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Posted by on Sunday, April 8, 2012 at 4:50pm.

At 55C, the K for the reaction: 2NO2(g) <--> N2O4 is 1.15

a) write the equilibrium expression

b) calculate the concentration of N2O4(g) present in equilibrium with 0.50 mole of NO2

Please help and explain

  • Chemistry - , Sunday, April 8, 2012 at 4:59pm

    Don't you know Keq expression? products/reactants with coefficients as exponents.
    b. Substitute 0.40 mol for NO2 into Keq and solve for N2O4.

  • Chemistry - , Sunday, April 8, 2012 at 5:13pm

    Is this right?

    a) kc= [N2O4]/[NO2]^2

    =(1.15)/(2)^2
    =0.2875?

    B) I still can't figure it out :( please help

  • Chemistry - , Sunday, April 8, 2012 at 5:29pm

    Frankly I don't know how to answer the question. Is this Kc or is it Kp? The problem calls it Keq and gives moles. Moles can't go in the Keq expression. It must be molarity for Kc or partial pressure for Kp. With no volume given mols can't be converted to M nor to pressure. Is there more to the problem or did you post an edited version? The Kc expression you wrote is perfect.

  • Chemistry - , Sunday, April 8, 2012 at 5:31pm

    Okay thank you

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