Problem: An automobile tire has a maximum rating of 38.0 psi (gauge pressure).​The tire is inflated (while cold) to a volume of 11.8 L and a gauge pressure of 36.0 psi (Note: The  gauge pressure is the difference between the total pressure and atmospheric pressure. In this case, assume that atmospheric pressure is 14.7 psi.) at a temperature of 12.0 oC. While driving on a hot day, the tire warms to 65.0 oC and its volume expands to 12.2 L.​What is the total pressure (gauge pressure + atmospheric pressure) in the tire after warming on a hot day?

FREE Expert Solution

We have to calculate the total pressure of air inside a tire when it warmed on a hot day.


We will solve this problem through these steps:

Step 1: Calculate the total pressure of air inside the tire when cold.

Step 2: Make sure that the values given have consistent units.

Step 3: Use the ideal gas law to calculate the pressure of air in time after warming.

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Problem Details

An automobile tire has a maximum rating of 38.0 psi (gauge pressure).


The tire is inflated (while cold) to a volume of 11.8 L and a gauge pressure of 36.0 psi (Note: The  gauge pressure is the difference between the total pressure and atmospheric pressure. In this case, assume that atmospheric pressure is 14.7 psi.) at a temperature of 12.0 oC. While driving on a hot day, the tire warms to 65.0 oC and its volume expands to 12.2 L.

What is the total pressure (gauge pressure + atmospheric pressure) in the tire after warming on a hot day?


Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Chemistry Gas Laws concept. If you need more Chemistry Gas Laws practice, you can also practice Chemistry Gas Laws practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Ranasinghe's class at AMARILLO.