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Combustion of coal releases sulfur dioxide into the atmosphere. The following process converts this gas into sulfuric acid, a component of acid rain. 2SO2(g) + O2(g) → 2SO3(g) SO3(g) + H2O(l) → H2SO4(aq) If each tonne of coal produces 1.30 × 104 L of sulfur dioxide (measured at STP), what mass of sulfuric acid can result from combustion of each tonne of coal? (1 tonne = 1000 kg)

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Answer:

[tex]m=7.07gH_{2}SO_{4}[/tex]

Explanation:

1. Take in account the sulfuric acid at STP:

[tex]1840\frac{g}{L}[/tex]

2. Density is expressed as the ratio between the mass and the volume of a substance so:

[tex]d=\frac{m}{V}[/tex]

Solving for m:

[tex]m=\frac{V}{d}[/tex]

3. Replace values:

[tex]m=\frac{1.30*10^{4}L}{1840\frac{g}{L}}[/tex]

[tex]m=7.07gH_{2}SO_{4}[/tex]

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