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Preparation of 1 kg of ferrous sulphate?

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If I were to produce 1 kg of ferrous sulphate through reaction of sulphuric acid and iron, in what quantities would two of those chemicals be needed

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  1. The reaction would be

    Fe + H2SO4 -----> FeSO4 + H2

    1 kg of FeSO4 would be equal to

    1 kg x 1000g/kg / 151.909 grams/mol = 6.58 moles of FeSO4

    Since the reaction requires an equal amount of Fe and H2SO4

    then you need

    6.58 moles Fe x 55.845 g/mol = 367.46 grams

    6.58 moles H2SO4 x 98.0836 g/mol = 645.39 grams

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