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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.
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How will the temperature affect the spontaneity of a reaction with positive h and s?
A high temperature will make it spontaneous.
According to the Gibbs free energy equation G H - TS when could a high temperature make a reaction that was nonspontaneous at low temperature spontaneous?
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.
When is rxn non spontaneous?
A reaction is considered non-spontaneous when the Gibbs free energy change (ΔG) is positive, indicating that the reaction requires an input of energy to occur. This could happen when the reactants have high energy relative to the products or when the reaction conditions do not favor the formation of products.
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.
What conditions will cause a redox reaction to be no spontaneous?
A redox reaction will not be spontaneous if the standard cell potential (E°) is negative, indicating that the reaction favors the reactants rather than the products. Additionally, high activation energy barriers, unfavorable temperature conditions, or the presence of competing reactions can also hinder spontaneity. In such cases, external energy input may be required to drive the reaction forward.
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.
When Could A High Temperature Make A Reaction That Was Nonspontaneous At Low Temperature Spontaneous?
A high temperature can make a nonspontaneous reaction spontaneous by providing enough energy to overcome the activation energy barrier, allowing the reaction to proceed. At low temperatures, the kinetic energy of the molecules may not be sufficient for them to react, but increasing the temperature can provide the necessary energy for the reaction to occur spontaneously.
How will the temperature affect the spontaneity of a reaction with positive h and s?
A high temperature will make it spontaneous.
A chemical reaction has a positive H value and a positive S value Under what conditions is the reaction spontaneous?
The spontaneity of a reaction is determined by the sign of the Gibbs free energy (ΔG). If both enthalpy (H) and entropy (S) are positive, the reaction can be spontaneous at high temperatures where the TΔS term outweighs the positive ΔH term, resulting in a negative ΔG. This means the reaction will be spontaneous at elevated temperatures.
According to the Gibbs free energy equation G H - TS when could a high temperature make a reaction that was nonspontaneous at low temperature spontaneous?
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.
A chemical reaction has a positive ΔH value and a positive ΔS value Under what conditions is the reaction spontaneous?
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.
How will temperature affect the spontaneity of reaction with positive H and S?
A high temperature will make it spontaneous.
When is rxn non spontaneous?
A reaction is considered non-spontaneous when the Gibbs free energy change (ΔG) is positive, indicating that the reaction requires an input of energy to occur. This could happen when the reactants have high energy relative to the products or when the reaction conditions do not favor the formation of products.
What part is in charge of automatic processes?
In science, Gibbs free energy can tell if a chemical reaction is spontaneous. It is given by the formula: G = H - TS H = enthalpy of reaction S = entropy of reaction T = temperature in Kelvin If G is negative the reaction is spontaneous. However if activation energy is high, reaction rate is slow and the reaction may take a while to progress, regardless of its 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.
What conditions will cause a redox reaction to be no spontaneous?
A redox reaction will not be spontaneous if the standard cell potential (E°) is negative, indicating that the reaction favors the reactants rather than the products. Additionally, high activation energy barriers, unfavorable temperature conditions, or the presence of competing reactions can also hinder spontaneity. In such cases, external energy input may be required to drive the reaction forward.
How will temperature affect the spontaneity of a reaction with positive AH and AS?
For a reaction with a positive enthalpy change (ΔH > 0) and a positive entropy change (ΔS > 0), the spontaneity is influenced by temperature according to the Gibbs free energy equation: ΔG = ΔH - TΔS. As temperature increases, the term TΔS becomes larger, which can help drive ΔG to be negative, indicating spontaneity. Therefore, at sufficiently high temperatures, the reaction can become spontaneous despite the positive ΔH. Conversely, at low temperatures, the reaction may not be spontaneous.
