anonymous
  • anonymous
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?
Chemistry
chestercat
  • chestercat
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anonymous
  • anonymous
data to use:
anonymous
  • anonymous
i got -1834 kJ but i guess it's not right><
anonymous
  • anonymous
first we have to balance the equation CH4 + 4F2 -> CF4 +4HF

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anonymous
  • anonymous
ok :)
anonymous
  • anonymous
actually you should watch this video its very helpful https://www.youtube.com/watch?v=cKcnQACdOW8
anonymous
  • anonymous
like i get it but i cant seem to gget the right answer
anonymous
  • anonymous
let me post my work one second !
anonymous
  • anonymous
ok nvm my phone is not gonna send. anyways i found the limiting reagent, and used q = delta Hrxn x (moles/4)
anonymous
  • anonymous
i dont know if i did something wrong with conversions
anonymous
  • anonymous
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
anonymous
  • anonymous
i still havent gotten the right answer><

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