Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: magnus on February 07, 2019, 02:56:53 AM
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For this reaction Kc is 55.2, increasing the stoichiometric coefficients the value is always the same ...
H2 (g) + I2 (g) ⇄ 2 HI (g) risulta Kc=55.2 a 698 K.
2 H2 (g) +2 I2 (g) ⇄ 4 HI (g)
Kc= [HI]² / [H₂][I₂]
??? ??? ???
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No it would be Kc =[HI]4/([H2]2*[I2]2 )
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ok, but with the same concentration values, doubling the stechimetric values Kc will always be 55.2, it is a constant ...
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No, it would be 55.22.
[HI]4/[H2]2[I2]2 = ([HI]2/[H2][I2])2
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Ok
Thanks
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For this reaction Kc is 55.2, increasing the stoichiometric coefficients the value is always the same ...
H2 (g) + I2 (g) ⇄ 2 HI (g) risulta Kc=55.2 a 698 K.
2 H2 (g) +2 I2 (g) ⇄ 4 HI (g)
Kc= [HI]² / [H₂][I₂]
??? ??? ???
If you multiply an equilibrium reaction by a coefficient n then new K is n raised to power of previous K
Mathematics on K expression
Every textbook of chemistry has great explanation of it.
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I think you mean "new K is previous K raised to power of n"