Hi guys I am a student of AP Chemistry. I am trying to understand the effect of temperature on equilibrium. I know that under the change of temperature, the equilibrium will shift to favor the endothermic process if heat is added and vice versa. But employing the Arrhenius Equation, I see a necessary concentration.(adsbygoogle = window.adsbygoogle || []).push({});

[tex]

Suppose that `⇌`(A, B);

print(`output redirected...`); # input placeholder

A ⇌ B

According to the definition of rate laws,

Rate*forward = k[A][A];

and

Rate*reverse = k;

where

k; is the rate constant

[X]; is the respective concentration of substance X.

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Also, according to the Arrhenius Equation, for any reaction,

k = A*exp(-E[a]/RT);where

A; is a constant

E[a]; is the activation energy

R is the gas constant

T is the temperature at which the reaction

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According to the definition of the equilibrium constant,

K[c] = k[A]/kand k[A]/k= A[1]*exp(-E[a1]/RT)/(A[2]*exp(-E[a2]/RT)) and A[1]*exp(-E[a1]/RT)/(A[2]*exp(-E[a2]/RT)) = A[1]*exp(E[a2]-E[a1])/A[2];

Therefore the K[c]; does not depend on T, which contradicts with Le Chatelier's Principle!

How can I resolve this paradox, or what is the fault with my logic?

[/tex]

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# Effect of Temperature on Chemical Equilibrium

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