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?

Question

anonymous · Answer

data to use:

anonymous · Answer

i got -1834 kJ but i guess it's not right><

anonymous · Answer

first we have to balance the equation CH4 + 4F2 -> CF4 +4HF

anonymous · Answer

ok :)

anonymous · Answer

actually you should watch this video its very helpful https://www.youtube.com/watch?v=cKcnQACdOW8

anonymous · Answer

like i get it but i cant seem to gget the right answer

anonymous · Answer

let me post my work one second !

anonymous · Answer

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

anonymous · Answer

i dont know if i did something wrong with conversions

anonymous · Answer

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 · Answer

i still havent gotten the right answer><