In an experiment, 25.0 mL of a gas with a pressure of 1.00 atm is contained in a balloon at 25.0°C. The balloon is then cooled to 5.0 $\circ$ C, and the pressure is found to be 0.750 atm. What is the volume of the gas under the new conditions?

Question

Quizplus · Accepted Answer

To find the new volume, we can use the combined gas law: $P_1V_1/T_1 = P_2V_2/T_2$. Given $P_1 = 1.00$ atm, $V_1 = 25.0$ mL, $T_1 = 25.0°C = 298K$, $P_2 = 0.750$ atm, and $T_2 = -10°C = 263K$, solving for $V_2$ gives $V_2 = (P_1V_1T_2)/(P_2T_1) = (1.00 \times 25.0 \times 263)/(0.750 \times 298) = 31.1$ mL.

In an Experiment, 25 ∘\circ∘ C, and the Pressure Is Found to Be 0

In an Experiment, 25 $\circ$ C, and the Pressure Is Found to Be 0