d) 2KBr(s) 2K(s) + Br2(g):
9) The Bunsen burner in our lab is fueled by mostly methane CH4. The thermochemical
equation for the combustion of methane is:
CH4 (g) +202 (g) → CO2 (g) + 2H2O(1) AH = -890.3kJ
a) Calculate AH when 5.00g of O2 react.
ΔΗΣ
5.00g Oxmox - 890,3KJ = (-69,55 kJ
3290
2mol
b) How many moles of methane are needed to release 487kJ of energy?
487KJmol CH4
-890.3KJ CH4
= 0.547 mol CH4