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∘freactan ts What is the value for the standard enthalpy of formation for Ag(s) that would be used in the equation above?

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

answer : one can design an experiment using a liquid and an additive that can be added to the liquid and observe the chemical changes in the reaction species.

one would need a beaker which is filled with a known amount of the liquid in which thermometer is placed to measure the temperature changes; after addition of the additive to the liquid solution one can note down the temperature change and find whether the reaction is endothermic or exothermic in nature. by subtracting the initial temperature value with the final temperature one can find the temperature changes.

various combinations of liquid and additive can be used. liquid in this case can be a known quantity of water and additives can be epsom salt or without epsom salt the experiment can be conducted to notice the changes. water and ice, hydrogen peroxide and dry yeast, vinegar and baking soda,etc.