any drivers report low tire pressure at the start of winter when the temperature drops. If the pressure in a tire is 2.38 atm when the outside temperature is 294 K, what will the essure in the tire be if the outside temperature drops to 280. K? (Assume that the volume and atmospheric pressure remain constant.) A B 0.170 atm 2.27 atm
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.
![### Understanding Tire Pressure Changes with Temperature
**Scenario:**
Many drivers report low tire pressure at the start of winter when the temperature drops. Consider the following situation:
- The pressure in a tire is 2.38 atm when the outside temperature is 294 K.
- What will the pressure in the tire be if the outside temperature drops to 280 K?
**Assumptions:**
- The volume and atmospheric pressure remain constant.
**Options:**
- **A**: 0.170 atm
- **B**: 2.27 atm
- **C**: 2.50 atm
- **D**: 14.0 atm
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To solve problems like this, we use the ideal gas law in the form of the combined gas law, which relates pressure and temperature when volume is constant:
\[ \frac{P_1}{T_1} = \frac{P_2}{T_2} \]
Where:
- \( P_1 \) and \( P_2 \) are the initial and final pressures
- \( T_1 \) and \( T_2 \) are the initial and final temperatures (in Kelvin)
By plugging in the values:
- \( P_1 = 2.38 \) atm
- \( T_1 = 294 \) K
- \( T_2 = 280 \) K
You can solve for \( P_2 \) to find the final pressure in the tire.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5574c7aa-ac3d-4de1-a702-2eca5a8a3b7f%2F43072d05-8b7c-4b0c-b2a4-cc34e2aaeb3d%2Fe79oiu_processed.jpeg&w=3840&q=75)
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