Use the reaction to answer the question.
CH4 + 2O2 → CO2 + 2H2O
H–C: 412 kJ/mol
O=O: 496 kJ/mol
C=O: 743 kJ/mol
O–H: 463 kJ/mol
What is the total energy of the reaction?
(1 point)
Responses
228 kJ/mol
228 kJ/mol
294 kJ/mol
294 kJ/mol
–265 kJ/mol
–265 kJ/mol
–698 kJ/mol
–698 kJ/mol
To find the total energy of the reaction, you need to calculate the energy change for each bond broken and formed.
Breaking bonds:
4 x C-H = 4 x 412 kJ/mol = 1648 kJ/mol
4 x O=O = 4 x 496 kJ/mol = 1984 kJ/mol
Forming bonds:
2 x C=O = 2 x 743 kJ/mol = 1486 kJ/mol
4 x O-H = 4 x 463 kJ/mol = 1852 kJ/mol
Total energy change = (energy of bonds broken) - (energy of bonds formed)
= (1648 kJ/mol + 1984 kJ/mol) - (1486 kJ/mol + 1852 kJ/mol)
= 3632 kJ/mol - 3338 kJ/mol
= 294 kJ/mol
Therefore, the total energy change of the reaction is 294 kJ/mol.