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anonymous

  • one year ago

When a collision occurs between two reactant particles that, between them, have the required minimum kinetic energy, or activation energy, a product does not always form. Which of the following reasons explains this?

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  1. anonymous
    • one year ago
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    low temperature small surface area unfavorable geometry low concentration

  2. Photon336
    • one year ago
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    Technically particles have to have the right orientation, sufficient kinetic energy, and all that good stuff. When you raise the temperature, the fraction of particles that have sufficient kinetic energy to and are in the proper orientation increases, so the probability goes up. So higher temperature is a must, over lower temperature. When you increase concentration, that's more particles per a certain volume, that increases the number collisions between particles, and the likelihood your particles will collide to form your products. I believe surface area has the same effect.

  3. Photon336
    • one year ago
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    Thoughts? @arindameducationusc @Rushwr @taramgrant0543664 I don't think that it's temperature. it's gotta be unfavorable geometry. (surface area and, low concentration) i think have a similar effect.

  4. Rushwr
    • one year ago
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    I agree @Photon336

  5. anonymous
    • one year ago
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    Does your answer have an option of "All of the above"?

  6. ilovebmth1234
    • one year ago
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    yes it would be unforgivable geometry

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