Methane combusts according to the following thermochemical equation: CH4 (g) +2O2 (g) - CO2 (g) + 2H2O(I) AH = -891 kJ
If 25 g of methane combusts, how much energy is released in the reaction?
(Show all work and answer with the correct significant figures and units.)
CH4(g) + 202(g) --> CO2(g) + 2H2O(g)deltaH = -891 kJ/mol.
Multipliedby2: = - 1780.8.4k) multipled by ZAH=-
I= -445.2kJ
AH°rxn = [2AHºf(CO2) + 3AHºf(H20)]-[AH°f(C2H5OH) + 3AH° S(02)] = [2( - 393.5kJ).+31 - 2
41.8)] - [ - 277.7) + 3(0)]= -1234.7kJ