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Which direction will the following reaction in a 5.0 L flask proceed if
Qp = 0.013?
2H2O(g) = 2H2(g) + O2(g)
Kp = 1.6 x 10-5
Choose one answer.

a. to the right because Q > Kp

b. to the left because Q > Kp

c. to the right because Q < Kp

d. to the left because Q < Kp

e. The reaction is at equilibrium.

  • Chem -

    Kp = (H2)^2(O2)/(H2O)^2 = 1.6 x 10^-5

    So if Q = 0.013, that is larger than K which means the numerator is too large and the denominator is too small. So the reaction will shift to make the numerator smaller and the denominator larger. Which way is that?

  • Chem -

    so it would be Q<K so it would shift from left to right

  • Chem -

    Absolutely not. The problem and my response CLEARLY says Q = 0.013. Is that larger or smaller than Kc which is 1.6 x 10^-5? It is larger than Kc. How can you possibly think Q<K? (The only way I can think of is that you have the < and > signs confused.) And look at my response again. It says the denominator is too small and the numerator is too large. So the reaction must shift to reverse those numbers; i.e., make the denominator larger and the numerator smaller. The ONLY way it can do that is to shift to the left.

  • Chem -

    My sign was backwards so I typed it in wrong....thanks

  • Chem -

    How can one find Q if it is not given with this same kind of problem

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