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For which of reaction listed below will gibbs free energy always be positive?
Guys watch out the question, if your question end with positive then the answer will be An endothermic reaction that decreases in entropy. If the question end with negative then its An exothermic reaction that increases in entropy--APEX hope this help
What is the difference between a reaction that happens spontaneously and a reaction that doesn't?
The difference can be clarified by entropy (the second rule of thermodynamics).The reaction is more spontaneous with higher entropy, for the reactions that occur spontaneously the entropy is higher than for the ones that do not.
What could make G become negative at a given enthalpy and entropy?
Changing the temperature
What can be said about a reaction with H 620 kJmol and S -0.46 kJ molK?
it can never be spontanious
Which statement describes a reaction at 298 K if H 31 kJ mol S 0.093 kJ molK?
It is not spontaneous.
For which of reaction listed below will gibbs free energy always be positive?
Guys watch out the question, if your question end with positive then the answer will be An endothermic reaction that decreases in entropy. If the question end with negative then its An exothermic reaction that increases in entropy--APEX hope this help
Is Entrophy change in a system that undergoes a spontaneous process positive negative or zero?
Negative entropy is a process or chemical reaction proceeds spontaneously in the forward direction.Positive entropy is a process proceeds spontaneously in reverse.
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.
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 is the difference between a reaction that happens spontaneously and a reaction that doesn't?
The difference can be clarified by entropy (the second rule of thermodynamics).The reaction is more spontaneous with higher entropy, for the reactions that occur spontaneously the entropy is higher than for the ones that do not.
What is the relationship between the enthalpy (H) and entropy (S) of a reaction that is never spontaneous?
A reaction that is never spontaneous has a positive Gibbs free energy change (ΔG > 0) under all conditions. This can occur when the enthalpy change (ΔH) is positive and the entropy change (ΔS) is negative, which leads to a situation where the term TΔS (temperature times the change in entropy) does not offset the positive ΔH. As a result, the overall Gibbs free energy remains positive, indicating that the reaction does not occur spontaneously.
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 do you determine whether a reaction is spontaneous or non spontaneous?
The first of two factors that determine whether a reaction is spontaneous or non-spontaneous is entropy. The second is energy. For a reaction to be spontaneous, it must have both of these factors.
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.
Is the Gibbs free energy negative in the spontaneous reaction?
Yes, as long as the entropy of the universe increases.
What value should the heat of the reaction have in a spontaneous reaction?
It can be + or - depending on the value of the entropy (∆S). Recall, that ∆G = ∆H - T∆S and for a spontaneous reaction, ∆G must be negative, so you can see how this will depend on the values and signs of both enthalpy and entropy.
What could make G become negative at a given enthalpy and entropy?
Changing the temperature
