This question is about iron and some of its compounds.
Complete the table to show the numbers of subatomic particles in 56Fe2+.
Number of protons | Number of neutrons | Number of electrons |
A sample of iron contains the following isotopes.
Isotope | Percentage abundance |
54Fe | 5.84 |
56Fe | 91.68 |
57Fe | 2.17 |
58Fe | 0.31 |
Calculate the relative atomic mass of this sample of iron.
Give your answer to three significant figures.
Magnesium reacts with aqueous iron(II) sulfate in a displacement reaction.
Write the ionic equation for this reaction.
Include state symbols.
25.00 g of a compound contains 6.98 g of iron and 6.03 g of sulfur.
The remaining mass is oxygen.
Calculate the empirical formula of this compound.
[Ar values: O = 16.0 S = 32.1 Fe = 55.8]
When 6.95 g of FeSO4•xH2O is heated, 2.00 g of iron(III) oxide, 0.80 g of sulfur dioxide and 1.00 g of sulfur trioxide are produced.
The only other product is water.
Deduce the overall equation for the reaction using these data.
State symbols are not required.
You must show your working.
[Ar values: H = 1.0 O = 16.0 S = 32.1 Fe = 55.8]
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