What is ΔS° for the reaction between nitrogen gas and fluorine gas to form nitrogen trifluoride gas, and how can the sign of ΔS° be rationalized?

Verified step by step guidance

1. <insert step 1> Identify the balanced chemical equation for the reaction: \( N_2(g) + 3F_2(g) \rightarrow 2NF_3(g) \).
2. <insert step 2> Determine the standard molar entropy (S°) values for each substance involved in the reaction from a reliable data source.
3. <insert step 3> Calculate the change in standard entropy (ΔS°) for the reaction using the formula: \( \Delta S^\circ = \sum S^\circ_{\text{products}} - \sum S^\circ_{\text{reactants}} \).
4. <insert step 4> Substitute the standard molar entropy values into the formula to find ΔS°.
5. <insert step 5> Rationalize the sign of ΔS° by considering the change in the number of gas molecules: the reaction goes from 4 moles of gas (1 mole of \(N_2\) and 3 moles of \(F_2\)) to 2 moles of \(NF_3\), indicating a decrease in entropy.>