7.50 L of water vapor at 50.2 °C and 0.121 atm reacts with excess iron, how many grams of iron(III) oxide will be produced? 2 Fe(s) + 3 H,O(g) – → Fe,O,(s) + 3 H,(g) 1.2125 nass: g Incorrect
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 and Calculation Problem**
**Problem Statement:**
If 7.50 L of water vapor at 50.2 °C and 0.121 atm reacts with excess iron, how many grams of iron(III) oxide will be produced?
**Chemical Equation:**
\[ \text{2 Fe(s) + 3 H}_2\text{O(g)} \rightarrow \text{Fe}_2\text{O}_3\text{(s) + 3 H}_2\text{(g)} \]
**Student Response:**
- Mass entered: 1.2125 g
- Feedback: Incorrect
**Explanation:**
This problem requires the use of stoichiometry and the ideal gas law to determine the mass of iron(III) oxide (\(\text{Fe}_2\text{O}_3\)) produced from a given volume of water vapor at specific temperature and pressure conditions. The student's response of 1.2125 g has been marked incorrect.
To solve this correctly, follow these general steps:
1. **Use the Ideal Gas Law:** Calculate the number of moles of water vapor (\(\text{H}_2\text{O}\)) using the formula \(PV = nRT\), where \(P\) is pressure, \(V\) is volume, \(n\) is number of moles, \(R\) is the ideal gas constant, and \(T\) is temperature in Kelvin.
2. **Convert Temperature:** First, convert the temperature from Celsius to Kelvin:
\[ T(K) = 50.2 + 273.15 = 323.35 \, \text{K} \]
3. **Calculate Moles of \(\text{H}_2\text{O}\):**
\[ n = \frac{PV}{RT} \]
Use \(R = 0.0821 \, \text{L} \cdot \text{atm}/(\text{mol} \cdot \text{K})\).
4. **Stoichiometry:**
Use the balanced chemical equation to find the ratio of moles of \(\text{H}_2\text{O}\) to moles of \(\text{Fe}_2\text{O}_3}\). From the equation:
\[ 3 \, \text{mol} \, \text{H}_](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2e1ea85c-702b-4278-9649-5b535ffa5734%2F8058ac4f-a53f-4f2b-8c8a-a36ccf213272%2Fj38xuxb_processed.png&w=3840&q=75)
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