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The equation for ∆G is ∆G = ∆H - T∆S H is enthalpy and S is entropy
So, ∆G is negative if T∆S is greater than ∆H
What else can I help you with?
What could make delta G become negative at a given enthalpy and entropy?
For delta G to become negative at a given enthalpy and entropy, the process must be spontaneous. This can happen when the increase in entropy is large enough to overcome the positive enthalpy, leading to a negative overall Gibbs free energy. This typically occurs at higher temperatures where entropy effects dominate.
What conditions make delta G always positive?
G is always positive when enthalpy increases and entropy decreases.
Is Delta S is the change in enthalpy a measure of randomness?
No, ΔS (change in entropy) and ΔH (change in enthalpy) are not measurements of randomness. Entropy is a measure of the disorder or randomness in a system, while enthalpy is a measure of the heat energy of a system. The change in entropy and enthalpy can be related in chemical reactions to determine the overall spontaneity of the process.
Can delta s be negative Entropy?
yes
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.
Explain the combined effects of entropy and enthalpy during the melting of ice?
During the melting of ice, entropy and enthalpy work together. The increase in entropy (disorder) as solid ice turns into liquid water disrupts the ordered crystal lattice structure. This process requires an input of energy (enthalpy) to break these intermolecular forces holding the ice together.
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 is S in the equation delta G equals delta H minus TdeltaS?
The change in enthalpy between products and reactants in a reaction
What is delta S in the equation Delta G Delta H - Temperature Delta S?
In the equation ΔG = ΔH - TΔS, ΔS represents the change in entropy of a system. Entropy is a measure of the disorder or randomness in a system, and a positive ΔS indicates an increase in disorder. The equation relates the change in free energy (ΔG) to changes in enthalpy (ΔH) and entropy (ΔS) at a given temperature (T), helping to determine the spontaneity of a process. A negative ΔG suggests that a reaction is spontaneous, which can be influenced by the values of ΔH and ΔS.
What is delta S in the equation DeltaGDeltaH-Tdelta S?
Delta S in this equation represents the change in entropy of a system. It is a measure of the system's disorder or randomness, with a positive value indicating an increase in disorder and a negative value indicating a decrease in disorder. The equation you provided, ΔG = ΔH - TΔS, relates the change in Gibbs free energy to the enthalpy change, temperature, and entropy change of a system.
What is delta S in the equation delta G delta H-T delta S?
Delta S represents the change in entropy of a system. In the equation delta G = delta H - T delta S, it is used to determine the contribution of entropy to the overall change in Gibbs free energy. A negative delta S value suggests a decrease in the disorder of a system.
What is melting equation?
The melting equation describes the phase transition of a substance from solid to liquid as it absorbs heat. It typically involves the relationship between temperature and pressure, often represented in the context of the Gibbs free energy, where the change in enthalpy equals the product of temperature and change in entropy. The equation can be expressed as ( \Delta G = \Delta H - T\Delta S ), where ( \Delta G ) is the change in Gibbs free energy, ( \Delta H ) is the change in enthalpy, and ( \Delta S ) is the change in entropy. At the melting point, the Gibbs free energy change is zero, indicating equilibrium between the solid and liquid phases.
