So this is the problem:
Write expressions for K for the following reactions:
a. P4 (s) + 5O2 (g) <----> P4O10 (s)
The equation for an equilibrium expression is K = [C]^c[D]^d
................................................................[A]^a[b]^b
Using this formula, I thought the answer would have been [P4O10]
.............................................................................[P4][O2]^5
The back of the book says 1/[O2]^5
Anyone willing to explain to me why that is? I thought about if maybe they'd cancel, but that'd leave O10/[O2]^5
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Write expressions for K for the following reactions:
a. P4 (s) + 5O2 (g) <----> P4O10 (s)
The equation for an equilibrium expression is K = [C]^c[D]^d
................................................................[A]^a[b]^b
Using this formula, I thought the answer would have been [P4O10]
.............................................................................[P4][O2]^5
The back of the book says 1/[O2]^5
Anyone willing to explain to me why that is? I thought about if maybe they'd cancel, but that'd leave O10/[O2]^5
=\
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