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What is the relationship between the enthalpy h and entropy s of a reaction that is spontaneous at higher temperatures but not at lower temperatures?
-H, +S
What else can I help you with?
Which statement describes a reaction at 298 K if H 31 kJ mol S 0.093 kJ molK?
It is not spontaneous.
What kind of enthalpy change favors a spontaneous reaction?
For a spontaneous reaction, the overall change in enthalpy should be negative (exothermic). This means that the products have a lower enthalpy than the reactants, releasing energy in the form of heat.
How does the Gibbs free energy predict spontaneity?
It tells if the reaction will process spontaneously or not
What can be said about the reaction at 500K?
At 500K, the reaction rate will increase as temperature rises, following the Arrhenius equation. This increase in temperature will also influence the equilibrium position of the reaction if it is a reversible reaction. Higher temperatures can sometimes shift the equilibrium towards the products or reactants, depending on the enthalpy change.
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.
Which statement describes a reaction at 298 K if H 31 kJ mol S 0.093 kJ molK?
It is not 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.
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.
What kind of enthalpy change favors a spontaneous reaction?
For a spontaneous reaction, the overall change in enthalpy should be negative (exothermic). This means that the products have a lower enthalpy than the reactants, releasing energy in the form of heat.
What kind of reaction occurs when the entropy change of an endothermic reaction is negative?
The reaction is exothermic
According to gibb's free energy equation GH-TS When is a reaction always spontaneous?
A reaction is always spontaneous when the change in Gibbs free energy (ΔG) is negative. This occurs when the enthalpy change (ΔH) is negative (exothermic reaction) and the entropy change (ΔS) is positive, particularly at all temperatures. Even if ΔH is positive, if ΔS is sufficiently large and positive, the reaction can still be spontaneous at high temperatures, as the term TΔS will outweigh ΔH.
How does the Gibbs free energy predict spontaneity?
It tells if the reaction will process spontaneously or not
How do enthalpy and entropy affect the spontaneity of a reaction?
Enthalpy and entropy are key factors in determining the spontaneity of a reaction, as described by Gibbs free energy (ΔG = ΔH - TΔS). A reaction is spontaneous when ΔG is negative, which can occur if the enthalpy change (ΔH) is negative (exothermic) or if the entropy change (ΔS) is positive (increased disorder). High temperatures can also enhance the effect of entropy, making reactions with positive ΔS more likely to be spontaneous. Thus, both ΔH and ΔS contribute to the overall favorability of a reaction.
What conditions will a low temperature male a reaction spontaneous?
A reaction will be spontaneous at low temperatures if the decrease in enthalpy (change in heat content) of the reaction is greater than the decrease in entropy (measure of disorder) multiplied by the temperature. This can be represented by the equation ΔG = ΔH - TΔS, where ΔG is the change in Gibbs free energy, ΔH is the change in enthalpy, T is the temperature in Kelvin, and ΔS is the change in entropy.
Under what conditions will a low temperature make a reaction spontaneous apex?
A low temperature can make a reaction spontaneous when it is exothermic, meaning it releases heat, and has a negative change in enthalpy (ΔH < 0). Additionally, if the reaction has a positive change in entropy (ΔS > 0), the Gibbs free energy change (ΔG = ΔH - TΔS) will be negative at low temperatures, favoring spontaneity. Conversely, if the reaction is endothermic (ΔH > 0) and has a negative entropy change (ΔS < 0), it will not be spontaneous at low temperatures.
What can be said about the reaction at 500K?
At 500K, the reaction rate will increase as temperature rises, following the Arrhenius equation. This increase in temperature will also influence the equilibrium position of the reaction if it is a reversible reaction. Higher temperatures can sometimes shift the equilibrium towards the products or reactants, depending on the enthalpy change.
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.
