[References) Use the References to access important values if needed for this question. How many grams of iron are needed to completely consume 10.2 L of chlorine gas according to the following reaction at 25 °C and 1 atm? iron (s) + chlorine (g)-iron(III) chloride (s) grams iron Submit Answer Retry Entire Group 9 more group attempts remaining
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 Problem
#### Objective
Determine the mass of iron required to completely react with 10.2 liters of chlorine gas according to the given chemical equation at 25°C and 1 atm.
#### Chemical Equation
\[ \text{iron (s)} + \text{chlorine (g)} \rightarrow \text{iron(III) chloride (s)} \]
#### Solution Steps
1. **Identify Reactants and Products:**
- **Iron (Fe):** Solid reactant
- **Chlorine (Cl\(_2\)):** Gaseous reactant
- **Iron(III) chloride (FeCl\(_3\)):** Solid product
2. **Volume of Chlorine Gas:**
- Given: 10.2 L
3. **Determine Moles of Chlorine Gas:**
- Use Ideal Gas Law and molar volume (22.4 L/mol at STP for gases):
\[
\text{Moles of Cl\(_2\)} = \frac{10.2 \, \text{L}}{22.4 \, \text{L/mol}}
\]
4. **Stoichiometry:**
- Use balanced equation to calculate the moles of iron needed.
5. **Calculate Mass of Iron:**
- Use the molar mass of iron to convert from moles to grams.
#### User Interaction
- **Input Field:** Enter the computed grams of iron.
- **Buttons:**
- *Submit Answer*: Validate your response.
- *Retry Entire Group*: Try the problem again if needed.
#### Attempts
- Up to 10 attempts available for answering.
---
This structured approach aims to help students practice application of stoichiometry principles in chemical reactions.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F18395f57-75e3-4bdb-980a-ed8850989594%2F96f3676f-385e-4fa0-8b19-dca28cf18fe8%2F5qludh5_processed.jpeg&w=3840&q=75)
![**Question:**
What volume of chlorine gas is required to react completely with 0.375 mol of phosphorus (P₄) according to the following reaction at 0°C and 1 atm?
\[ \text{phosphorus (P}_4\text{)} (s) + \text{chlorine} (g) \rightarrow \text{phosphorus trichloride} (l) \]
**Answer Box:**
\[ \text{Volume =} \, \_\_\_\_ \, \text{L} \]
**Options:**
- Submit Answer
- Retry Entire Group
**Additional Information:**
There are 8 more group attempts remaining.
**Navigation:**
- Previous
- Next
---
This question requires you to calculate the volume of chlorine gas needed for the complete reaction with phosphorus at specified conditions of temperature and pressure. Here, using the ideal gas law and stoichiometry might be necessary to find the exact volume in liters.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F18395f57-75e3-4bdb-980a-ed8850989594%2F96f3676f-385e-4fa0-8b19-dca28cf18fe8%2Fvhdgsm9_processed.jpeg&w=3840&q=75)
Given,
(i) The reaction:
Iron (s) + Chlorine (g ) format('truetype')%3Bfont-weight%3Anormal%3Bfont-style%3Anormal%3B%7D%3C%2Fstyle%3E%3C%2Fdefs%3E%3Ctext%20font-family%3D%22math12bba9f4124283edd644799e0ce%22%20font-size%3D%2216%22%20text-anchor%3D%22middle%22%20x%3D%2210.5%22%20y%3D%2216%22%3E%26%23x2192%3B%3C%2Ftext%3E%3C%2Fsvg%3E)
Iron (III) chloride
volume of chlorine gas = 10.2 L
pressure = 1 atm
temperature = 25 oC
(ii) Phosphorus ( P4 ) (s) + Chlorine ( g ) Phosphorus trichloride (l)
moles of P4 = 0.375 mol
temperature = 0 oC
pressure = 1 atm
Step by step
Solved in 4 steps with 4 images
