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A first order reaction initially contains 1. 00 × 10²⁰ molecules. If the reaction has a half-life of 20. 0 minutes, how many molecules remain unreacted after 80. 0 minutes?.

Respuesta :

Using proportions, it is found that [tex]1.25 \times 10^{19}[/tex] molecules remain unreacted after 80. 0 minutes.

What is a proportion?

A proportion is a fraction of a total amount.

In this problem, the half-life of the reaction is of 20 minutes, hence:

  • After 20 minutes, 50% of the molecules are unreacted.
  • After 40 minutes, 25% of the molecules are unreacted.
  • After 80 minutes, 12.5% of the molecules are unreacted.

Then:

[tex]0.125 \times 10^{20} = 1.25 \times 10^{19}[/tex]

Hence:

[tex]1.25 \times 10^{19}[/tex] molecules remain unreacted after 80. 0 minutes.

More can be learned about proportions at https://brainly.com/question/24372153

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