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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.
Under what conditions will a low temperature make a reaction spontaneous apex?
A low temperature can make a reaction spontaneous when it is exothermic, meaning it releases heat, and has a negative change in enthalpy (ΔH < 0). Additionally, if the reaction has a positive change in entropy (ΔS > 0), the Gibbs free energy change (ΔG = ΔH - TΔS) will be negative at low temperatures, favoring spontaneity. Conversely, if the reaction is endothermic (ΔH > 0) and has a negative entropy change (ΔS < 0), it will not be spontaneous at low temperatures.
What is the sign of ΔT in an endothermic reaction?
ΔH is the enthalpy of the reaction and will be positive in an endothermic reaction and negative in an exothermic reaction.ΔT designates a change in temperature. T2-T1 = ΔTOften the change in temperature will be negative for an endothermic reaction.
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.
Will this entropy change by positive or negative?
If the system becomes more disordered, the entropy change will be positive. If the system becomes more ordered, the entropy change will be negative.
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.
How does an endothermic reaction change the entropy of the surroundings?
An endothermic reaction which absorbs heat from the surroundings decreases the entropy of the surroundings. This is because the surroundings lose thermal energy during the reaction, leading to a decrease in the disorder or randomness of the surroundings.
What can be said about an exothermic reaction with a negative entropy change?
An exothermic reaction with a negative entropy change indicates that the reaction releases heat to its surroundings and results in a decrease in disorder or randomness of the system.
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.
Under what conditions will a low temperature make a reaction spontaneous apex?
A low temperature can make a reaction spontaneous when it is exothermic, meaning it releases heat, and has a negative change in enthalpy (ΔH < 0). Additionally, if the reaction has a positive change in entropy (ΔS > 0), the Gibbs free energy change (ΔG = ΔH - TΔS) will be negative at low temperatures, favoring spontaneity. Conversely, if the reaction is endothermic (ΔH > 0) and has a negative entropy change (ΔS < 0), it will not be spontaneous at low temperatures.
What is the sign of ΔT in an endothermic reaction?
ΔH is the enthalpy of the reaction and will be positive in an endothermic reaction and negative in an exothermic reaction.ΔT designates a change in temperature. T2-T1 = ΔTOften the change in temperature will be negative for an endothermic reaction.
When a chemical reaction has a negative delta G is the reaction exothermic or endothermic?
When a chemical reaction has a negative delta G, the reaction is exothermic because delta G is the change in energy of a system and the change in its entropy. If the effect of a reaction is to reduce G, the process will be spontaneous so delta G is negative. Hope this helps :)
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.
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.
What does the entropy of a reaction describe?
The amount of randomness in the system
What could make G become negative at a given enthalpy and entropy?
Changing the temperature
What describes the entropy change of gas reaction?
if there is an increase in the number of gas molecules , then ^S > 0
