Consider the following balanced chemical reaction: 2H₂ +02 → 2H₂O How many liters of oxygen gas (0₂) are needed to produce 43.2 liters of water at STP? O A. 0.51 liters 0₂ OB. 10.5 liters 02 O c. 21.6 liters 02 OD. 86.4 liters 02
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.
![### Balanced Chemical Reaction and Stoichiometry Question
Consider the following balanced chemical reaction:
\[ 2H_2 + O_2 \rightarrow 2H_2O \]
The problem is:
**How many liters of oxygen gas (O\(_2\)) are needed to produce 43.2 liters of water at STP (Standard Temperature and Pressure)?**
### Multiple Choice Options:
A. 0.51 liters \( O_2 \)
B. 10.5 liters \( O_2 \)
C. 21.6 liters \( O_2 \)
D. 86.4 liters \( O_2 \)
### Explanation of the Balanced Equation:
The given balanced chemical equation shows that two molecules of hydrogen gas (\(H_2\)) react with one molecule of oxygen gas (\(O_2\)) to produce two molecules of water (\(H_2O\)). This reaction is in a 2:1:2 molar ratio. At STP, the volume of gases can be directly related to their molar ratios.
### Problem-Solving Approach:
1. Determine the molar ratio of \( O_2 \) to \( H_2O \) from the balanced chemical equation: \( 1 \text{ mole of } O_2 \) produces \( 2 \text{ moles of } H_2O \).
2. Using the molar ratio, calculate the volume of \( O_2 \) needed to produce 43.2 liters of \( H_2O \).
**Note:** 1 mole of any gas at STP occupies 22.4 liters.
By understanding these steps and concepts, you should be able to solve the problem accurately.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F590bcdfe-2834-4ce5-a4ca-671e0b630a2f%2F2f3fa64c-87b3-4540-84b7-8c7c4431e023%2Fqqkn7yi_processed.jpeg&w=3840&q=75)
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