nitrogen monoxide gas spontaneously decomposes into dinitrogen oxide and nitroge
ID: 909135 • Letter: N
Question
nitrogen monoxide gas spontaneously decomposes into dinitrogen oxide and nitrogen dioxide gases. what is the standard entropy change for the decomposition of 3.0 mol of nitrogen monoxidenitrogen monoxide gas spontaneously decomposes into dinitrogen oxide and nitrogen dioxide gases. what is the standard entropy change for the decomposition of 3.0 mol of nitrogen monoxide
nitrogen monoxide gas spontaneously decomposes into dinitrogen oxide and nitrogen dioxide gases. what is the standard entropy change for the decomposition of 3.0 mol of nitrogen monoxide
Explanation / Answer
Values tabulated standard molar entropy can be used to calculate the entropy of a chemical reaction, similar to the use of enthalpies of formation to determine the enthalpy change, seen in a previous section.
Unlike what happens in the use of entropy standard molar, when we calculate the entropy of a reaction if we put the Greek letter delta, , ie, S, because we speak of entropy from an initial state to a final state (product of reagents):
Sro = Sproductos - Sreactivos
For a generic reaction:
aA -> cC + dD
Total entropy of products: c · Smo (C) + d · Blessed (D)
Total entropy of the reactants: a · Smo (A)
(We multiply the entropies of each species by the stoichiometric coefficient because as molars are for 1 mole of compound, so it should consider the total moles present).
Thus, the entropy of the reaction will be:
Sro = total entropy of products - total entropy of the reactants
Sro = c · Smo (C) + d · Blessed (D) - [a · Smo (A)]
Sro = (2*(240.5+216.2)- [3*210.6]
=913.4-631.8=281.6 J/K
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