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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?
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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anonymous
 one year ago
Best ResponseYou've already chosen the best response.0i got 1834 kJ but i guess it's not right><

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0first we have to balance the equation CH4 + 4F2 > CF4 +4HF

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0actually you should watch this video its very helpful https://www.youtube.com/watch?v=cKcnQACdOW8

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0like i get it but i cant seem to gget the right answer

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0let me post my work one second !

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0ok nvm my phone is not gonna send. anyways i found the limiting reagent, and used q = delta Hrxn x (moles/4)

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0i dont know if i did something wrong with conversions

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0I 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
 one year ago
Best ResponseYou've already chosen the best response.0i still havent gotten the right answer><
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