SUMMARY
The discussion centers on calculating the time required for a first-order reaction to reach a concentration of 1/8 of its initial value, given a rate constant of 6.70×10−3. The half-life for this reaction is determined using the formula half-life = 0.693/k, resulting in a half-life of 103.43 units of time. It is established that reaching 1/8 concentration requires three half-lives, as each half-life reduces the concentration by half: 1/2 after one half-life, 1/4 after two, and 1/8 after three.
PREREQUISITES
- Understanding of first-order reaction kinetics
- Familiarity with the half-life formula: half-life = 0.693/k
- Basic knowledge of exponential decay functions
- Ability to perform simple mathematical calculations involving fractions
NEXT STEPS
- Study the implications of first-order kinetics in chemical reactions
- Learn about the derivation and applications of the half-life formula
- Explore exponential decay models in various scientific contexts
- Investigate the impact of different rate constants on reaction times
USEFUL FOR
Chemistry students, educators, and professionals involved in chemical kinetics or reaction rate analysis will benefit from this discussion.