The element oxygen was prepared by Joseph Priestley in 1774 by heating mercury(II) oxide: HgO(s) → Hg(l) ½O2(g), ΔH° = 90.84 kJ/mol.Estimate the temperature at which this reaction will become spontaneous under standard state conditions.S°(Hg) = 76.02 J/K • molS°(O2) = 205.0 J/K • molS°(HgO) = 70.29 J/K • mol

SOLVED:Joseph Priestley discovered oxygen in 1774 by heating "red calx of mercury" [mercury(II) oxide]. The calx decomposed to its elements. The equation is HgO ⟶Hg O2 (not balanced) What mass of oxygen is produced by the decomposition of 18.0  g HgO ?

#OnThisDay Joseph Priestley discovered oxygen here at Bowood House! On 1st August 1774, Priestley discovered what he called ‘dephlogisticated air’ after burning the ash left behind from heating mercury. Upon heating the ash, he saw globules of quicksilver forming and a colourless air rising from it. He noted ‘But what surprised me more than I can well express’, he wrote, ‘was that a candle burned in this air with a remarkably vigorous flame’. The more you know! 🧪🔬 | Bowood House & Gardens

Joseph Priestley's discovery of oxygen involved the unbalanced ... | Filo

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