True, a large positive value of entropy tends to favor products of a chemical reaction. However, entropy can be offset by enthalpy; a large positive value of enthalpy tends to favor the reactants of a chemical reaction. The true measure to determine which side of a chemical reaction is favored is the change in Gibbs' free energy, which accounts for both entropy and enthalpy, as calculated by: Change in Gibbs = Change in Enthalpy - Temp in Kelvin * Change in Entropy A negative value of Gibbs free energy will always favour the products of a chemical reaction.
A combustion reaction typically results in an increase in entropy due to the increase in the number of gaseous molecules formed during the reaction, leading to more disorder in the system. Therefore, combustion generally has a positive entropy change.
To calculate the standard entropy change (ΔS°) for a reaction, you need to use the formula: [ \Delta S° = \sum S°{\text{products}} - \sum S°{\text{reactants}} ] You would sum the standard entropy values of the products and subtract the sum of the standard entropy values of the reactants. If you provide the specific reaction and the standard entropy values, I can calculate it for you.
Exothermic reaction Decrease in entropy Increase in entropy Positive change in free energy Negative change in free energy
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.
The spontaneity of a reaction is closely linked to changes in entropy, which is a measure of disorder or randomness in a system. Generally, spontaneous reactions tend to increase the overall entropy of the universe, meaning that the total entropy of the system and its surroundings increases. According to the second law of thermodynamics, a reaction is spontaneous if the change in the Gibbs free energy is negative, which often occurs when the entropy of the products is greater than that of the reactants. Thus, a reaction that leads to greater disorder is more likely to be spontaneous.
The entropy change in a reaction can be calculated by comparing the entropy of the products to the entropy of the reactants. Without specific entropy values provided, it is difficult to determine the exact change. However, in general, the entropy change is positive in reactions where the products have higher entropy than the reactants, indicating an increase in disorder.
The entropy INCREASES. There are more moles in the products than in the reactants.
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
If the ∆H is positive and the ∆S is positive, then the reaction is entropy driven. If the ∆H is negative and the ∆S is negative, then the reaction is enthalpy driven. If ∆H is positive and ∆S is negative, then the reaction is driven by neither of these. If ∆H is negative and ∆S is positive, then the reaction is driven by both of these.
For a spontaneous reaction, the change in entropy (delta S) is typically positive.
delta s (change in entropy) is positive when.... -you go from a solid to a liquid -you go from a liquid to a gas -when you go from a solid to a gas -when there are more mols of products than mols of reactant the change in entropy is negative when the reverse of the above happens
A combustion reaction typically results in an increase in entropy due to the increase in the number of gaseous molecules formed during the reaction, leading to more disorder in the system. Therefore, combustion generally has a positive entropy change.
The factors that determine whether a chemical reaction will proceed in an energetically favorable or unfavorable direction include the difference in energy between the reactants and products (enthalpy change), as well as the entropy change and temperature of the system. If the overall change in energy is negative (exothermic) and the increase in disorder (entropy) is positive, the reaction is likely to proceed in a favorable direction.
A chemical reaction is spontaneous if it releases energy in the form of heat or light, or if it increases the disorder (entropy) of the system. This can happen when the products of the reaction are more stable or have lower energy than the reactants. The key factor is whether the reaction can proceed with a net decrease in free energy.
Negative entropy is a process or chemical reaction proceeds spontaneously in the forward direction.Positive entropy is a process proceeds spontaneously in reverse.
if there is an increase in the number of gas molecules , then ^S > 0
Several factors contribute to making a chemical reaction energetically favorable, including the difference in energy between reactants and products, the stability of the products formed, and the presence of catalysts that lower the activation energy required for the reaction to occur. Additionally, the entropy change of the system and the temperature at which the reaction takes place can also influence the favorability of a chemical reaction.