For a first order reaction if the time for 50%, 75% and 87.5% changes are t1, t2 and t3 respectively then what would be the value of t1: t2: t3 ?
Recall, for a first order elementary reaction,
Without more data, I couldn't give you a real value, but I could give you one as a factor of
We can conceptually assume that
Consider a first-order reaction
The time required for the initial concentration
#1/2["A"]_0#is one half-life #1/4["A"]_0#is two half-lives #1/8["A"]_0#is three half-lives
The ratios are
Here is a typical plot for a first-order reaction.
The initial concentration is 1.7.
- 400 s for the concentration to drop by 50 % (to 0.85)
- 800 s for the concentration to drop by 75 % (0.42)
- 400 s for the concentration to drop by 87.5 % (to 0.21)
The times are in the ratio