Question:

The time required for completion of 93.75% of a first order reaction is $x$ minutes. The half-life of it (in minutes) is

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Remember the percentage completion to half-life equivalents: 93.75% = 4 half-lives.

Updated On: May 19, 2025

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For a first order reaction, time for 93.75% completion = 4 half-lives ($t = 4t_{1/2}$)
So, $x = 4t_{1/2} \Rightarrow t_{1/2} = x/4$

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Experiment	\([A]\) (mol L\(^{-1}\))	\([B]\) (mol L\(^{-1}\))	Initial Rate (mol L\(^{-1}\) min\(^{-1}\))
1	0.01	0.01	\(5 \times 10^{-3}\)
2	0.02	0.01	\(1 \times 10^{-2}\)
3	0.01	0.02	\(5 \times 10^{-3}\)

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