On a cold day, you take in 4.2 L of air into your lungs at a temperature of 0°C. If you hold your breath until the temperature of the air in your lungs reaches 37°C, what is the volume of the air in your lungs at that point, assuming the pressure does not change?
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- Initial volume of air, \( V_1 = 4.2 \, \text{L} \) - Initial temperature, \( T_1 = 0^\circ \text{C} \) - Final temperature, \( T_2 = 37^\circ \text{C} \) - Pressure remains constant - Required: Final volume of air, \( V_2 \) Show more…
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On a chilly $10^{\circ} \mathrm{C}$ day, you quickly take a deep breath-all your lungs can hold, $4.0 \mathrm{L}$. The air warms to your body temperature of $37^{\circ} \mathrm{C}$. If the air starts at a pressure of $1.0 \mathrm{atm},$ and you hold the volume of your lungs constant (a good approximation) and the number of molecules in your lungs stays constant as well (also a good approximation), what is the increase in pressure inside your lungs?
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