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Posted by on Sunday, May 17, 2009 at 4:51pm.

Two moles of pure ammonia were injected into a 2.00L flask at a certain temperature. The equilibrium mixture:
2NH3(G)-->N2(G) + 3H2(G)
<--

A) What is the value of the equilibrium constant at this temperature?
b) how would the number of moles of ammonia be affected if the volume of the system was increased?
C) How would the value of the equilibrum constant be affected by this increase in volume?

  • Chemistry - , Sunday, May 17, 2009 at 4:56pm

    For a, to calculate it you have to have the concentrations at equilibrium. If you are supposed to look it up, you need the temp.
    for b, there are 2 volumes on the left, 4 on the right. So increasing volume tends a shift to the right.
    for c, The equibrium constant wont change.

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