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.
![**Question 4 of 22**
Write a balanced chemical equation based on the following description: butanoic acid, C₃H₇COOH(l) burns in air.
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**Explanation:**
The prompt asks for the chemical reaction when butanoic acid burns in air, which typically involves a combustion reaction. In a combustion reaction, a substance reacts with oxygen (O₂) to produce carbon dioxide (CO₂) and water (H₂O).
Steps to balance the equation:
1. Write the unbalanced equation:
\[ \text{C}_3\text{H}_7\text{COOH(l)} + \text{O}_2(g) \rightarrow \text{CO}_2(g) + \text{H}_2\text{O}(l) \]
2. Balance carbon atoms:
\[ \text{C}_3\text{H}_7\text{COOH(l)} + \text{O}_2(g) \rightarrow 4\text{CO}_2(g) + \text{H}_2\text{O}(l) \]
3. Balance hydrogen atoms:
\[ \text{C}_3\text{H}_7\text{COOH(l)} + \text{O}_2(g) \rightarrow 4\text{CO}_2(g) + 4\text{H}_2\text{O}(l) \]
4. Balance oxygen atoms:
- Total oxygen atoms needed on the product side: \(4 \times 2 (\text{from CO}_2) + 4 \times 1 (\text{from H}_2\text{O}) = 12\)
- Oxygen in butanoic acid: 2 (from C₃H₇COOH)
- Oxygen needed from O₂: \( \frac{10}{2} = 5 \)
5. Final balanced equation:
\[ \text{C}_3\text{H}_7\text{COOH(l)} + \frac{9}{2}\text{O}_2(g) \rightarrow 4\text{CO}_2(g) + 4\text{H}_2\text{O}(l) \]
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**Note:**
To avoid using fractional coefficients, multiply the entire equation by 2:
\[ 2\text{C}_3\text](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F46f39eb1-69b3-4ba7-b54b-af6952f33d23%2Fc9ea456e-9bab-4fdb-af6b-60466fc61730%2Fy3oqwop_processed.jpeg&w=3840&q=75)
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