Chemistry

From the equation : C + 2H₂SO₄ ⟶ CO₂ + 2H₂O + 2SO₂
Calculate :
(i) The mass of carbon oxidized by 49 g of sulphuric acid [C = 12 ; relative molecular mass of H₂SO₄ = 98].
(ii) The volume of SO₂ measured at s.t.p., liberated at the same time.

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$\underset{12 \text{g}}{\text{C}} + \underset{2(98) = 196 \text{ g}}{2\text{H}$

(i) 196 g of sulphuric acid oxidizes 12 g carbon

∴ 49 g of sulphuric acid will oxidize = $\dfrac{12}{196}$ x 49 = 3 g

Hence, 3 g of carbon is oxidized.

(ii) 12 g carbon liberates 2 vol = (2 x 22.4) lit of SO₂

∴ 3 g of carbon will liberate $\dfrac{2 \times 22.4}{12}$ x 3 = 11.2 lit of SO₂.

Hence, 11.2 lit of SO₂ is liberated.

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