Problem: 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/mol2 Rb(s) + S(s) → Rb 2S(s)      ΔE = -361 kJ/mol2 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/molAssume that all values are known to +1 kJ/mol.

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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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