high temperature could make a reaction spontaneous that was nonspontaneous at low temperature when the increase in entropy due to the reaction outweighs the increase in enthalpy. At higher temperatures, the TΔS term in the Gibbs free energy equation becomes more dominant, leading to a positive ΔG becoming negative, thus making the reaction spontaneous.
On what conditions does a spontaneous reaction become spontaneous?
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.
Using the Gibbs free energy equation what is the temperature range for which the oxidation of lead is spontaneous?
The reaction is spontaneous below 554.8/0.1975 K.
Use the gibbs free energy equation shown below to determine the temperature for which the decomposition of KClO4 is spontaneous?
To determine the temperature at which the decomposition of KClO4 is spontaneous, you need to know the Gibbs free energy change (∆G) for the reaction. If ∆G is negative, the reaction is spontaneous. Use the equation ∆G = ∆H - T∆S, where ∆H is the enthalpy change, ∆S is the entropy change, and T is the temperature in Kelvin. Set ∆G to 0 and solve for T to find the temperature at which the decomposition becomes spontaneous.
According to the Gibbs free energy equation what is the temperature range for which the formation of liquid bromine is spontaneous?
The formation of liquid bromine is spontaneous when the Gibbs free energy change for the process is negative, which occurs when ΔG < 0. This means the temperature must be within the range where ΔG is negative, which typically corresponds to temperatures above the boiling point of bromine (~332K) where the entropy term dominates over the enthalpy term in the Gibbs free energy equation.
Using the Gibbs free energy equation what is the temperature in degrees celsius above which decompostion of KCIO4 is spontaneous?
-51 - -50.5
Use the Gibbs free energy equation shown below to determine the temperature range for which the decomposition of KCIO4 is spontaneous?
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.
At which temperature would a reaction with H-92kJmol S-0.199kJmol(mol.K) be spontaneous?
A reaction will be spontaneous at a given temperature if the Gibbs free energy change (ΔG) is negative. ΔG = ΔH - TΔS. As ΔH = -92 kJ/mol and ΔS = -0.199 kJ/(mol.K), plug these values into the equation along with the temperature to solve for ΔG. If ΔG is negative, the reaction will be spontaneous at that temperature.
Which equation represents a spontaneous nuclear decay?
All nuclear decay is spontaneous.
What is the Delta G prime equation used for in thermodynamics?
The Delta G prime equation is used in thermodynamics to calculate the standard Gibbs free energy change of a chemical reaction under standard conditions. It helps determine whether a reaction is spontaneous or non-spontaneous at a given temperature.
The equation G equals H-TS predicts that?
the Gibbs free energy (G) of a system is equal to the enthalpy (H) minus the temperature (T) multiplied by the entropy (S). This equation is used to determine whether a reaction is spontaneous (ΔG < 0) or non-spontaneous (ΔG > 0) at a given temperature.
What temperature is a reaction spontaneous?
A reaction is considered spontaneous when it occurs without external intervention, typically at a specific temperature where the Gibbs free energy change (ΔG) is negative (ΔG < 0). The temperature at which a reaction becomes spontaneous can vary depending on the enthalpy (ΔH) and entropy (ΔS) changes associated with the reaction, as expressed in the Gibbs free energy equation: ΔG = ΔH - TΔS. If the entropy increases (ΔS > 0), the reaction may be spontaneous at lower temperatures, while if the enthalpy is favorable (ΔH < 0), it may be spontaneous at higher temperatures.
