The second-order decomposition of hi has a rate constant of 1.80 x 10−3 m−1 s−1. How much hi remains after 45.6 s if the initial
concentration of hi is 3.81 m?
1 answer:
Answer:
2.9 M
Explanation:
The concentration-time equation for a second order reaction is:
1/[A] = kt + 1/[A°]
Where,
A = concentration remaining at time, t
A° = initial concentration
k = rate constant
1/[A] = (1.80 x 10^-3) * (45.6) + 1/3.81
1/[A] = 0.345
= 1/0.345
= 2.9 M.
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