1. A reaction was shown to follow second-order kinetics. How much time is required for [A] to change from 0.500 M to 0.160 M? (k = 0.456 M⁻¹ s⁻¹)
2. A substance decomposes with a rate constant of 9.05 × 10⁻⁴ s⁻¹. How long does it take for 16.0% of the substance to decompose?
3. How long will it take for the concentration of A to decrease from 0.500 M to 0.100 M in the first-order reaction A → B? (k = 0.800 s⁻¹)
1)
we have:
[A]o = 0.5 M
[A] = 0.16 M
k = 0.456 M-1.s-1
use integrated rate law for 2nd order reaction
1/[A] = 1/[A]o + k*t
1/(0.16) = 1/(0.5) + 0.456*t
6.25 = 2 +0.456*t
0.456*t = 4.25
t = 9.32 s
Answer: 9.32 s
Only 1 question at a time please
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