what mass of iron sulfate would be needed to provide 28g of iron
what mass of iron sulfate would be needed to provide 28g of iron
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what mass of iron sulfate would be needed to provide 28g of iron
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by cxllum210what mass of iron sulfate would be needed to provide 28g of iron
You need to specify which sulphate of iron you are making. Iron(II) sulphate (FeSO4.xH2O) and iron(III) sulphate (Fe2(SO4)3.xH2O) will form in different masses and you also need to be aware of the hydration state of the salt you are making.
For simplicity, let’s assume this is a GCSE question and you are making anhydrous iron(II) sulphate (e.g x = 0, so FeSO4 which has a molar mass of approximately 152 g/mol).
Can you start by writing an equation for the reaction of anhydrous iron(II) sulphate and a suitable reducing agent (let’s say magnesium, Mg) to make iron (Fe, molar mass = 56 g/mol) and MgSO4?
(edited 1 year ago)
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