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Endothermic reactions require an input of energy to proceed, which means they do not occur spontaneously. Spontaneous reactions release energy to their surroundings, unlike endothermic reactions that absorb energy from the surroundings. Therefore, endothermic reactions cannot be spontaneous as they need an external energy source to drive the reaction forward.
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Is spontaneous reaction exo or endo?
A spontaneous reaction could be either exothermic (exo) or endothermic (endo), depending on the specific reaction. Exothermic reactions release energy (usually as heat) to the surroundings, while endothermic reactions absorb energy from the surroundings. The spontaneity of a reaction is determined by the overall change in Gibbs free energy (ΔG), not by whether the reaction is exo or endo.
Are endothermic reactions always nonspontaneous?
No, many exothermic reactions need the heat of activation to start the reaction. Paper, for instance, does not spontaneously burst into flame... you need to raise its temperature to the kindling point for it to burn.
Reactions that release heat as bonds are broken are called .?
exothermic
What is the difference between Endothermic and Exothermic in five to ten points?
Endothermic reactions absorb heat from the surroundings, causing a decrease in temperature, while exothermic reactions release heat into the surroundings, causing a temperature increase. Endothermic reactions require an external heat source to proceed, while exothermic reactions release enough heat to sustain themselves. Endothermic reactions have a positive change in enthalpy (∆H), indicating absorption of energy, while exothermic reactions have a negative ∆H, indicating energy release. Endothermic reactions are typically non-spontaneous at low temperatures, requiring energy input to occur, while exothermic reactions are often spontaneous as they release energy. Examples of endothermic reactions include photosynthesis and ice melting, while examples of exothermic reactions include combustion and neutralization reactions.
Difference between endothermic and endergonic?
Endothermic refers to a reaction that absorbs heat from the surroundings, while endergonic refers to a reaction that requires an input of energy in order to proceed. Endothermic reactions specifically relate to heat transfer, while endergonic reactions encompass various forms of energy input beyond just heat.
Is spontaneous reaction exo or endo?
A spontaneous reaction could be either exothermic (exo) or endothermic (endo), depending on the specific reaction. Exothermic reactions release energy (usually as heat) to the surroundings, while endothermic reactions absorb energy from the surroundings. The spontaneity of a reaction is determined by the overall change in Gibbs free energy (ΔG), not by whether the reaction is exo or endo.
Are endothermic reactions always nonspontaneous?
No, many exothermic reactions need the heat of activation to start the reaction. Paper, for instance, does not spontaneously burst into flame... you need to raise its temperature to the kindling point for it to burn.
How can an endothermic reaction be spontaneous at room temperature?
An endothermic reaction can be spontaneous at room temperature if the increase in entropy of the system is large enough to overcome the energy input required for the reaction. This can happen if the products of the reaction have higher entropy than the reactants. As a result, the overall change in free energy can be negative even though the reaction is endothermic.
What are some examples of endothermic reactions that are endothermic as well?
All ENDOthermic reactions are of course ENDOthermic by themselves, aren't they?
On what conditions does a spontaneous reaction become spontaneous?
A spontaneous reaction occurs when the change in Gibbs free energy (ΔG) is negative, indicating that the reaction proceeds without the need for external energy input. This can happen when the entropy (ΔS) of the system increases and/or the enthalpy (ΔH) decreases, resulting in a negative ΔG value.
Reactions that release heat as bonds are broken are called .?
exothermic
Which reactions requires or stores energy?
Endothermic reactions require energy while exothermic reactions release energy.
What is the difference between Endothermic and Exothermic in five to ten points?
Endothermic reactions absorb heat from the surroundings, causing a decrease in temperature, while exothermic reactions release heat into the surroundings, causing a temperature increase. Endothermic reactions require an external heat source to proceed, while exothermic reactions release enough heat to sustain themselves. Endothermic reactions have a positive change in enthalpy (∆H), indicating absorption of energy, while exothermic reactions have a negative ∆H, indicating energy release. Endothermic reactions are typically non-spontaneous at low temperatures, requiring energy input to occur, while exothermic reactions are often spontaneous as they release energy. Examples of endothermic reactions include photosynthesis and ice melting, while examples of exothermic reactions include combustion and neutralization reactions.
Difference between endothermic and endergonic?
Endothermic refers to a reaction that absorbs heat from the surroundings, while endergonic refers to a reaction that requires an input of energy in order to proceed. Endothermic reactions specifically relate to heat transfer, while endergonic reactions encompass various forms of energy input beyond just heat.
Is combustion exothermic or endothermic?
exothermic reactions are the reactions which give out heat and endothermic reactions are the reaction which absorb heat.so combustion is an exothermic reaction.
What is the opposite of exothermic?
The opposite of exothermic is endothermic. Exothermic reactions are those which give off energy in the form of heat. Endothermic reactions require energy.
Does all irreversible reactions are spontaneous?
No, all irreversible reactions are not necessarily spontaneous. Irreversible reactions can be either spontaneous or non-spontaneous, depending on the change in Gibbs free energy (∆G) for the reaction. Spontaneous reactions have a negative ∆G, while non-spontaneous reactions have a positive ∆G.
