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Ch.18 - Free Energy and Thermodynamics
Chapter 18, Problem 58

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?

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1
<insert step 1> Identify the balanced chemical equation for the reaction: N2(g)+3F2(g)2NF3(g).
<insert step 2> Determine the standard molar entropy (S°) values for each substance involved in the reaction from a reliable data source.
<insert step 3> Calculate the change in standard entropy (ΔS°) for the reaction using the formula: ΔS=SproductsSreactants.
<insert step 4> Substitute the standard molar entropy values into the formula to find ΔS°.
<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 N2 and 3 moles of F2) to 2 moles of NF3, indicating a decrease in entropy.>