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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?

Respuesta :

Answer: 0 kJ/mol

Explanation:

The enthalpy of formation for an element in its standard state is 0kJmol by definition. The standard state of elemental silver is Ag(s); thus Ag(s) will have an enthalpy of formation is equal to 0kJmol.

The value for the standard enthalpy of formation for Ag(s)  is zero.

What is Enthalpy of formation?

The standard enthalpy of formation of a substance is the enthalpy change that occurs when 1 mole of the substance is formed from its constituent elements in their standard states.

Condition for pure element:

A pure element in its standard state has a standard enthalpy of formation of zero. Thus, since silver is a pure element in solid state thus its enthalpy of formation will be zero.

Find more information about Enthalpy of formation here:

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