Sulfur trioxide decomposes to sulfur and oxygen. (9.2,9.6) 2 SO3(g) ⟶2 S(s)+3 O2(g) ΔH=+790

step 1 All right, so we have here a balanced thermochemical equation. For part A, we want to know if it

Sulfur trioxide decomposes to sulfur and oxygen. (9.2,9.6) 2...

Sulfur trioxide decomposes to sulfur and oxygen. $(9.2,9.6)$ $$ 2 \mathrm{SO}_{3}(g) \longrightarrow 2 \mathrm{~S}(s)+3 \mathrm{O}_{2}(g) \quad \Delta H=+790 \mathrm{~kJ} $$ a. Is the reaction exothermic or endothermic? b. How many kilojoules are required when $1.5 \mathrm{~mol}_{\text {of } \mathrm{SO}_{3}}$ reacts? c. How many kilojoules are required when $150 \mathrm{~g}$ of $\mathrm{O}_{2}$ is formed?

Sulfur trioxide decomposes to sulfur and oxygen. $(9.2,9.6)$
$$
2 \mathrm{SO}_{3}(g) \longrightarrow 2 \mathrm{~S}(s)+3 \mathrm{O}_{2}(g) \quad \Delta H=+790 \mathrm{~kJ}
$$
a. Is the reaction exothermic or endothermic?
b. How many kilojoules are required when $1.5 \mathrm{~mol}_{\text {of } \mathrm{SO}_{3}}$ reacts?
c. How many kilojoules are required when $150 \mathrm{~g}$ of $\mathrm{O}_{2}$ is formed?

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Key Concepts

Enthalpy Change Calculations

Enthalpy change is a measure of the heat absorbed or released during a reaction at constant pressure. It is often given per the mole or per the balanced reaction, and calculations involve scaling this value according to the amount of reagent or the fraction of the reaction occurring.

Mole-Mass Conversions

This concept involves converting between the mass of a substance and the number of moles using its molar mass. It is fundamental in chemical calculations where the quantitative relationship between mass and amount of substance, expressed in moles, is necessary for stoichiometric computations.

Exothermic and Endothermic Reactions

This concept pertains to whether a chemical reaction releases or absorbs energy, usually in the form of heat. In exothermic reactions, energy is released to the surroundings, whereas in endothermic reactions, energy is absorbed from the surroundings. Understanding this helps in predicting temperature changes and energy requirements in a reaction.

Stoichiometry in Chemical Reactions

Stoichiometry involves using the balanced chemical equation to relate the quantities of reactants and products in a reaction. It enables one to calculate the amounts of substances consumed or produced, based on the mole ratios provided by the coefficients in the chemical equation.

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