For the unbalanced reaction: FeSO4

(s) → Fe
2O3
(s) + SO2
(g) + O2
(g) ; how many total moles
of gas are produced from the decomposition of 9.98 mol FeSO4
(s)?

Balance the equation first.

4FeSO4(s) ==> 2Fe2O3(s) + 4SO2(g) + O2(g)
9.98mols FeSO4 x [(5 mols SO2+O2)/4 mols FeSO4] = 9.98 x 5/4 = ?

To determine the number of moles of gas produced from the decomposition of FeSO4, we need to first balance the chemical equation. The given unbalanced equation is:

FeSO4(s) → Fe2O3(s) + SO2(g) + O2(g)

The subscript next to Fe in Fe2O3 indicates that there are 2 moles of Fe for every 1 mole of Fe2O3. Therefore, we can rewrite the balanced equation as:

FeSO4(s) → 1 Fe2O3(s) + SO2(g) + O2(g)

Now, let's calculate the number of moles of each substance produced from the decomposition of 9.98 mol FeSO4.

From the balanced equation, we can see that for every 1 mole of FeSO4 decomposed, we get 1 mole of Fe2O3, 1 mole of SO2, and 1 mole of O2. Therefore, the total number of moles of gas produced is equal to the sum of moles of SO2 and O2.

So, for every 1 mole of FeSO4, we get a total of 2 moles of gas (1 mole of SO2 + 1 mole of O2).

To find the number of moles of gas produced from 9.98 mol of FeSO4, we can multiply the number of moles of gas produced per mole of FeSO4 (2 moles/mol) by the given number of moles:

Total moles of gas = 2 moles/mol × 9.98 mol = 19.96 mol

Therefore, the total number of moles of gas produced from the decomposition of 9.98 mol FeSO4 is approximately 19.96 moles.