The standard enthalpies of formation of PbS(s), SO2(g) and PbO(s) are -98.3, -296.8. and -217.3kj mol...

The standard enthalpies of formation of PbS(s), SO2(g) and PbO(s) are -98.3, -296.8. and -217.3kj mol respectively.

Calculate the reaction enthalpy for the roasting of PbS(s).

PbS(s)+3O2(g)--->2SO2(g)+2PbO(s)

Expert Solution

Balanced reaction is

2PbS_(s) + 3O_2(g) 2SO_2(g) + 2PbO_(s)

H⁰ = _fH⁰ (Product) - _fH⁰ (Reactant)

H⁰ = [(2_fH⁰ SO₂) + (2_fH⁰ PbO)] - [(2_fH⁰ PbS) + (3_fH⁰ O₂)]

= [(2(-296.8)) + (2 (-217.3))] - [(2(-98.3)) + (3 (0))]

= [-1028.2] - [-196.6]

= [-1028.2] + [196.6]

H⁰ = -831.6 KJ/mol

reaction enthalpy for the roasting of PbS_(s) = -831.6 KJ/mol

queen_honey_blossom answered 2 years ago

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