the first-order reaction A products, the initial concentration of A is 1.56 M an
ID: 1087418 • Letter: T
Question
the first-order reaction A products, the initial concentration of A is 1.56 M and the concentration is 0.869 M after 48.0 min. What is the value of the rate constant, k, in min ? a. 3.84 x 10 b. 2.92 x 10 c. 5.68 x 102 d. 1.22 x 102 -12. The following time and concentration data was obtained for the reaction: 2A products time (min) IAL.M 1.1 2.3 4.0 1.20 1.00 0.80 0.60 Refer to the table above. If the reaction is known to be first-order, determine the rate constant for reaction. b. 0.37 c. 0.49 d. 0.60 13. Consider the reaction 2HI(g) H2(g) + 12(g) What is the value of the equilibrium constant, K equilibrium, [H2]s 6.50 x 10.7 M, [b]106 x iOs M, and [HI]s i 87 x iOsM? a. 3.68 x 107 d. 50.8 b. 1.97 x 102 c. 1.29 x 10-16Explanation / Answer
11)
we have:
[A]o = 1.56 M
[A] = 0.869 M
t = 48.0 min
use integrated rate law for 1st order reaction
ln[A] = ln[A]o - k*t
ln(0.869) = ln(1.56) - k*48
-0.1404 = 0.4447 - k*48
k*48 = 0.5851
k = 1.22*10^-2 min-1
Answer: d
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