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April 3rd, 2018, 08:37 AM   #1
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why Keq depends on how we write the equation?

For the rxn

N2(g) +3H2(g) ⇌ 2NH3(g)

Keq1 = ( [NH3]^2 ) / ( [N2] * [H2]^3 )

But for the same rxn, in different form

0.5N2(g) +1.5H2(g) ⇌ NH3(g)

Keq2 = ( [NH3] ) / ( [N2]^0.5 * [H2]^1.5 )

Here Keq1 ≠ Keq2

But practically Keq should only depend on Temperature, so why is it affected on changing stoichiometric coefficients?
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April 6th, 2018, 11:38 AM   #2
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Quote:
Originally Posted by ThreXys View Post
For the rxn

N2(g) +3H2(g) ⇌ 2NH3(g)

Keq1 = ( [NH3]^2 ) / ( [N2] * [H2]^3 )

But for the same rxn, in different form

0.5N2(g) +1.5H2(g) ⇌ NH3(g)

Keq2 = ( [NH3] ) / ( [N2]^0.5 * [H2]^1.5 )

Here Keq1 ≠ Keq2

But practically Keq should only depend on Temperature, so why is it affected on changing stoichiometric coefficients?
A word of advise. It is better trying not to use fractions or non-integer numbers as stoichiometric coefficients as it will render weird results or misinterpretations of what you're trying to prove. Maybe you want to check this link.

As it was mentioned in that discussion what in ordinary arithmetic can be held true in practical terms does not. Equilibrium constants depend on the rate of reaction which is determined experimentally and this is the result from its mechanism therefore we cannot imply so easily that a fraction of whatever you're trying to use will held true.
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