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Iron tablets' usually contain iron sulphate (FeSO4).
This salt can be made by reacting iron with sulphuric acid.
Fe +
H2SO4 →
FeSO4 + H2
Calculate the mass of iron sulphate that could be obtained from 4 g of iron.
(Relative atomic masses: Fe = = 56, H = 1, O = 16, S = 32)

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Answer:The atomic weight is the lower number on each chemical. Fe has a mass of 56, S a mass of 32 and O a mass of 16. As there are four oxygens present in this compound, you multiply 16 by 4 to get 64. Lastly you add all these separate masses together, which gives a total relative mass of 152.

Explanation:

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The mass of iron sulfate that could be obtained from 4 g of iron is 10.79 grams.

What is the relation between mass & moles?

Moles of any substance from mass will be calculated by using the below equation as:

n = W/M, where

W = given mass

M = molar mass

Moles of Fe = 4g / 56g/mol = 0.071 mol

From the stoichiometry of the reaction it is clear that equal moles of iron sulfate will be generated by same moles of iron.

0.071 moles of Fe = produces 0.071 moles of FeSO₄

Mass of FeSO₄ = (0.071mol)(152g/mol) = 10.79g

Hence obtained mass of FeSO₄ is 10.79g.

To know more about mass & moles, visit the below link:
https://brainly.com/question/21182981

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