Use the following data (in kJ/mol) to estimate ΔE for the reaction S -(g) + e- → S2-(g). Include an estimate of uncertainty. ΔEsub is the energy of sublimation.
2 Na(s) + S(s) → Na 2S(s) ΔE = -365 kJ/mol
2 K(s) + S(s) → K 2S(s) ΔE = -381 kJ/mol
2 Rb(s) + S(s) → Rb 2S(s) ΔE = -361 kJ/mol
2 Cs (s) + S(s) → Cs 2S(s) ΔE = -360 kJ/mol
S(s) → S(g) ΔE = 277 kJ/mol
S(g) + e - → S-(g) ΔE = -200 kJ/mol
Assume that all values are known to +1 kJ/mol.
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