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Delta G (Gibbs free energy change) for a reaction is always positive when the reaction is non-spontaneous under the given conditions. This typically occurs when the system is at equilibrium or when the enthalpy change (ΔH) is positive and the entropy change (ΔS) is negative, leading to a situation where the temperature multiplied by ΔS (TΔS) is not sufficient to drive the reaction forward. Additionally, when the reactants are more stable than the products, or when the reaction requires external energy input to proceed, delta G will also be positive.
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When Under what conditions is G for a reaction always positive apex?
The Gibbs free energy change (ΔG) for a reaction is always positive when the reaction is non-spontaneous under the given conditions. This typically occurs at high temperatures for exothermic reactions (where ΔH is negative and ΔS is positive) or when the entropy change (ΔS) is negative while ΔH is positive. In such cases, the term TΔS is not large enough to overcome the positive ΔH, resulting in a positive ΔG.
Is G for a reaction always positive?
No, the Gibbs free energy change (ΔG) for a reaction is not always positive. A negative ΔG indicates that a reaction is spontaneous and can proceed in the forward direction, while a positive ΔG means the reaction is non-spontaneous under standard conditions. When ΔG is zero, the system is at equilibrium, and no net change occurs. Thus, ΔG can be positive, negative, or zero, depending on the reaction conditions.
Under what conditions is G for a reaction always positive-apex?
The Gibbs free energy change (ΔG) for a reaction is always positive when the reaction is non-spontaneous under the given conditions. This typically occurs at high temperatures for endothermic reactions (where ΔH is positive and ΔS is negative), or when both ΔH is positive and the entropy change (ΔS) is negative. In these cases, the term TΔS is either small or negative, resulting in ΔG being greater than zero.
Under what condition would pressure affect the reaction rate?
If the reaction occurs in the gas phase
What does a positive value of delta G mean for a reaction?
A positive value of delta G (ΔG) indicates that a reaction is non-spontaneous under standard conditions, meaning it requires an input of energy to proceed. In this case, the products have higher free energy than the reactants, suggesting that the reaction is unfavorable in its current direction. Therefore, the reaction is more likely to occur when coupled with a spontaneous process or under different conditions that favor the formation of products.
When Under what conditions is G for a reaction always positive apex?
The Gibbs free energy change (ΔG) for a reaction is always positive when the reaction is non-spontaneous under the given conditions. This typically occurs at high temperatures for exothermic reactions (where ΔH is negative and ΔS is positive) or when the entropy change (ΔS) is negative while ΔH is positive. In such cases, the term TΔS is not large enough to overcome the positive ΔH, resulting in a positive ΔG.
Under what conditions is G for a reaction always positive?
When H is positive and S is negative
Is G for a reaction always positive?
No, the Gibbs free energy change (ΔG) for a reaction is not always positive. A negative ΔG indicates that a reaction is spontaneous and can proceed in the forward direction, while a positive ΔG means the reaction is non-spontaneous under standard conditions. When ΔG is zero, the system is at equilibrium, and no net change occurs. Thus, ΔG can be positive, negative, or zero, depending on the reaction conditions.
Under what conditions is G for a reaction always positive-apex?
The Gibbs free energy change (ΔG) for a reaction is always positive when the reaction is non-spontaneous under the given conditions. This typically occurs at high temperatures for endothermic reactions (where ΔH is positive and ΔS is negative), or when both ΔH is positive and the entropy change (ΔS) is negative. In these cases, the term TΔS is either small or negative, resulting in ΔG being greater than zero.
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.
Under what condition would pressure affect the reaction rate?
If the reaction occurs in the gas phase
Give example of closure property?
Add two positive integers and you ALWAYS have a positive integers. The positive integers are closed under addition.
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.
What is the generalization that always works in the same way under the same condition is what?
Law
Is a half-cell's standard reduction potential positive?
Yes, a half-cell's standard reduction potential is positive if the reduction reaction is spontaneous under standard conditions.
What does a positive value of delta G mean for a reaction?
A positive value of delta G (ΔG) indicates that a reaction is non-spontaneous under standard conditions, meaning it requires an input of energy to proceed. In this case, the products have higher free energy than the reactants, suggesting that the reaction is unfavorable in its current direction. Therefore, the reaction is more likely to occur when coupled with a spontaneous process or under different conditions that favor the formation of products.
What is the answer to a positive number mines a negative number if the number on the left side is positive and its bigger?
I don't know but I think it is always 0 or under
