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Consider the reaction described by the following chemical equation. 2 Ag2S(s) + 2 H2O(l) ⟶ 4 Ag(s) + 2 H2S(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∘ = ∑nΔHf products ∘−∑nΔHf 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

Consider the reaction described by the following chemical equation. 2 Ag2S(s) + 2 H2O(l) ⟶ 4 Ag(s) + 2 H2S(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∘ = ∑nΔHf products ∘−∑nΔHf 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

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Consider the reaction described by the following chemical equation.
2 A g 2 S ( s ) + 2 H 2 O ( l ) ⟶ 4 A g ( s ) + 2 H 2 S ( g ) + O 2 ( g ) Δ H r x n ∘ = 595.5 k J m o l
The change in enthalpy for this reaction can be determined theoretically by using the standard enthalpies of formation for the species involved.
Δ H r x n ∘ = ∑ n Δ H f products ∘ − ∑ n Δ H f reactants ∘
What is the value for the standard enthalpy of formation for A g ( s ) that would be used in the equation above?
Provide your answer below: ◻ k J / m o l

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