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anonymous

  • one year ago

Suppose that 0.650mol of methane, CH4(g), is reacted with 0.800mol of fluorine, F2(g), forming CF4(g) and HF(g) as sole products. Assuming that the reaction occurs at constant pressure, how much heat is released?

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  1. anonymous
    • one year ago
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    data to use:

  2. anonymous
    • one year ago
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    i got -1834 kJ but i guess it's not right><

  3. anonymous
    • one year ago
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    first we have to balance the equation CH4 + 4F2 -> CF4 +4HF

  4. anonymous
    • one year ago
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    ok :)

  5. anonymous
    • one year ago
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    actually you should watch this video its very helpful https://www.youtube.com/watch?v=cKcnQACdOW8

  6. anonymous
    • one year ago
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    like i get it but i cant seem to gget the right answer

  7. anonymous
    • one year ago
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    let me post my work one second !

  8. anonymous
    • one year ago
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    ok nvm my phone is not gonna send. anyways i found the limiting reagent, and used q = delta Hrxn x (moles/4)

  9. anonymous
    • one year ago
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    i dont know if i did something wrong with conversions

  10. anonymous
    • one year ago
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    I know the problem the heat released is the delta h of the products times there coefficients minus the delta h of the reactants times there coefficients

  11. anonymous
    • one year ago
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    i still havent gotten the right answer><

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spraguer (Moderator)
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