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Calculate the oxidation number of the underlined element in the following molecules. H_(2)ul(S)O_(4) |
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Answer» Solution :`H_(2)SO_(4)` Suppose the oxidation number of S in `H_(2)SO_(4)` is x. The oxidation number of each H atom is +1 while that of each O atom is-2. Since`H_(2)SO_(4)` is a NEUTRAL molecule, the SUM of oxidation NUMBERS of all atoms must be EQUAL to zero. Therefore, we have `(+1)xx2(x)+(-2)xx4=0` or `+2+(x)-8=0orx=+8-2=+6` HENCE the oxidation number of S in `H_(2)SO_(4)` is +6. |
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