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anonymous

  • one year ago

Which of the following will shift this equilibrium system to the left? Energy + N2O4 (g) Two arrows stacked on top of each other. The top arrow points to the right. The bottom arrow points to the left. 2 NO2 (g) Increasing the concentration of N2O4 Increasing the volume of the container Decreasing the temperature of the system Decreasing the concentration of NO2

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  1. anonymous
    • one year ago
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    @Photon336

  2. anonymous
    • one year ago
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    ok

  3. Photon336
    • one year ago
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    increasing the concentration of N2O4 would push the reaction to the right so I think that's out

  4. anonymous
    • one year ago
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    so d is wrong also

  5. Photon336
    • one year ago
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    |dw:1439931673570:dw| Increasing the volume though would decrease the pressure and that means that the reaction is going to favor the side with the greater number of moles which is the product so that's out too.

  6. anonymous
    • one year ago
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    so c is left and correct

  7. Photon336
    • one year ago
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    i think it's decreasing concentration of NO2 would go to reactants; @taramgrant0543664 what do you think?

  8. taramgrant0543664
    • one year ago
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    In order to reach an equilibrium if you decrease the concentration of the NO2 it's going to want to increased he concentration to achieve equilibrium again so that would go to products

  9. anonymous
    • one year ago
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    so decreasing the temperature would be rigt

  10. anonymous
    • one year ago
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    @taramgrant0543664

  11. Photon336
    • one year ago
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    wait.. it's endothermic increasing temperature would favor products but decreasing temp would favor reactants.

  12. Photon336
    • one year ago
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    I'm more sure on C now but still.. @taramgrant0543664 could you explain why it's not D

  13. taramgrant0543664
    • one year ago
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    Yes it would @Photon

  14. taramgrant0543664
    • one year ago
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    If you decrease the concentration of the products when the reaction had already achieved equilibrium it's going to want to achieve equilibrium again since the decrease in concentration kicked it out of its equilibrium. In order for the products to achieve the equilibrium they want to increase the concentration, the increase in concentration will allow the reaction to achieve its equilibrium back. The increase in concentration for the products occurs when more products get made so therefore the forward reaction, so the shift to the right will occur

  15. Photon336
    • one year ago
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    so.. it's under the assumption that the reaction was already at equilibrium. the decreased concentration of product disrupted equilibrium.

  16. Photon336
    • one year ago
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    so something is being removed..say a product, that pushes the reaction to the right

  17. taramgrant0543664
    • one year ago
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    Ya I just assumed that it was at equilibrium because it didn't say anything to contradict that possibility If you remove product the reaction proceeds in forward direction If you remove reactant the reaction proceeds in the reverse direction

  18. Photon336
    • one year ago
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    Thank you tara, my brain hurts so I have to go lol

  19. taramgrant0543664
    • one year ago
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    No problem go have a rest you deserve it!

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