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-   -   Equilibrium and enthalpy (https://www.askmehelpdesk.com/showthread.php?t=577567)

  • May 22, 2011, 06:03 AM
    SWalker92
    Equilibrium and enthalpy
    I have a few questions that I am stuck on and would really appreciate any help :)

    1) Kp = 85 at 460°C and Kp = 21 at 800°C for the following reaction:

    NO2(g) + SO2(g) <----> NO(g) + SO3(g)

    Which one of the following statements is true?

    a) △rH° > 0 and Kc < Kp
    b) △rH° < 0 and Kc > Kp
    c) △rH° = 0 and Kc = Kp
    d) △rH° < 0 and Kc = Kp
    e) △rH° > 0 and Kc = Kp

    The answer says D but I can't figure out why.



    2) Given the following thermochemical data, what is the enthalpy of formation △fH°298 for C6H6 (l) at 298K and 100kPa?

    C6H6 (l) + 3H2(g) --> C6H12 (l) △H° = -206 kJ mol-1
    6H2 (g) + 6C (s) --> C6H12 (l) △H° = -123 kJ mol-1


    3) Samples of A (2.0 mol) and B (3.0 mol) are placed in a 10.0 L container and the following reaction takes place:

    2A(g) <-----> 3B(g)

    At equilibrium, the concentration of A is 0.14 M. What is the value of Kc?

  • May 22, 2011, 06:05 AM
    SWalker92
    Sorry, the  symbol represents a triangle :)
  • May 24, 2011, 08:45 AM
    Unknown008

    1. The is directly related to the yield. You know that Kc is a measure of the yield, do you? When the yield is greater, the delta H is more negative, because the reactants lose energy to get to a lower energy level (you can see that very clearly in a Born Haber Cycle).

    Can you write down the Kc and Kp expressions? :)

    2. First, write down the equation for the formation of C6H6:



    You see that in the given equations, you can do this, by first passing through C6H12.



    You started with 3 more H2 molecules, and you end up with 3 more H2 molecules... which means that you can take the given delta H without worrying about the excess H2 molecules.

    3. If there are initially 2.0 mol of A and there is 0.14 mol of A left, how many mol of A got converted to B?

    2 mol of A gives 3 mol of B. If you have the number of moles of A above which became B, how many mol of B did you get?

    Using this now, use the equation for Kc.



    The volume is kept constant, at 10, so you can find the final concentrations of A and B. Then, work Kc out! :)

    Post what you get!

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