Reaction of ozone with black lead sulphide
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This is a semi-standard example of why 'naive' balancing does not work.
Ozone is a source of atomic oxygen, producing free oxygen molecules. So, in 'mild' conditions only one oxygen per ozone molecule would react as a strong oxidizer, and the remaining molecular oxygen would require elevated temperatures to react. Thus the equation would be
PbS+4O3⟶PbSO4+4O2PbS+4OX3⟶PbSOX4+4OX2
Similarly, in excess of reducer at elevated temperature (though why would you want it with ozone is another matter) all atoms in ozone would react. Thus, the reaction should be
3PbS+4O3⟶3PbSO4
Ozone is a source of atomic oxygen, producing free oxygen molecules. So, in 'mild' conditions only one oxygen per ozone molecule would react as a strong oxidizer, and the remaining molecular oxygen would require elevated temperatures to react. Thus the equation would be
PbS+4O3⟶PbSO4+4O2PbS+4OX3⟶PbSOX4+4OX2
Similarly, in excess of reducer at elevated temperature (though why would you want it with ozone is another matter) all atoms in ozone would react. Thus, the reaction should be
3PbS+4O3⟶3PbSO4
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