. A sample of 1.0 g of solid Fe2O3 of 80 % purity is dissolved in a moderately concentrated HCl solution which is reduced by zinc dust. The resulting solution required 16.7 mL of a 0.1 M solution of the oxidant. Calculate the number of electrons taken up by the oxidant.

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Vikas TU · Answer

moles of Fe in Fe2O3 would be => (0.8/160)*2 => 0.01 Now to react after zinc dust the moles required would be: 0.01*2 = 0.1*16.7*10^-3*v.f v.f = 12 elctrons approx.

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. A sample of 1.0 g of solid Fe2O3 of 80 % purity is dissolved in a moderately concentrated HCl solution which is reduced by zinc dust. The resulting solution required 16.7 mL of a 0.1 M solution of the oxidant. Calculate the number of electrons taken up by the oxidant.

. A sample of 1.0 g of solid Fe2O3 of 80 % purity is dissolved in a moderately concentrated HCl solution which is reduced by zinc dust. The resulting solution required 16.7 mL of a 0.1 M solution of the oxidant. Calculate the number of electrons taken up by the oxidant.

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. A sample of 1.0 g of solid Fe2O3 of 80 % purity is dissolved in a moderately concentrated HCl solution which is reduced by zinc dust. The resulting solution required 16.7 mL of a 0.1 M solution of the oxidant. Calculate the number of electrons taken up by the oxidant.

. A sample of 1.0 g of solid Fe2O3 of 80 % purity is dissolved in a moderately concentrated HCl solution which is reduced by zinc dust. The resulting solution required 16.7 mL of a 0.1 M solution of the oxidant. Calculate the number of electrons taken up by the oxidant.

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