Consider the reaction described by the following chemical equation. 2Ag2S (s) + 2H2O (l) ⟶4Ag (s) + 2H2S (g) + O2 (g) ΔH∘rxn=595.5kJmol The change in enthalpy for this reaction can be determined theoretically by using the standard enthalpies of formation for the species involved. ΔH∘rxn=∑nΔH∘fproducts-∑nΔH∘freactants What is the value for the standard enthalpy of formation for Ag (s) that would be used in the equation above?

Question

Izabella Henry

Chemistry

26 April, 03:03

Consider the reaction described by the following chemical equation. 2Ag2S (s) + 2H2O (l) ⟶4Ag (s) + 2H2S (g) + O2 (g) ΔH∘rxn=595.5kJmol The change in enthalpy for this reaction can be determined theoretically by using the standard enthalpies of formation for the species involved. ΔH∘rxn=∑nΔH∘fproducts-∑nΔH∘freactants What is the value for the standard enthalpy of formation for Ag (s) that would be used in the equation above?

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Answers (1)

Know the Answer?

Deon Benson · Answer 1

standard enthalpy of formation for Ag (s) value = 0

Explanation:

standard enthalpy of formation for a single elements is = 0 hence,

standard enthalpy of formation for Ag (s) = 0