Consider two reaction vessels, one containing A and the other containing B. At t = 0, [A]0 = [B]0. A and B decompose by first order kinetics with rate constants of
kA = 4.50 × 10-4 s-1 and kB = 3.70 × 10-3 s-1, respectively. Calculate the time that must pass to reach the condition such that [A] = (7.18)[B]
Ap Chemistry?
2020-04-12 1:41 pm
回答 (1)
2020-04-12 3:10 pm
✔ 最佳答案
Let [A]ₒ = [B]ₒ = cIntegrated rate equation for first-order reaction:
ln[A] = -kA t + ln(c) …… [1]
ln[B] = -kB t + ln(c) …… [2]
[1] - [2]:
ln[A] - ln[B] = (-kA t) - (-kB t)
ln([A]/[B]) = (kB - kA) t
When [A] = 7.18[B]:
ln(7.18) = [(3.70 × 10⁻³) - (4.50 × 10⁻⁴)] t
ln(7.18) = (3.25 × 10⁻³) t
t = ln(7.18) / (3.25 × 10⁻³) s
Time taken, t = 607 s = 10 min 10 s
收錄日期: 2021-04-18 18:25:56
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