STARTING AMOUNT X What volume in liters of CH₂OH gas are formed when 3.20 L of H gas are completely reacted at STP according to the following chemical reaction? Remember 1 mol of an ideal gas has a volume of 22.4 L at STP. CO(g) + 2 H₂(g) → CH₂OH(g)
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.
![### Chemical Reaction Volume Calculation at STP
**Problem Statement:**
What volume in liters of CH₃OH gas is formed when 3.20 L of H₂ gas are completely reacted at STP according to the following chemical reaction?
\[ \text{CO(g)} + 2 \text{H}_2\text{(g)} \rightarrow \text{CH}_3\text{OH(g)} \]
**Key Information:**
- 1 mol of an ideal gas has a volume of 22.4 L at STP.
**Calculation Setup:**
\[ \text{Starting Amount} \times \left( \frac{\text{Conversion Factor}}{\text{Molar Ratio}}\right) \]
1. **Starting Amount**: The given starting volume is 3.20 L of H₂.
2. **Conversion Factor**:
- This relates the volume of H₂ to moles, using the molar volume of an ideal gas (22.4 L/mol).
3. **Molar Ratio**:
- From the balanced chemical equation, the molar ratio of H₂ to CH₃OH is 2:1.
**Visual Explanation:**
- The diagram below the problem statement has two main parts:
- **Left Box** ("Starting Amount"): Represents the initial volume of H₂ gas (3.20 L).
- **Right Parenthesis**: Represents the calculation using conversion factor and molar ratio:
- Top row inside the parenthesis is for the initial volume and conversion to moles.
- Bottom row is for applying the molar ratio to find the volume of CH₃OH produced.
The solution involves calculating the theoretical yield of CH₃OH gas based on the stoichiometry of the reaction and the known properties of ideal gases at standard temperature and pressure.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F31f59ff4-c1b6-4bfe-b48e-f376b2b8e1ed%2F5fa68806-9ef2-401a-9056-7131f60a6052%2Fn9ixeyg_processed.png&w=3840&q=75)
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