Consider the apparatus shown below. The valve is closed. the left bulb contains nitrogen gas and the right bulb hydrogen gas. N₂ H₂ 300 K 3.00 L 300 K 9.00 L 2.00 atm 2.00 atm When the valve is opened the two gases mix and react completely to form ammonia gas (NH3). The temperature remains constant. What is the pressure in the apparatus after the chemical reaction? 2.00 atm none of the answers are correct O 1.00 atm
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.
- **Left Bulb (N₂):**
- Temperature: 300 K
- Volume: 3.00 L
- Pressure: 2.00 atm
- **Right Bulb (H₂):**
- Temperature: 300 K
- Volume: 9.00 L
- Pressure: 2.00 atm
When the valve is opened, the two gases mix and react completely to form ammonia gas (NH₃). The temperature remains constant. What is the pressure in the apparatus after the chemical reaction?
**Options:**
1. 2.00 atm
2. None of the answers are correct
3. 1.00 atm
**Explanation:**
1. The initial state of the gases in separate bulbs indicates that both gases are at the same pressure (2.00 atm) and temperature (300 K) but occupy different volumes.
2. According to the balanced chemical equation for the formation of ammonia:
\[ N₂ + 3 H₂ \rightarrow 2 NH₃ \]
3. For every 1 mole of nitrogen, 3 moles of hydrogen react. Therefore, the limiting reagent must be determined:
- Moles of N₂: \( n(N₂) = \frac{P \cdot V}{R \cdot T} = \frac{2.00 \cdot 3}{0.0821 \cdot 300} = \frac{6}{24.63} \approx 0.244 \text{ moles} \)
- Moles of H₂: \( n(H₂) = \frac{2.00 \cdot 9}{0.0821 \cdot 300} = \frac{18}{24.63} \approx 0.73 \text{ moles} \)
Since 1 mole of N₂ requires 3 moles of H₂, to react with 0.244 moles of N₂, we need \(3 \cdot 0.244 = 0.732 \text { moles of H₂}\). Therefore, N₂ is the limiting reagent.
4. Using gas](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F464fe16a-00d5-4182-8379-61bd4b8bbe02%2F2d85179a-156c-4117-953c-394a94da69fd%2Fbgnmjlf_processed.png&w=3840&q=75)
Trending now
This is a popular solution!
Step by step
Solved in 2 steps with 1 images
