Suppose a student performed a similar experiment using pentane and hexane as his gases. Pentane Hexane Molar Mass 72.15 m (g/mol) na oniz Mass (g) 0.541d 340.646 100 Given the data in the figure above, which gas will occupy a larger volume at STP? 86.18 up samat elimi
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.
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### Experiment with Pentane and Hexane Gases
**Objective:**
This experiment aims to compare the volumes of pentane and hexane gases at standard temperature and pressure (STP) based on their molar masses and given masses.
#### Data Table
| | **Pentane** | **Hexane** |
|--------------|-------------|------------|
| **Molar Mass (g/mol)** | 72.15 | 86.18 |
| **Mass (g)** | 0.541 | 0.646 |
#### Key Concept:
Molar mass is the mass of one mole of a substance, measured in grams per mole (g/mol). Using the given mass and molar mass, we can determine the number of moles for each substance.
#### Calculation:
1. **Number of moles (n)** can be calculated using the formula:
\[
n = \frac{\text{mass (g)}}{\text{molar mass (g/mol)}}
\]
2. **Volume at STP (22.4 L/mol)**:
At standard temperature and pressure, one mole of any gas occupies 22.4 liters.
#### Steps:
1. Calculate the moles of pentane and hexane.
2. Use the volume at STP to find out which gas occupies a larger volume.
**Given the data in the figure above, which gas will occupy a larger volume at STP?**
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#### Graph/Diagram Explanation:
The table provides essential values for the molar masses and given masses for pentane and hexane. Use this data to perform calculations that will help identify which gas will occupy a larger volume under standard conditions.
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