4. Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water according to the equation: CH(g) + H2O(g)→ CO(g)+ 3 H2(g) In a particular reaction, 25.5 L of methane gas (measured at a pressure of 732 torr and a temperature of 25°C) mixes with 22.8 L of water vapor (measured at a pressure of 702 torr and a temperature of 125°C). The reaction produces 26.2 L of hydrogen gas at STP. A. Determine the theoretical yield (Volume, L) of hydrogen gas (hint- calculate moles of each reactant and remember to use the limiting reactant to determine theoretical yield). B. Calculate the percent yield of the reaction. Table 1. Vapor Pressure of Water at Various Temperatures Temperature (°C) Vapor Pressure (torr) 24.0 22.4 24.1 22.5 24.2 22.6 24.3 22.8 24.4 22.9 24.5 23.1
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.
![### Hydrogen Gas Production by Methane-Water Reaction
Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water according to the equation:
\[ \text{CH}_4(g) + \text{H}_2\text{O}(g) \rightarrow \text{CO}(g) + 3 \text{H}_2(g) \]
In a particular reaction, 25.5 L of methane gas (measured at a pressure of 732 torr and a temperature of 25°C) mixes with 22.8 L of water vapor (measured at a pressure of 702 torr and a temperature of 125°C). The reaction produces 26.2 L of hydrogen gas at STP.
**Tasks:**
**A.** Determine the theoretical yield (Volume, L) of hydrogen gas. (Hint: Calculate moles of each reactant and remember to use the limiting reactant to determine theoretical yield).
**B.** Calculate the percent yield of the reaction.
### Table 1. Vapor Pressure of Water at Various Temperatures
| Temperature (°C) | Vapor Pressure (torr) |
|-----------------|-----------------------|
| 24.0 | 22.4 |
| 24.1 | 22.5 |
| 24.2 | 22.6 |
| 24.3 | 22.7 |
| 24.4 | 22.8 |
| 24.5 | 22.9 |
The table lists the vapor pressure of water at various temperatures, providing crucial data for calculations involving gas laws and reaction conditions.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6501bcec-69f0-41c7-aaf6-9d4563ecc7cd%2Fdd03c02d-05e5-4611-88d5-daae93478706%2F8vt065a_processed.jpeg&w=3840&q=75)
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