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    I'm trying to do my homework and i've tried every logical way I can think of for this question, can anyone help?

    The equilibrium constant for A --> B is 39 when at 100 degrees C. If you had 2.00 moles of A at the start, how much would be left at equilibrium at this temperature?

    Thanks for any help, much appreciated!
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    (Original post by thegaypixie)
    I'm trying to do my homework and i've tried every logical way I can think of for this question, can anyone help?

    The equilibrium constant for A --> B is 39 when at 100 degrees C. If you had 2.00 moles of A at the start, how much would be left at equilibrium at this temperature?

    Thanks for any help, much appreciated!
    let moles of A reacted at equilibrium equal x ...
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    (Original post by charco)
    let moles of A reacted at equilibrium equal x ...
    Thanks
    Could you help me on the last question as well?
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    (Original post by thegaypixie)
    Thanks
    Could you help me on the last question as well?
    Which last question? There was only one!
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    (Original post by charco)
    let moles of A reacted at equilibrium equal x ...
    isnt kc calculated using concentration values tho
    like how do we work that out if kc = conc products / conc reactants
    we only have mol here?
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    (Original post by medhelp)
    isnt kc calculated using concentration values tho
    like how do we work that out if kc = conc products / conc reactants
    we only have mol here?
    For this question, the volume "does not matter" as the sum of the Stoichiometric coefficients are the same on both sides of the equation.

    Let the volume be an unknown 'V' when we write out the respective concentrations, the 'V's will cancel each other out when substituted into the Kc expression.
 
 
 
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