Water bottle in a hot car. In the American Southwest, the temperature in a closed car parked in sunlight during the summer can be high enough to burn flesh. Suppose a bottle of water at a refrigerator temperature of `5.00^@ C` is opened, then closed, and then left in a closed car with an internal temperature of `65.0^@ C`. Neglecting the thermal expansion of the water and the bottle, find the pressure in the air pocket trapped in the bottle. (The pressure can be enough to push the bottle cap past the threads that are intended to keep the bottle closed.)

Explanation

To solve the problem of finding the pressure in the air pocket trapped in a water bottle left in a hot car, we can use the ideal gas law and the concept of temperature and pressure relationships. Here’s a step-by-step solution:

### Step 1: Convert Temperatures to Kelvin
The initial temperature of the water in the bottle is given as \(5.00^\circ C\). To convert this to Kelvin:
\[ T_1 = 5.00 + 273.15 = 278.15 \, K \]

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