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How much electricity is required in coulomb for the oxidation of (i) 1 mol of H_(2)O to O_(2) ? (ii) 1 mol of FeO to Fe_(2)O_(3) ? |
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Answer» Solution :(i) Calculation for REQUIRED ELECTRICITY for production of `O_(2)` from the oxidation of 1 mol `H_(2)O` : ACCORDING to following reaction `1/2` mol of `O_(2)` is produced from 1 mol of `H_(2)O`. `H_(2)O_((l)) to (1)/(2)O_(2(g))+2H^(+)+2e^(-)` 1 mol `H_(2)O to 1/2` mol of `O_(2)`, in this 2 mole `2e^(-)` is used. So, to produce `O_(2)` from 1 mol `H_(2)O` 2F electricity is required. So, `2F=2xx96500=193000` coulomb electricity. (ii) Calculation for required electricity for production of `Fe_(2)O_(3)` from oxidation of 1 mol of `FeO`: 1 mol of FeO gives following reaction to obtain `Fe_(2)O_(3)`. `underset((+2))(Fe)O to (1)/(2) underset((+3))(Fe_(2))O_(3)+underset(1mol)(e^(-))+H^(+)` So, oxidation of1mol FeO gives `1/2` mole of `Fe_(2)O_(3)` and in this reaction 1 mol ELECTRON =1F=96500 coloumb electricity is used. |
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