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$$\ce{PbS(s) + 4 H2O2(aq) -> PbSO4(s) + 4 H2O(l)}$$

I been trying to find the half equations for a while now. How would you find the balanced half equations for this redox reaction? Do you just add water for the extra oxygens on the sulfate??? Assume acidic solution.

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  • $\begingroup$ That's a possible option. $\endgroup$ Jan 27 at 6:31

1 Answer 1

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The two half-equations are :

$\ce{PbS + 4 H2O -> PbSO4 + 8 H+ + 8e-}$

$\ce{H2O2 + 2 e^- + 2 H+ -> 2 H2O}$

Multiplying the second equation by $4$ and summing them gives :

$\ce{PbS + 4 H2O2 -> PbSO4 + 4 H2O}$

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