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Lena772

  • one year ago

How to calculate Kc if not given temperature?

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  1. Lena772
    • one year ago
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    \[K _{c}=\frac{ K _{p}}{(RT)^{\Delta \eta}}\]

  2. cuanchi
    • one year ago
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    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?

  3. cuanchi
    • one year ago
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    do you have the reaction or they said is a STP condition?

  4. cuanchi
    • one year ago
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    the delt n is =0?

  5. Lena772
    • one year ago
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    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

  6. cuanchi
    • one year ago
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    you dont have any gas

  7. Lena772
    • one year ago
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    no @cuanchi

  8. aaronq
    • one year ago
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    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).

  9. Jhannybean
    • one year ago
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    Woot. using that `/sf` @aaronq :)

  10. Photon336
    • one year ago
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    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.

  11. Lena772
    • one year ago
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    Concentration of (s) = 1 so, 1/(((2)^1)(2)^1))= 1/4 = 0.25 ?

  12. Lena772
    • one year ago
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    @Photon336 @aaronq

  13. Lena772
    • one year ago
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    @mathmate

  14. mathmate
    • one year ago
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    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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