A volume of 2.2 L of air at 37. °C is expelled from the lungs into cold surroundings at 8.6 °C. The pressure and the number of gas particles do not change.
What volume (in L) does the expelled air occupy at 8.6 °C? Be sure your answer has the correct number of significant figures.
Using the ideal gas law equation:
\( \frac{P_1V_1}{T_1} = \frac{P_2V_2}{T_2} \)
where:
\( P_1 = P_2 \) (pressure remains constant)
\( V_1 = 2.2 L \)
\( T_1 = 37 + 273 = 310 K \)
\( T_2 = 8.6 + 273 = 281.6 K \)
\( \frac{2.2 \times 310}{281.6} = V_2 \)
\( V_2 = 2.4 L \)
Therefore, the expelled air would occupy 2.4 L at 8.6 °C.