JAMB - Chemistry (2004 - No. 26)
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
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
Explanation
Energy change = ΔH\(_{product}\) - ΔH\(_{reactants}\)
Given: ΔH\(_{CO_2}\) = - 393, ΔH\(_{CO}\) = - 110.4 , ΔH\(_{O_2}\) = 0 (The standard enthalpy of formation for molecular oxygen (O\(_2\)) is zero because oxygen in its diatomic form (O\(_2\)) is the most stable form of oxygen under standard conditions).
Energy change (ΔH) = ΔH\(_{CO_2}\) - (ΔH\(_{CO}\) + ΔH\(_{O_2}\))
= - 393 - ( - 110.4 + 0)
= - 393 + 110.4
= -282.6 kJ
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