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ashlynchristianson
20.03.2020 •
Chemistry
At a certain fixed temperature, the reaction A(g) + 2 B(g) → AB2(g) is found to be first order in the concentration of A and zero order in the concentration of B. The reaction rate constant is 0.0672 s−1 . If 2.000 moles of A and 4.000 moles of B are placed in a 1.000 liter container, how many seconds will elapse before the concentration of A has fallen to 0.300 mol/liter? 1. 36.6948 2. 60.226 3. 63.2373 4. 34.244 5. 49.9242 6. 23.8631 7. 51.2735 8. 29.6425 9. 36.1356 10. 28.231 Answer in units of s.
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Ответ:
28.231 seconds
Explanation:
Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.
Thus overall order = 1
Expression for rate law for first order kinetics is given by:
where,
k = rate constant =![0.0672s^{-1}](/tpl/images/0555/2030/ad02f.png)
t = time taken for decomposition
a = initial amount of the reactant A =![\frac{moles}{volume}=\frac{2.000}{1.000L}=2.000M](/tpl/images/0555/2030/253d1.png)
a - x = amount left after decay process = 0.300 M
28.231 seconds will elapse before the concentration of A has fallen to 0.300 mol/liter
Ответ: