An ore contains 80.0% by mass of FeS₂. A batch of 60.0 kg of the ore is roasted: 4 FeS₂ + 11 O₂ → 2 Fe₂O₃ + 8 SO₂, and 90.0% of the FeS₂ reacts this way (the rest stays unreacted and gives no SO₂). Next, 2 SO₂ + O₂ → 2 SO₃ converts 95.0% of the SO₂. All the SO₃ then reacts with water: SO₃ + H₂O → H₂SO₄. What mass of H₂SO₄ is formed, in kg, to the nearest integer? Atomic masses in g mol⁻¹: O 16.0, S 32.0, Fe 56.0, H 1.0.

ChemistryHardHigh School (11–12)Chemical Reactions › Chemical Equations Olympiad

An ore contains $80.0\%$ by mass of $\text{FeS}_2$ . A batch of $60.0\ \text{kg}$ of the ore is roasted: $4\,\text{FeS}_2 + 11\,\text{O}_2 \rightarrow 2\,\text{Fe}_2\text{O}_3 + 8\,\text{SO}_2$ , and $90.0\%$ of the $\text{FeS}_2$ reacts this way (the rest stays unreacted and gives no $\text{SO}_2$ ). Next, $2\,\text{SO}_2 + \text{O}_2 \rightarrow 2\,\text{SO}_3$ converts $95.0\%$ of the $\text{SO}_2$ . All the $\text{SO}_3$ then reacts with water: $\text{SO}_3 + \text{H}_2\text{O} \rightarrow \text{H}_2\text{SO}_4$ . What mass of $\text{H}_2\text{SO}_4$ is formed, in $\text{kg}$ , to the nearest integer? Atomic masses in $\text{g mol}^{-1}$ : O 16.0, S 32.0, Fe 56.0, H 1.0.

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← A solution at 298 K contains benzoic acid at 0.10 mol L⁻¹ (Ka = 6.4 × 10⁻⁵) and acetic acid at 0.20 mol L⁻¹ (Ka = 1.8 × 10⁻⁵). Both acids are weak, and each is only slightly ionised. What is the pH of the solution?Dinitrogen tetroxide partly breaks up: N₂O₄(g) ⇌ 2 NO₂(g). A sample of the equilibrium mixture has density 2.46 g L⁻¹ at 350 K and 1.00 atm. Take R = 0.0821 L atm K⁻¹ mol⁻¹ and treat the gases as ideal. What percentage of the N₂O₄ originally present has broken up, to the nearest integer? Atomic masses in g mol⁻¹: N 14.0, O 16.0. →

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