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.

----------------------------------------------------------------------------------------

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

------------------------------------------------------------------------------------

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]

**Physics Forums | Science Articles, Homework Help, Discussion**

Join Physics Forums Today!

The friendliest, high quality science and math community on the planet! Everyone who loves science is here!

The friendliest, high quality science and math community on the planet! Everyone who loves science is here!

# Effect of Temperature on Chemical Equilibrium

**Physics Forums | Science Articles, Homework Help, Discussion**