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anonymous

  • one year ago

Graphs of two different reactions are shown. ’both graphs show the reaction pathway on the x-axis and potential energy on the y-axis. Graph A shows reactants at a low potential energy an increase to a high potential energy and products at a lower potential energy than the peak, but a higher potential energy than the reactants. Graph B shows reactants at a high potential energy, a slight increase and then a drop to products at a lower potential energy. Compare the activation energies of these two reactions.

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  1. anonymous
    • one year ago
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    Reaction A requires more activation energy. Reaction B requires more activation energy. Both reactions require the same amount of activation energy, but reaction A absorbs more of this energy. Both reactions require the same amount of activation energy, but reaction B absorbs more of this energy.

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  2. anonymous
    • one year ago
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    @Cuanchi

  3. anonymous
    • one year ago
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    @Cuanchi

  4. anonymous
    • one year ago
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    @ChantySquirrel1129**

  5. anonymous
    • one year ago
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    @texaschic101

  6. anonymous
    • one year ago
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    @timo86m

  7. anonymous
    • one year ago
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    @Koikkara

  8. anonymous
    • one year ago
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    @Photon336

  9. Photon336
    • one year ago
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    okay @d2live82

  10. anonymous
    • one year ago
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    ? @Photon336

  11. Photon336
    • one year ago
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    the first reaction is endothermic because the energy for the products is higher than the reactants. while the second one is exothermic because the energy of the products is lower than the reactants.

  12. anonymous
    • one year ago
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    I don't get it tbh

  13. Photon336
    • one year ago
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    Take a look at this \[\Delta H = Products - Reactants \] \[\Delta H < 0 exothermic \] \[\Delta H > 0 heat = ,absorbed, endothermic \] |dw:1444278904776:dw|

  14. Photon336
    • one year ago
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    If you notice something? the first reaction the energy for the products is greater than the reactants so it would be exothermic what about the second graph based off of what I said what would it be?

  15. anonymous
    • one year ago
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    i think its called endothermic right?

  16. Photon336
    • one year ago
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    The first one would be endothermic and the second one exothermic

  17. anonymous
    • one year ago
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    hmmmm....

  18. Photon336
    • one year ago
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    I believe that the activation energies are the same

  19. Photon336
    • one year ago
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    but what is different about the first and second reactions? in terms of energy

  20. anonymous
    • one year ago
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    the products are opposite

  21. Photon336
    • one year ago
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    yeah, the first reaction is endothermic so it needs to absorb energy, the second reaction is exothermic and it releases energy

  22. anonymous
    • one year ago
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    tbh i might be wrong when i say this but is it A/B or C/D? as in like which 2 should i look at more.

  23. anonymous
    • one year ago
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    @Photon336

  24. Photon336
    • one year ago
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    I think it's between C/D

  25. anonymous
    • one year ago
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    okay

  26. anonymous
    • one year ago
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    @Photon336 is it C?

  27. anonymous
    • one year ago
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    that one word made me feel so dumb....

  28. Photon336
    • one year ago
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    LOL I didnt even see that was a huge typo

  29. anonymous
    • one year ago
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    oh... okay lol... can you dumb it down for me then haha..

  30. Photon336
    • one year ago
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    Why do you think it's C??

  31. Photon336
    • one year ago
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    |dw:1444280117908:dw|

  32. anonymous
    • one year ago
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    Because of when it says "Both reactions require the same amount of activation energy, but reaction A absorbs more of this energy", to me it's sayings that they need the same amount of energy but one just absorbs more so i just thought it was that

  33. anonymous
    • one year ago
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    Okay i have no clue again ._.

  34. Photon336
    • one year ago
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    I think that's right

  35. anonymous
    • one year ago
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    really?

  36. Photon336
    • one year ago
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    because reaction A above is endothermic and it absorbs energy. they both need the same energy to get started.

  37. anonymous
    • one year ago
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    meh it's okay i kinda gave up i'll try it tomorrow it's late

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