Hydrogen produced from a hydrolysis reaction was collected over water. The data is compiled in the table. Total volume of H₂(g) collected 96.17 mL Temperature 27.0 °C Barometric pressure 738 mmHg Vapor pressure of water at 27.0 °C 27.0 mmHg Calculate the moles of hydrogen gas produced by the reaction. moles: mol H₂
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.
![### Calculation of Moles of Hydrogen Gas Produced from Hydrolysis Reaction
Hydrogen produced from a hydrolysis reaction was collected over water. The data is compiled in the table below:
| | |
|---------------------------------|----------------------------------|
| **Total volume of H₂(g) collected** | 96.17 mL |
| **Temperature** | 27.0 °C |
| **Barometric pressure** | 738 mmHg |
| **Vapor pressure of water at 27.0 °C** | 27.0 mmHg |
**Task:**
Calculate the moles of hydrogen gas produced by the reaction.
**Formula:**
To calculate the moles of hydrogen gas (n), you can use the Ideal Gas Law equation:
\[ PV = nRT \]
Where:
- \( P \) is the pressure of the gas (in atm)
- \( V \) is the volume of the gas (in liters)
- \( n \) is the number of moles of the gas
- \( R \) is the ideal gas constant (0.0821 L·atm/(mol·K))
- \( T \) is the temperature (in Kelvin)
**Data given:**
- Total volume of H₂(g) collected = 96.17 mL = 0.09617 L (converted to liters)
- Temperature = 27.0 °C = 300.15 K (converted to Kelvin)
- Barometric pressure = 738 mmHg
- Vapor pressure of water at 27.0 °C = 27.0 mmHg
**Steps:**
1. **Calculate the partial pressure of H₂ gas:**
\[
P_{H₂} = \text{Barometric pressure} - \text{Vapor pressure of water}
\]
\[
P_{H₂} = 738 \, \text{mmHg} - 27.0 \, \text{mmHg} = 711 \, \text{mmHg}
\]
Convert mmHg to atm:
\[
P_{H₂} = 711 \, \text{mmHg} \times \frac{1 \, \text{atm}}{760 \, \text{mmHg}} \approx 0.9355 \, \text{atm}
\]
2. **Apply the Ideal Gas](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5c433f37-c484-4136-9ada-41e91862a98c%2Fab44dabd-5547-419f-af92-56f22dbe4049%2Fbvlrjom_processed.png&w=3840&q=75)
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