A sample of gas at an initial volume of 65.0 mL, an initial pressure of 866 torr, and an initial temperature of 10.0°C simultaneously changes its temperature to 60.0°C and its volume to 46.0 mL. What is the final pressure of the gas?

Question

Quizplus · Accepted Answer

The final pressure of the gas can be calculated using the combined gas law, which is $P_1V_1/T_1 = P_2V_2/T_2$, where $P$ is pressure, $V$ is volume, and $T$ is temperature in Kelvin. First, convert temperatures to Kelvin: $T_1 = 10.0°C + 273.15 = 283.15 K$ and $T_2 = 60.0°C + 273.15 = 333.15 K$. Then, solve for $P_2$: $P_2 = P_1V_1T_2 / (V_2T_1) = (866 \, \text{torr} \times 65.0 \, \text{mL} \times 333.15 \, K) / (46.0 \, \text{mL} \times 283.15 \, K)$. This calculation gives $P_2 \approx 1440 \, \text{torr}$, making the correct answer E.

A Sample of Gas at an Initial Volume of 65