Calculate ΔH298^∘ for the process Zn(s)+S(s)+2 O2(g) ⟶ZnSO4(s) from the following information:

step 1 Let's determine which osmium reaction produces more heat. In the first one, we have osmium solid

Calculate ΔH298^∘ for the process Zn(s)+S(s)+2 O2(g)...

Calculate $\Delta H_{298}^{\circ}$ for the process $\mathrm{Zn}(s)+\mathrm{S}(s)+2 \mathrm{O}_{2}(g) \longrightarrow \mathrm{ZnSO}_{4}(s)$ from the following information: $$\begin{array}{l}{\mathrm{Zn}(s)+\mathrm{S}(s) \longrightarrow \mathrm{ZnS}(s) \quad \Delta H_{298}^{\circ}=-206.0 \mathrm{kJ}} \\ {\mathrm{ZnS}(s)+2 \mathrm{O}_{2}(g) \longrightarrow \mathrm{ZnSO}_{4}(s) \quad \Delta H_{298}^{\circ}=-776.8 \mathrm{kJ}}\end{array}$$

Calculate $\Delta H_{298}^{\circ}$ for the process $\mathrm{Zn}(s)+\mathrm{S}(s)+2 \mathrm{O}_{2}(g) \longrightarrow \mathrm{ZnSO}_{4}(s)$ from the following information:
$$\begin{array}{l}{\mathrm{Zn}(s)+\mathrm{S}(s) \longrightarrow \mathrm{ZnS}(s) \quad \Delta H_{298}^{\circ}=-206.0 \mathrm{kJ}} \\ {\mathrm{ZnS}(s)+2 \mathrm{O}_{2}(g) \longrightarrow \mathrm{ZnSO}_{4}(s) \quad \Delta H_{298}^{\circ}=-776.8 \mathrm{kJ}}\end{array}$$

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Key Concepts

Standard State Conditions

Standard state conditions refer to a set of agreed-upon conditions (typically 298 K and 1 atm pressure) under which thermodynamic measurements like enthalpy change are tabulated. This standardization allows for consistent and comparable thermodynamic data across different reactions.

Thermochemical Equations

Thermochemical equations are balanced chemical equations that include the enthalpy change for the reaction. They provide a way to track the energy flow in individual steps, which can then be added together according to Hess's Law to determine the overall energy change.

Enthalpy Change (?H)

Enthalpy change represents the heat absorbed or released during a chemical reaction at constant pressure. It is an extensive property measured in kilojoules, and its calculation can involve summing known enthalpy changes from intermediate steps in a reaction.

Hess's Law

Hess's Law states that the total enthalpy change for a reaction is the same, no matter how many steps the reaction is carried out in, because enthalpy is a state function. This principle allows us to add enthalpy changes of individual steps to find the overall enthalpy change of a reaction.

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