6. For the following reaction – 2PbS(s) + 3O2(g) ? 2PbO(s) + 2SO2 a. What is being oxidized and what is being reduced? b. What is the oxidizing agent and what is the reducing agent? c. Give the oxidation number of each atom in the equation.
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- S has an oxidation state of -2 in PbS. - O has an oxidation state of -2 in PbO and -2 in SO2. Now, let's look at the reaction: 2PbS(s) + 3O2(g) → 2PbO(s) + 2SO2(g) We can see that PbS is being oxidized to PbO, which means that Pb is losing electrons and its Show more…
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