Questions: Submitting an external tool Question Consider the reaction described by the following chemical equation. 2 Ag2 S(s)+2 H2 O(l) -> 4 Ag(s)+2 H2 S(g)+O2(g) ΔHrxn^°=595.5 kJ/mol The change in enthalpy for this reaction can be determined theoretically by using the standard enthalpies of formation for the species involved. ΔHrxn^°=∑ n ΔHf products^°-∑ n ΔHf reactants^° What is the value for the standard enthalpy of formation for Ag(s) that would be used in the equation above? Provide your answer below: kJ / mol

Submitting an external tool Question Consider the reaction described by the following chemical equation. 2 Ag2 S(s)+2 H2 O(l) -> 4 Ag(s)+2 H2 S(g)+O2(g) ΔHrxn^°=595.5 kJ/mol The change in enthalpy for this reaction can be determined theoretically by using the standard enthalpies of formation for the species involved. ΔHrxn^°=∑ n ΔHf products^°-∑ n ΔHf reactants^° What is the value for the standard enthalpy of formation for Ag(s) that would be used in the equation above? Provide your answer below: kJ / mol
Transcript text: Submitting an external tool Question Consider the reaction described by the following chemical equation. \[ 2 \mathrm{Ag}_{2} \mathrm{~S}(\mathrm{~s})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \longrightarrow 4 \mathrm{Ag}(\mathrm{~s})+2 \mathrm{H}_{2} \mathrm{~S}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \quad \Delta H_{\mathrm{r} \times \mathrm{n}}^{\circ}=595.5 \frac{\mathrm{~kJ}}{\mathrm{~mol}} \] The change in enthalpy for this reaction can be determined theoretically by using the standard enthalpies of formation for the species involved. \[ \Delta H_{\mathrm{rxn}}^{\circ}=\sum n \Delta H_{f \text { products }}^{\circ}-\sum n \Delta H_{f \text { reactants }}^{\circ} \] What is the value for the standard enthalpy of formation for $\mathrm{Ag}(\mathrm{s})$ that would be used in the equation above? Provide your answer below: $\square$ $\mathrm{kJ} / \mathrm{mol}$ Next .
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Solution

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Solution Steps

Step 1: Understanding the Reaction and Enthalpy Change

The given reaction is:

\[ 2 \mathrm{Ag}_{2} \mathrm{~S}(\mathrm{~s})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \longrightarrow 4 \mathrm{Ag}(\mathrm{~s})+2 \mathrm{H}_{2} \mathrm{~S}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \]

The standard enthalpy change for the reaction is given as:

\[ \Delta H_{\mathrm{r} \times \mathrm{n}}^{\circ}=595.5 \frac{\mathrm{~kJ}}{\mathrm{~mol}} \]

Step 2: Using the Standard Enthalpy of Formation Equation

The standard enthalpy change of the reaction (\(\Delta H_{\mathrm{rxn}}^{\circ}\)) can be calculated using the standard enthalpies of formation (\(\Delta H_f^{\circ}\)) of the reactants and products:

\[ \Delta H_{\mathrm{rxn}}^{\circ} = \sum n \Delta H_{f \text { products }}^{\circ} - \sum n \Delta H_{f \text { reactants }}^{\circ} \]

Step 3: Identifying the Standard Enthalpy of Formation for Silver

The standard enthalpy of formation for an element in its standard state is zero. Silver (\(\mathrm{Ag}\)) in its solid form is in its standard state. Therefore, the standard enthalpy of formation for \(\mathrm{Ag}(\mathrm{s})\) is:

\[ \Delta H_f^{\circ}(\mathrm{Ag}(\mathrm{s})) = 0 \, \mathrm{kJ/mol} \]

Final Answer

\[ \boxed{0 \, \mathrm{kJ/mol}} \]

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