Question

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)

Answer 1

Answer:

$m=7.07gH_{2}SO_{4}$

Explanation:

1. Take in account the sulfuric acid at STP:

$1840\frac{g}{L}$

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

$d=\frac{m}{V}$

Solving for m:

$m=\frac{V}{d}$

3. Replace values:

$m=\frac{1.30*10^{4}L}{1840\frac{g}{L}}$

$m=7.07gH_{2}SO_{4}$