The enthalpy of the reaction, [tex]S_{(s)} + O_{2}_{(g)} \rightarrow SO_{2}_{(g)}[/tex], ΔH is -197 kJ.
What is the enthalpy change of the reaction?
The enthalpy change of a reaction, ΔH, is the heat absorbed or given off when reactants form products for a given reaction.
The enthalpy change, ΔH, of the reaction given below:
[tex]S_{(s)} + O_{2}_{(g)} \rightarrow SO_{2}_{(g)}[/tex]
The enthalpy change is calculated from the intermediate reactions:
[tex]S_{(s)} + \frac{3}{2}\:O_{2}_{(g)} \rightarrow SO_{3}_{(g)} \:\Delta H_{1} = -395.2 \:kJ\\SO_{3}_{(g)}\rightarrow SO_{2}{(g)} + \frac{1}{2}O_{2}_{(g)} \:\Delta H_{2} = 198.2\:kJ[/tex]
ΔH = ΔH₁ + ΔH₂
ΔH = -395.2 + 198.2 kJ
ΔH = -197 kJ
Therefore, the enthalpy of the reaction, [tex]S_{(s)} + O_{2}_{(g)} \rightarrow SO_{2}_{(g)}[/tex], ΔH = -197 kJ.
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