Sulfur dioxide gas reacts with oxygen, O2(g), to produce SO3(g) . This reaction releases 99.0 k

step 1 So what we have here is the combustion reaction where we have 1 mole of sulfur dioxide and oxyge

Sulfur dioxide gas reacts with oxygen, O2(g), to produce...

Sulfur dioxide gas reacts with oxygen, $\mathrm{O}_{2}(g)$, to produce $\mathrm{SO}_{3}(g) .$ This reaction releases $99.0 \mathrm{~kJ}$ of heat (at constant pressure) for each mole of sulfur dioxide that reacts. Write the thermochemical equation for the reaction of $2 \mathrm{~mol}$ of sulfur dioxide, and then also for the decomposition of $3 \mathrm{~mol}$ of sulfur trioxide gas into oxygen gas and sulfur dioxide gas. Do you need any other information to answer either question?

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Key Concepts

Thermochemical Equations

These are chemical equations that include the amount of energy released or absorbed during a reaction, usually represented as heat. They combine the chemical stoichiometry with thermodynamic data, allowing one to track both the substances and the associated energy change in a reaction.

Stoichiometry

This concept deals with the quantitative relationships between reactants and products in a balanced chemical equation. It is essential when scaling up or down the number of moles involved in a reaction, ensuring that the proportionality between chemical species and energy changes is maintained.

Scaling of Reaction Enthalpy

When a chemical equation is multiplied by a factor to reflect a different number of moles reacting, the enthalpy change must also be multiplied by this factor. This ensures that the energy change is accurately represented for the provided stoichiometric amounts in the reaction.

Reversing Chemical Reactions and Enthalpy Change

When a chemical reaction is reversed, the sign of the enthalpy change also reverses. This is critical when writing equations for the reverse or decomposition reactions, ensuring that the energy flow (endothermic versus exothermic) is correctly annotated.

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