2CO(g) + O\(_2\)(g) → 2CO\(_2\)(g)
Given that ΔH[CO]is -110.4 kJmol-1 and ΔH[CO\(_2\)] is -393.0 kJmol-1, the energy change for the reaction above is
- -503.7 kJ
-
-282.6 kJ
- +282.6 kJ
- +503.7 kJ
The correct answer is: B
Explanation
Energy change = ΔH\(_{product}\) - ΔH\(_{reactants}\)
Energy change (ΔH) = 2ΔH\(_{CO2}\) - (2ΔH\(_{CO}\) + ΔH\(_{O2}\))
= - 393 - ( - 110.4 + 0)
= - 393 + 110.4
= -282.6 kJ