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ICSE Class 10 Chemistry Question 12 of 28

Stoichiometry — Percentage Composition — Empirical & Molecular Formula — Chemical Equations — Question 20

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20
Question

Question 1(2008)

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.

Answer

C12g+2H2SO42(98)=196 g⟶CO2+2H2O+2SO2\underset{12 \text{g}}{\text{C}} + \underset{2(98) = 196 \text{ g}}{2\text{H}_2\text{SO}_4} \longrightarrow \text{CO}_2 + 2\text{H}_2\text{O} + 2\text{SO}_2

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

∴ 49 g of sulphuric acid will oxidize = 12196\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 2×22.412\dfrac{2 \times 22.4}{12} x 3 = 11.2 lit of SO2.

Hence, 11.2 lit of SO2 is liberated.