Ammonia, NH3(g), and hydrogen chloride, HCl(g), react to form solid ammonium chloride, NH4Cl(s): NH3 (9) + HCl (g) → NH4Cl (s) Two 3.00 L flasks at 20.0 °C are connected by a stopcock, as shown in the drawing . One flask contains 6.00gNH3(g), and the other contains 5.00 g HCl(g). When the stopcock is opened, the gases react until one is completely consumed. Part B NH3(g) Pfinal HCI(g) What will be the final pressure of the system after the reaction is complete? (Neglect the volume of the ammonium chloride formed.) VE ΑΣΦ = 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.
I'm having trouble understanding both questions
![**Part C**
**What mass of ammonium chloride will be formed?**
\[
m_{\text{NH}_4\text{Cl}} = \_\_\_\_\_\_\_\_\_ \, \text{g}
\]
This section includes an input box where users can enter the calculated mass of ammonium chloride in grams. The interface provides options for formatting and entering text or equations, as indicated by icons, such as equation tools and keyboard input settings. There are no graphs or diagrams associated with this text.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fcb45a7b7-d1aa-4ac7-ad98-90aa0325071f%2F7f02dc01-6e69-4793-8b03-6d20ff05ca1f%2Fb4spagr_processed.png&w=3840&q=75)
![**Ammonia, NH₃(g), and hydrogen chloride, HCl(g), React to Form Solid Ammonium Chloride, NH₄Cl(s):**
\[ \text{NH}_3 \, (g) + \text{HCl} \, (g) \rightarrow \text{NH}_4\text{Cl} \, (s) \]
Two 3.00 L flasks at 20.0 °C are connected by a stopcock, as shown in the drawing.
- **Setup Description:**
- The left flask contains 6.00 g of NH₃(g).
- The right flask contains 5.00 g of HCl(g).
**Process:**
- When the stopcock is opened, the gases react until one is completely consumed.
**Part B Question:**
- What will be the final pressure of the system after the reaction is complete? (Neglect the volume of the ammonium chloride formed.)
**Diagram Details:**
- The image shows two spherical flasks connected by a pipe with a stopcock in the middle.
- The left flask is labeled "NH₃(g)" and the right flask is labeled "HCl(g)".
**Final Pressure Calculation:**
- \( P_{\text{final}} = \) _____ atm](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fcb45a7b7-d1aa-4ac7-ad98-90aa0325071f%2F7f02dc01-6e69-4793-8b03-6d20ff05ca1f%2Fo4kzv1p_processed.png&w=3840&q=75)
we have to calculate the final pressure and mass of ammonium chloride formed
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