?The equilibrium constant for the dissociation of molecular iodine, \(\mathrm{I}_{2}(g) \rightleftharpoons 2 \mathrm{I}(g)\), at 800 K is \(K_{c}=3.1 \
Chapter 15, Problem 15.14(choose chapter or problem)
The equilibrium constant for the dissociation of molecular iodine, \(\mathrm{I}_{2}(g) \rightleftharpoons 2 \mathrm{I}(g)\), at 800 K is \(K_{c}=3.1 \times 10^{-5}\).
(a) Which species predominates at equilibrium \(\mathrm{I}_{2}\) or I?
(b) Assuming both forward and reverse reactions are elementary processes, which reaction has the larger rate constant, the forward or the reverse reaction?
Text Transcription:
I_2(g) \rightleftharpoons 2 I(g)
K_c = 3.1 X 10-5
I_2
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