Question

Nickel (II) sulfide ore can be roasted to produce sulfur dioxide, which can then be converted to sulfuric acid. What mass of sulfuric acid can be produced if you roast 46.3 grams of ore that is of 86.6 % nickel (II) sulfide?

Answer 1

Roasting means heating in presence of air

2NiS + 3O₂ ——->2 NiO +2 SO₂

mass of NiS in sample = 46.3 x 86.6/100 = 40.10 g

molarmass of NiS = 90.76 g/mol

Moles of NiS = 40.10g/90.76 g/mol = 0.442 mol

moles of SO₂ formed should be equal to moles of NiS = 0.442 mol

1 mole SO₂ produces 1 mol H₂SO₄

mass of sulphuric acid = 0.442 mol x 98g/mol = 43.30 g