The time for half life of a first order reaction is 1 hour . What's th...
First half life 50% second half life (50+25)%third half life (50+25+12.5)% which is equal to 87.5%this implies (1+1+1) hrs i.e 3 hours
The time for half life of a first order reaction is 1 hour . What's th...
Time for 87.5% completion of a first-order reaction
To determine the time required for 87.5% completion of a first-order reaction, we need to understand the concept of half-life and how it relates to the reaction's progress.
What is half-life?
The half-life of a reaction is the time it takes for the concentration of a reactant to decrease to half of its initial value. In a first-order reaction, the half-life remains constant regardless of the reactant's initial concentration.
Given that the half-life of the reaction is 1 hour, we can use this information to find the time required for 87.5% completion.
Step 1: Calculate the number of half-lives to reach 87.5% completion
To find the number of half-lives needed to reach 87.5% completion, we can use the formula:
Number of half-lives = (ln(initial concentration/final concentration)) / (ln(2))
Since we want to find the time taken for 87.5% completion, the final concentration will be 12.5% (100% - 87.5%) of the initial concentration.
Number of half-lives = ln(100/12.5) / ln(2)
Number of half-lives ≈ 3.5
Step 2: Calculate the time taken for 87.5% completion
Since each half-life takes 1 hour, we can multiply the number of half-lives by the half-life time to determine the total time taken for 87.5% completion.
Time taken = Number of half-lives * Half-life time
Time taken = 3.5 * 1 hour
Time taken = 3.5 hours
Thus, it takes approximately 3.5 hours for a first-order reaction to reach 87.5% completion, given that the half-life is 1 hour.
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