Which one of the following reactions is spontaneous at all temperatures? Group of answer choices N2(g) + 3 F2(g) → 2 NF3(g) ΔH° =−249 kJ/mol ; ΔS° = −278 J/K-mol N2(g) + 3 Cl2(g) → 2 NCl3(g) ΔH° = +460 kJ/mol; ΔS° = −275 J/K-mol N2F4(g) → 2 NF2(g) ΔH° =+85 kJ/mol ; ΔS° = +198 J/K-mol NH4NO3(s) → N2O(g) + 2H2O(ℓ) ΔH° =−125 kJ/mol ; ΔS° = +209 J/K-mol
Which one of the following reactions is spontaneous at all temperatures? Group of answer choices N2(g) + 3 F2(g) → 2 NF3(g) ΔH° =−249 kJ/mol ; ΔS° = −278 J/K-mol N2(g) + 3 Cl2(g) → 2 NCl3(g) ΔH° = +460 kJ/mol; ΔS° = −275 J/K-mol N2F4(g) → 2 NF2(g) ΔH° =+85 kJ/mol ; ΔS° = +198 J/K-mol NH4NO3(s) → N2O(g) + 2H2O(ℓ) ΔH° =−125 kJ/mol ; ΔS° = +209 J/K-mol
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Chapter18: Thermodynamics And Equilibrium
Section: Chapter Questions
Problem 18.20QP: Given the following information at 25C, calculate G at 25C for the reaction 2A(g)+B(g)3C(g)...
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Question
Which one of the following reactions is spontaneous at all temperatures?
Group of answer choices
N2(g) + 3 F2(g) → 2 NF3(g) ΔH° =−249 kJ/mol ; ΔS° = −278 J/K-mol
N2(g) + 3 Cl2(g) → 2 NCl3(g) ΔH° = +460 kJ/mol; ΔS° = −275 J/K-mol
N2F4(g) → 2 NF2(g) ΔH° =+85 kJ/mol ; ΔS° = +198 J/K-mol
NH4NO3(s) → N2O(g) + 2H2O(ℓ) ΔH° =−125 kJ/mol ; ΔS° = +209 J/K-mol
Expert Solution
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Step 1
∆G = ∆H - T∆S
For ∆H = -ve and ∆S = +ve, reaction will be spontaneous at all temperature (∆G <0)
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