using-the-thermodynamic-values-below-determine-the-s-rxn-for-the-following-react

Question

Using the thermodynamic data below calculate the ΔS°_{rxn} for the following reaction and justify the change in entropy.CO(g) + NH_{3}(g) → HCN(g) + $$H_{2}O(g)$$

Accepted Answer

ΔS°_{rxn} = +0.1 J/mol; The change in entropy is very small because the moles of gas in the reaction are the same.

Answer

ΔS°_{rxn} = +6.1 J/mol; The change in entropy is very small because the moles of gas in the reaction are the same.

Answer

ΔS°_{rxn} = –0.1 J/mol; The change in entropy is very small because the size and shape of the species in the reaction are the same.

Answer

ΔS°_{rxn} = –6.1 J/mol; The change in entropy is very small because the size and shape of the species in the reaction are the same.

Answer

ΔS°_{rxn} = +0.1 J/mol; The change in entropy is very small because the size and shape of the species in the reaction are the same.

Answer

ΔS°_{rxn} = –6.1 J/mol; The change in entropy is very small because the moles of gas in the reaction are the same.

Using the thermodynamic data below calculate the ΔS°rxn for the following reaction and justify the change in entropy.CO(g) + NH3(g) → HCN(g) + H2O(g)

Using the thermodynamic data below calculate the ΔS°_rxn for the following reaction and justify the change in entropy.
CO(g) + NH₃(g) → HCN(g) + H₂O(g)