Question

If we burn 1.5 g of iron, how many grams of iron (III) oxide will be produced? The equation is 4Fe (s) + 3 O2 (g) ==> 2 Fe2O3

Answer 1

Answer:

weight of iron = 1.5 g

atomic weight of iron = 56 g/mol

so, no of moles of iron = 1.5/56 = 0.027 mol

The equation is 4Fe + 3O₂ => 2Fe₂O₃

from equation, it is clear that 4 moles of iron produce 2 moles of iron(III) oxide.

so, 0.027 mole of iron will produce 2/4 × 0.027 = 0.0135 mol of iron (III) oxide.

mass of iron (III) oxide = mole × molecular weight of Fe₂O₃

= 0.0135 mol × (56 × 2 + 16 × 3)

= 0.0135 × (112 + 48)

= 0.0135 × 160

= 2.16 grams.

Therefore mass of iron(III) oxide is 2.16 grams.

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sulphur trioxide is prepared by the following two reactions :

S8(s) + 8O2(g) --> 8SO2(g)

2SO2(g) + O2(g) --> 2SO3(g)

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