The rate constant for the reaction is 0.390 M−1⋅s−1
at 200 ∘C.
A⟶products
If the initial concentration of A is 0.00780 M, what will be the concentration after 905 s?
[A] = ? M
Chemistry Question? Kinetics?
2020-05-19 12:26 am
回答 (2)
2020-05-19 12:58 am
✔ 最佳答案
As the unit of the rate constant M⁻¹•S⁻¹, the reaction is second-order.Integrated rate equation for second order reaction:
1/[A] = kt + (1/[A]ₒ)
1/[A] = 0.390 × 905 + (1/0.00780) M⁻¹
1/[A] = 481.2 M⁻¹
Concentration after 905 s = 1/481.2 M = 0.00208 M
2020-05-19 12:52 am
This is a second order reaction because the units on the rate constant are M^-1 s^-1. The integrated rate law for a 2nd order reaction is:
1/[A] = kt + 1/[A]o
1/[A] = 0.390 M^-1 s^-1 (905 s) + 1/7.80X10^-3 M
1/[A] = 481.16 M^-1
[A] = 2.08X10^-3 M
1/[A] = kt + 1/[A]o
1/[A] = 0.390 M^-1 s^-1 (905 s) + 1/7.80X10^-3 M
1/[A] = 481.16 M^-1
[A] = 2.08X10^-3 M
收錄日期: 2021-04-18 18:31:32
原文連結 [永久失效]:
https://hk.answers.yahoo.com/question/index?qid=20200518162618AAz9zHn