?At 800 K, the equilibrium constant for the reaction \(\mathrm{A}_{2}(g)
Chapter 15, Problem 15.99(choose chapter or problem)
At 800 K, the equilibrium constant for the reaction \(\mathrm{A}_{2}(g) \rightleftharpoons 2 \mathrm{~A}(\mathrm{~g})\) is \(K_{c}=3.1 \times 10^{-4}\).
(a) Assuming both forward and reverse reactions are elementary reactions, which rate constant do you expect to be larger, \(k_{f}\) or \(k_{r}\) ?
(b) If the value of \(k_{f}=0.27 \mathrm{~s}^{-1}\), what is the value of \(k_{r}\) at 800 K ?
(c) Based on the nature of the reaction, do you expect the forward reaction to be endothermic or exothermic?
(d) If the temperature is raised to 1000 K, will the reverse rate constant \(k_{r}\) increase or decrease? Will the change in \(k_{r}\) be larger or smaller than the change in \(k_{f}\) ?
Text Transcription:
A2(g) \rightleftharpoons 2 A(g)
Kc = 3.1 x 10-4.
k_f
k_r
k_f = 0.27 s-1
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