A balloon is filled with 3.00L of helium at a pressure of 765 torr. What is the volume of the balloon at an altitude where the pressure is 530 torr if the temperature remains constant? O 0.231L O2.08L O 1.00L O 4.33L
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.
![### Gas Laws in Action: Solving Volumetric Changes of a Helium Balloon
A balloon is filled with 3.00L of helium at a pressure of 765 torr. What is the volume of the balloon at an altitude where the pressure is 530 torr if the temperature remains constant?
#### Options:
- \( \circ \) 0.231L
- \( \circ \) 2.08L
- \( \circ \) 1.00L
- \( \circ \) 4.33L
#### Explanation:
This problem can be solved using **Boyle's Law**, which states that for a given mass of gas at constant temperature, the volume of the gas varies inversely with pressure. Mathematically, it is represented as:
\[ P_1 V_1 = P_2 V_2 \]
Where:
- \( P_1 \) is the initial pressure
- \( V_1 \) is the initial volume
- \( P_2 \) is the final pressure
- \( V_2 \) is the final volume
Given:
- \( P_1 = 765 \, \text{torr} \)
- \( V_1 = 3.00 \, \text{L} \)
- \( P_2 = 530 \, \text{torr} \)
We need to find \( V_2 \), the final volume of the balloon.
Rearranging the equation to solve for \( V_2 \):
\[ V_2 = \frac{P_1 V_1}{P_2} \]
Substitute the known values:
\[ V_2 = \frac{765 \, \text{torr} \times 3.00 \, \text{L}}{530 \, \text{torr}} \]
\[ V_2 = \frac{2295}{530} \]
\[ V_2 \approx 4.33 \, \text{L} \]
Therefore, the correct answer is:
- \( \circ \) 4.33L](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc7392a9d-ee4e-4113-86f6-910a06062102%2F40a324ed-90ca-4b49-8543-1bc4cca477e5%2Fz11h57n_processed.jpeg&w=3840&q=75)
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