Hikers noticed that a sealed bag of potato chips puffs up when taken to the top of a mountain. At the valley floor, the air pressure is 1.0 atm, the temperature is 25°C, and the volume of the bag is 0.985 L. At the top of the mountain, the temperature is 22°C and the bag has puffed up to 1.030 L.

What is the air pressure on top of the mountain?

Use the formula:
[tex]\[
\frac{P_1 V_1}{T_1}=\frac{P_2 V_2}{T_2}
\][/tex]

[tex]\[
\text{Answer:} \quad \text{______} \, \text{atm}
\][/tex]



Answer :

To determine the air pressure at the top of the mountain, we can use the combined gas law formula which relates pressure (P), volume (V), and temperature (T).

The formula is:
[tex]\[ \frac{P_1 V_1}{T_1} = \frac{P_2 V_2}{T_2} \][/tex]

Given data:
- At the valley floor:
- [tex]\(P_1 = 1.0 \, \text{atm}\)[/tex]
- [tex]\(V_1 = 0.985 \, \text{L}\)[/tex]
- [tex]\(T_1 = 25^{\circ} \text{C} + 273.15 = 298.15 \, \text{K}\)[/tex]
- At the top of the mountain:
- [tex]\(V_2 = 1.030 \, \text{L}\)[/tex]
- [tex]\(T_2 = 22^{\circ} \text{C} + 273.15 = 295.15 \, \text{K}\)[/tex]
- We need to find [tex]\(P_2\)[/tex].

First, rearrange the formula to solve for [tex]\(P_2\)[/tex]:
[tex]\[ P_2 = \frac{P_1 V_1 T_2}{T_1 V_2} \][/tex]

Plugging in the values:
[tex]\[ P_2 = \frac{(1.0 \, \text{atm}) (0.985 \, \text{L}) (295.15 \, \text{K})}{(298.15 \, \text{K}) (1.030 \, \text{L})} \][/tex]

Performing the calculation step-by-step:
1. Multiply the values in the numerator:
[tex]\[ 1.0 \times 0.985 \times 295.15 = 290.02275 \][/tex]
2. Multiply the values in the denominator:
[tex]\[ 298.15 \times 1.030 = 307.0955 \][/tex]
3. Divide the results:
[tex]\[ P_2 = \frac{290.02275}{307.0955} \approx 0.9467 \, \text{atm} \][/tex]

So, the air pressure at the top of the mountain is approximately [tex]\(0.9467 \, \text{atm}\)[/tex]. Considering significant figures based on the given data, the most appropriate answer would be:
[tex]\[ P_2 = 0.947 \, \text{atm} \][/tex]

This ensures the precision of the result matches the precision of the given values.