Lena772
  • Lena772
How to calculate Kc if not given temperature?
Chemistry
  • Stacey Warren - Expert brainly.com
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SOLVED
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chestercat
  • chestercat
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Lena772
  • Lena772
\[K _{c}=\frac{ K _{p}}{(RT)^{\Delta \eta}}\]
Cuanchi
  • Cuanchi
what information do you have? do you have the partial pressures of all the components at the equilibrium or the total pressure and the molar rates?
Cuanchi
  • Cuanchi
do you have the reaction or they said is a STP condition?

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Cuanchi
  • Cuanchi
the delt n is =0?
Lena772
  • Lena772
Calculate the Kc of the reaction below assuming all reactant and product concentrations are 2.00 M at equilibrium. Ag+ (aq) + Cl- (aq) ⇌ AgCl (s) I think delta N is 0, that's what I got
Cuanchi
  • Cuanchi
you dont have any gas
Lena772
  • Lena772
no @cuanchi
aaronq
  • aaronq
you dont need that equation. you have to do this.. For a general chemical equation: \(\sf aA+bB\rightleftharpoons cC\) The equilibrium expression is: \(\sf K_c=\dfrac{[Products]}{[Reactants]}=\dfrac{[C]^c}{[A]^a[B]^b}\) Where the brackets (\(\sf [ ~]\)) mean concentration (Molarity).
Jhannybean
  • Jhannybean
Woot. using that `/sf` @aaronq :)
Photon336
  • Photon336
I think another important fact is that the reaction has already reached equilibrium so I think you can just plug in all the values moles for both reactants and products they give you once you set up Kc as @aaronq said.
Lena772
  • Lena772
Concentration of (s) = 1 so, 1/(((2)^1)(2)^1))= 1/4 = 0.25 ?
Lena772
  • Lena772
@Photon336 @aaronq
Lena772
  • Lena772
@mathmate
mathmate
  • mathmate
If the question is about temperature, then I would calculate according to the standard formula (or see @arronq 's post) and state that Kc applies to the temperature at which the experiment was performed.

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