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Under what condition is delta G for a reaction always positive?
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.
What happens when delta h is positive?
When ΔH (the change in enthalpy) is positive, it means that the reaction is endothermic, absorbing heat from its surroundings. This indicates that energy is being consumed rather than released during the chemical reaction.
What determine whether a reaction took place?
Use the following equation: delta G = delta H - T*deltaS. A reaction is spontaneous if delta G is negative. A reaction will always be spontaneous (under any temperature) only if the change in enthalpy (delta H) is negative and the change in entropy (delta S) is positive. If this is not the case, the reaction will only be spontaneous (negative delta G) for a range of temperatures (or could be always non-spontaneous)
Can a reaction that is endothermic with a decrease in entropy never occur spontaneously?
An endothermic reaction with a decrease in entropy may still occur spontaneously under certain conditions, particularly at high temperatures. Spontaneity is determined by the Gibbs free energy change (( \Delta G )), which combines enthalpy and entropy changes (( \Delta G = \Delta H - T \Delta S )). If the negative contribution from ( T \Delta S ) (where ( \Delta S ) is negative) is outweighed by a sufficiently large positive ( \Delta H ), the reaction may not be spontaneous. However, at lower temperatures, the reverse can be true, and such a reaction could be spontaneous.
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.
Is the change in entropy, delta S, positive or negative for a spontaneous reaction?
For a spontaneous reaction, the change in entropy (delta S) is typically positive.
What does a positive delta H tell about reaction?
A positive delta H indicates that the reaction is endothermic, meaning it absorbs heat from the surroundings to proceed. This implies that the products have higher energy content compared to the reactants.
What is the difference between delta H and delta E in a chemical reaction?
Delta H represents the change in enthalpy, which is the heat energy exchanged during a chemical reaction. Delta E represents the change in internal energy, which includes both the heat energy and work done in a reaction. In simpler terms, delta H focuses on heat transfer, while delta E considers both heat and work.
Under what condition is delta G for a reaction always positive?
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.
What is the value of Delta E for the combustion of the fuel?
The value of ΔE for the combustion of a fuel is the change in internal energy of the reaction, typically measured in kilojoules per mole. It reflects the energy released or absorbed during the combustion process, with a negative value indicating energy release and a positive value indicating energy absorption.
A chemical reaction that has a positive ΔG is correctly described as?
This is a nonspontaneous reaction, which means that it is reactant-favored. According to the second law of thermodynamics, product-favored reactions must have a negative delta G.It can also be described as an endergonic reaction - that is a chemical reaction in which the standard change in free energy is positive, and energy is absorbed.
What does it mean by positive and negative delta S?
Means a increase or decrease in disorder in the reaction depending on the sign ( "-" or"+")
What is the significance of delta G in chemical reactions?
The significance of delta G in chemical reactions is that it indicates whether a reaction is spontaneous or non-spontaneous. A negative delta G value means the reaction is spontaneous and can proceed on its own, while a positive delta G value means the reaction is non-spontaneous and requires external energy input to occur.
What happens when delta h is positive?
When ΔH (the change in enthalpy) is positive, it means that the reaction is endothermic, absorbing heat from its surroundings. This indicates that energy is being consumed rather than released during the chemical reaction.
What is the Delta E chemistry formula used to calculate the change in energy of a chemical reaction?
The Delta E formula in chemistry is used to calculate the change in energy of a chemical reaction. It is represented as E E(final state) - E(initial state), where E is the change in energy, E(final state) is the energy of the system in its final state, and E(initial state) is the energy of the system in its initial state.
What is the significance of delta G prime in determining the spontaneity of a biochemical reaction?
The significance of delta G prime in determining the spontaneity of a biochemical reaction lies in its ability to indicate whether the reaction will proceed forward or backward. A negative delta G prime value indicates that the reaction is spontaneous and will proceed forward, while a positive value indicates that the reaction is non-spontaneous and will not proceed without external energy input.
What determine whether a reaction took place?
Use the following equation: delta G = delta H - T*deltaS. A reaction is spontaneous if delta G is negative. A reaction will always be spontaneous (under any temperature) only if the change in enthalpy (delta H) is negative and the change in entropy (delta S) is positive. If this is not the case, the reaction will only be spontaneous (negative delta G) for a range of temperatures (or could be always non-spontaneous)
