Thermodynamics govern reactions occur

AI Thread Summary
Thermodynamics plays a crucial role in determining whether chemical reactions occur, primarily through concepts like activation energy, entropy, and free energy. Activation energy is necessary to initiate reactions, while entropy influences the spontaneity of reactions. The relationship between free energy change (ΔG) and the equilibrium constant (K) is vital, as ΔG indicates the direction and extent of a reaction. A negative ΔG suggests a spontaneous reaction, while K provides insight into the ratio of products to reactants at equilibrium. Understanding these principles is essential for grasping the thermodynamic factors that govern chemical reactions.
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Homework Statement


What concepts from Thermodynamics govern whether reactions occur or not?


Homework Equations





The Attempt at a Solution



Activation energy-need some source of energy to start it-like pressure or light.
Entropy-but why?

Anything else, I'm sure there is more, but I don't understand it very well.
 
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Have you studied about how free energy relates the equilibrium constants of reactions?
 
like the K constant?
 
Yes. How is the change in free energy during a reaction (ΔG) related to the equilibrium constant (K)? What does the equilibrium constant tell you about the reaction?
 
Thread 'Confusion regarding a chemical kinetics problem'

Thread 'Confusion regarding a chemical kinetics problem'

TL;DR Summary: cannot find out error in solution proposed. [![question with rate laws][1]][1] Now the rate law for the reaction (i.e reaction rate) can be written as: $$ R= k[N_2O_5] $$ my main question is, WHAT is this reaction equal to? what I mean here is, whether $$k[N_2O_5]= -d[N_2O_5]/dt$$ or is it $$k[N_2O_5]= -1/2 \frac{d}{dt} [N_2O_5] $$ ? The latter seems to be more apt, as the reaction rate must be -1/2 (disappearance rate of N2O5), which adheres to the stoichiometry of the...
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