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vera_ewing

  • one year ago

How does adding NH3 to the reaction below affect the equilibrium of the reaction? N2(g) + 3H2(g) 2NH3(g) A. Increasing the amount of NH3 will make Q smaller than K. A net reaction occurs in the direction to increase NH3, or the forward reaction. B. Increasing the amount of NH3 will make Q smaller than K. A net reaction occurs in the direction to reduce NH3, or the reverse reaction. C. Increasing the amount of NH3 will make Q larger than K. A net reaction occurs in the direction to increase NH3, or the forward reaction. D. Increasing the amount of NH3 will make Q larger th

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  1. vera_ewing
    • one year ago
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    @sweetburger A or B?

  2. sweetburger
    • one year ago
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    Does D say that Increasing the amount of NH3 will make Q larger than K. A net reaction occurs in the direction to reduce NH3, or the reverse reaction. ?

  3. vera_ewing
    • one year ago
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    Increasing the amount of NH3 will make Q larger than K. A net reaction occurs in the direction to reduce NH3, or the reverse reaction.

  4. sweetburger
    • one year ago
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    Pretty sure it is D. As q represents the initial reaction quotient. If the reaction quotient has the amount of products increased which is the numerator it will become larger than the K value. To get Q to become K a reverse reaction must occur.

  5. vera_ewing
    • one year ago
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    Yeah you're right. Thank you.

  6. vera_ewing
    • one year ago
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  7. vera_ewing
    • one year ago
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    How about this one? I think either B or C.

  8. sweetburger
    • one year ago
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    i think you just take the square root of the solubility

  9. vera_ewing
    • one year ago
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    So D?

  10. sweetburger
    • one year ago
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    No, I believe it would be B.

  11. sweetburger
    • one year ago
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    i said that [Ag+][I-]=8.5x10^-17 then i let Ag and I represent x xo [x][x]=8.5x1-^-17 so \[\sqrt{8.5x10^-17} =9.2x10^-9\]

  12. sweetburger
    • one year ago
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    so x= 9.2x10^-9

  13. vera_ewing
    • one year ago
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    Ohh I see. Thanks for explaining that!

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