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What is the relationship between the enthalpy (H) and entropy (S) of a reaction that is never spontaneous?
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What is the relationship between enthalpy of atomisation of hydrogen and the bond dissociation enthalpy of the H-H bond?
the enthalpy of atomisation of hydrogen is equal and (in principle) identical to the bond dissociation enthalpy of the H-H bond. However, IF the first is measured by calorimetry and the second by spectrometry there might be a systematic difference.
Where was the energy that is released in an endothermic reaction originally stored?
Energy is released during an exothermic reaction. The energy released was enthalpy. This includes quantities such as the attraction between molecules, the lattice energy, the chemical bonds... depends on the reaction.An endothermic reaction absorbs energy in the enthalpy of solution. It comes from the surroundings.
What is delta h in the equation delta g delta h - t delta?
The change in enthalpy between products and reactants in a reaction
What forms a spontaneous redox reaction between two elements?
The element with the greater reduction potential is the one that is reduced.
What is relation between hydration energy lattice energy and enthalpy of solution?
enthalpy change of solution=enthalpy change of hydration - enthalpy change of lattice
What is the relationship between the enthalpy h and entropy s of a reaction that is spontaneous at higher temperatures but not at lower temperatures?
-H, +S
How is enthalpy related to spontaneity of a reaction?
S > 0 contributes to spontaneity.
How is the enthalpy of reaction related to the enthalpies of formation for the products and reactants?
The difference between the enthalpy of formation of the products minus the enthalpy of formation of the reactants is the enthalpy of the reaction
What is the difference between enthalpy change and enthalpy change per mole?
Enthalpy is the energy absorbed or lost from a reaction, but enthalpy change per mole is the amount of energy lost per mole, so in order to get the overall enthalpy from the change per mole, you must multiply that value by the amount of moles used in the reaction.
What is the relationship between the universe and spontaneous generation?
There is no relation.
What is an exergonic reaction?
Exergonic reactions indicate a negative change in Gibbs free energy, which in English means that the reactions are spontaneous and do not require addition of energy. The exchange of oxygen and carbon dioxide in blood and lungs is an example. It is the concentration gradient that runs these exchanges passively, without additional energy from the cells.
What does the different in potential energy between the reactant and products represent?
It represents the change in enthalpy for the reaction.
What is H in the equation G H TS?
The change in entropy between products and reactants in a reaction
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 term refers to the difference between the energy of the transition state and the energy of the reactants?
The different in energy between the products and reactant is known as enthalpy of the reaction, or ∆Hreaction.
What is the relationship between enthalpy of atomisation of hydrogen and the bond dissociation enthalpy of the H-H bond?
the enthalpy of atomisation of hydrogen is equal and (in principle) identical to the bond dissociation enthalpy of the H-H bond. However, IF the first is measured by calorimetry and the second by spectrometry there might be a systematic difference.
Where was the energy that is released in an endothermic reaction originally stored?
Energy is released during an exothermic reaction. The energy released was enthalpy. This includes quantities such as the attraction between molecules, the lattice energy, the chemical bonds... depends on the reaction.An endothermic reaction absorbs energy in the enthalpy of solution. It comes from the surroundings.
