Determine the volume of SO₂ (at STP) formed from the reaction of 96.7 g of FeS2 and 55.0 L of O₂ (at 398 K and 1.20 atm). 4 FeS₂(s) + 11 O2(g) →2 Fe₂O3(s) + 8 SO₂(g) O 27.6 L 18.1 L 45.3 L 36.1 L 32.9 L
Ideal and Real Gases
Ideal gases obey conditions of the general gas laws under all states of pressure and temperature. Ideal gases are also named perfect gases. The attributes of ideal gases are as follows,
Gas Laws
Gas laws describe the ways in which volume, temperature, pressure, and other conditions correlate when matter is in a gaseous state. The very first observations about the physical properties of gases was made by Robert Boyle in 1662. Later discoveries were made by Charles, Gay-Lussac, Avogadro, and others. Eventually, these observations were combined to produce the ideal gas law.
Gaseous State
It is well known that matter exists in different forms in our surroundings. There are five known states of matter, such as solids, gases, liquids, plasma and Bose-Einstein condensate. The last two are known newly in the recent days. Thus, the detailed forms of matter studied are solids, gases and liquids. The best example of a substance that is present in different states is water. It is solid ice, gaseous vapor or steam and liquid water depending on the temperature and pressure conditions. This is due to the difference in the intermolecular forces and distances. The occurrence of three different phases is due to the difference in the two major forces, the force which tends to tightly hold molecules i.e., forces of attraction and the disruptive forces obtained from the thermal energy of molecules.
![**Determining the Volume of Sulfur Dioxide (SO₂) at Standard Temperature and Pressure (STP)**
**Problem Statement:**
Calculate the volume of SO₂ (at STP) produced from the reaction of 96.7 grams of FeS₂ and 55.0 liters of O₂ (at 398 K and 1.20 atm).
**Chemical Reaction:**
\[ 4 \, \text{FeS}_2 (s) + 11 \, \text{O}_2 (g) \rightarrow 2 \, \text{Fe}_2\text{O}_3 (s) + 8 \, \text{SO}_2 (g) \]
**Options for the Volume of SO₂ Produced:**
- ○ 27.6 L
- ○ 18.1 L
- ○ 45.3 L
- ○ 36.1 L
- ○ 32.9 L
**Explanation of the Process:**
To solve this problem, one would need to:
1. **Convert the given mass of FeS₂ to moles.**
2. **Adjust the conditions to STP for the given volume of O₂ using the Ideal Gas Law.**
3. **Use stoichiometry based on the balanced chemical equation to find the moles of SO₂ produced.**
4. **Convert the moles of SO₂ to volume at STP using the molar volume of a gas (22.4 L/mol at STP).**
This process involves both stoichiometry and gas law calculations to determine the correct volume of SO₂ generated under standard conditions.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9b27e901-e87b-4228-8406-e843591659e6%2F3cc1729e-0f84-427c-9ec8-f86985dd2c7f%2Fj2qi5l7_processed.jpeg&w=3840&q=75)
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