Solving Gas Law Question: Tire Pressure at 14°C & 2.2atm

In summary, the conversation discusses the calculation of the temperature of the air in a car tire after it has been driven on the highway. It is mentioned that the tire pressure increases from 2.0atm to 2.2atm, despite the air temperature remaining at 14 degrees celsius. The conversation also references various gas laws, such as Charles' Law and Boyle's Law, and the unit of pressure, atm, which is equivalent to approximately 1.013 x 10^5 Pa. The speaker asks for assistance in solving the problem, and it is mentioned that 1 kPa is equal to 1000 Pa. It is noted that this conversion is not necessary for solving the problem. The speaker also
  • #1
iluvu
2
0
The question given were:

The tire pressure for a car that has not been driven is 2.0atm when sitting outside at 14 degrees celsius. After the car was on the highway the temperature of the tire increased even though the air temperature remained at 14 degrees celsius. The tire pressure increased to 2.2atm. Calculate the temperature of the air in the tire in degrees celsius.

The gas laws that the teacher ever told us is

charles law: V1/T1=V2/T2
Bogle's law is P1V1=P2/V2 and
Combine law, which is V1*P1/T1=V2*P2/T2

But in the question, there is atm...which stands for Atmosphere...I know that Atomosphere is a unit of pressure, but isn't the unit for pressure (kPa)?

I'm so stuck...=( someone please help me...
 
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  • #2
1 atm is approximately [tex]1.013 \times 10^5 Pa[/tex]. But you do not need to perform this conversion to solve the problem because this factor will eventually cancel off.

What quantities remain the same before and after the car was driven?
 
Last edited:
  • #3
1 kPa is 1000 Pa
 

FAQ: Solving Gas Law Question: Tire Pressure at 14°C & 2.2atm

What is the ideal gas law and how does it apply in this scenario?

The ideal gas law, also known as the universal gas law, is a fundamental equation that relates the pressure, volume, temperature, and amount of gas in a system. It states that PV = nRT, where P is the pressure, V is the volume, n is the number of moles of gas, R is the gas constant, and T is the temperature in Kelvin. In this scenario, we can use the ideal gas law to determine the final tire pressure at a given temperature and initial pressure.

How do I convert temperature from Celsius to Kelvin?

To convert Celsius to Kelvin, you simply add 273.15 to the Celsius temperature. In this scenario, we would add 273.15 to 14°C to get 287.15K.

What is the relationship between temperature and pressure in the ideal gas law?

According to the ideal gas law, temperature and pressure are directly proportional. This means that as temperature increases, pressure also increases, and vice versa. In this scenario, if the temperature is increased, the tire pressure will also increase.

What would happen to the tire pressure if the volume of the tire is decreased?

According to the ideal gas law, pressure and volume are inversely proportional. This means that as volume decreases, pressure increases, and vice versa. In this scenario, if the tire volume is decreased, the tire pressure will increase as well.

What other factors could affect the tire pressure in this scenario?

Other factors that could affect the tire pressure in this scenario could include the type of gas inside the tire, any leaks or changes in the tire's physical structure, and external factors such as changes in altitude or atmospheric pressure. Additionally, if the tire is not completely sealed or airtight, it could affect the pressure. It is important to consider all of these factors when solving gas law questions about tire pressure.

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