If 4.0 g of O2 and 4.0 g of He are placed in a 7.86 L vessel at 16.56°C, what will be the partial pressure of Helium in the vessel? decimal places
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.
![**Chemistry Quiz: Partial Pressure of Helium**
Welcome to the Chemistry section of our educational platform. Below is a sample quiz question that will help you understand and calculate the partial pressures of gases in a mixture.
**Question:**
If 4.0 g of O₂ and 4.0 g of He are placed in a 7.86 L vessel at 16.56°C, what will be the partial pressure of Helium in the vessel? Provide your answer to 2 decimal places.
*Answer box:*
[_____________]
**Explanation:**
To solve this problem, you will use the ideal gas law equation:
\[ PV = nRT \]
Where:
- \( P \) is the pressure,
- \( V \) is the volume of the gas,
- \( n \) is the number of moles of the gas,
- \( R \) is the ideal gas constant (0.0821 L·atm·K⁻¹·mol⁻¹),
- \( T \) is the temperature in Kelvin.
**Step-by-Step Solution:**
1. **Convert grams to moles:**
- For O₂ (Molecular weight of O₂ = 32 g/mol):
\[ n_{O₂} = \frac{4.0 \text{ g}}{32 \text{ g/mol}} = 0.125 \text{ mol} \]
- For He (Molecular weight of He = 4 g/mol):
\[ n_{He} = \frac{4.0 \text{ g}}{4 \text{ g/mol}} = 1.0 \text{ mol} \]
2. **Convert the temperature from Celsius to Kelvin:**
\[ T = 16.56°C + 273.15 = 289.71 \text{ K} \]
3. **Use the ideal gas law to calculate the total pressure (P\(_\text{total}\)):**
Since the vessel contains a mixture of gases, we use Dalton’s Law, stating that the total pressure is the sum of the partial pressures:
\[ PV = (n_{O₂} + n_{He})RT \]
\[ P_{\text{total}} \cdot V = (0.125 + 1.0) \cdot 0.0821 \cdot 289.71 \]
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