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Scorpion4ik [409]
3 years ago
12

3. In the formation of acid rain, sulfur dioxide reacts with oxygen and water in the air to form sulfuric acid. Write a balanced

chemical equation for the reaction. If 2.50 g sulfur dioxide react with excess oxygen gas and water, how many grams of sulfuric acid are produced
Chemistry
1 answer:
Andreyy893 years ago
4 0

Answer:

SO₂ + 0.5 O₂ + H₂O → H₂SO₄

3.83 g

Explanation:

In the formation of acid rain, sulfur dioxide reacts with oxygen and water in the air to form sulfuric acid. The balanced chemical equation is:

SO₂ + 0.5 O₂ + H₂O → H₂SO₄

The molar mass of SO₂ is 64.07 g/mol. The moles of SO₂ corresponding to 2.50 g are:

2.50 g × (1 mol/64.07 g) = 0.0390 mol

The molar ratio of SO₂ to H₂SO₄ is 1:1. The moles of H₂SO₄ formed are 0.0390 moles.

The molar mass of H₂SO₄ is 98.08 g/mol. The mass of H₂SO₄ is:

0.0390 mol × 98.08 g/mol = 3.83 g

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Answer:

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V₂ = 5.55 L

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7 0
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What mass of CaSO3 must have been present initially to produce 14.5 L of SO2 gas at a temperature of 12.5°C and a pressure of 1.
german
When the reaction equation is:

CaSO3(s) → CaO(s) + SO2(g)

we can see that the molar ratio between CaSO3 & SO2 is 1:1 so, we need to find first the moles SO2.

to get the moles of SO2 we are going to use the ideal gas equation:

PV = nRT

when P is the pressure =  1.1 atm

and V is the volume = 14.5 L 

n is the moles' number (which we need to calculate)

R ideal gas constant = 0.0821

and T is the temperature in Kelvin = 12.5 + 273 = 285.5 K

so, by substitution:

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when mass = moles * molar mass

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