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Alex17521 [72]
3 years ago
9

Combustion of coal releases sulfur dioxide into the atmosphere. The following process converts this gas into sulfuric acid, a co

mponent 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)
Chemistry
1 answer:
Usimov [2.4K]3 years ago
4 0

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}

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A solution made by mixing 20.0 g of a non-volatile compound with 125 mL of water at 25°C has a vapor pressure of 22.67 torr. What is the molecular weight (3sf) of the compound (g/mol).

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