A sample of gas collected at 21.0 ° C and a pressure of 660 torr has a volume of 1.83 liters. What volume in liters will the gas occupy at 38.0 ° C under a pressure of 500 torr?
A)2.56
B)4.37
C)2.28
D)1.33

Question

Quizplus · Accepted Answer

To find the new volume of the gas, we can use 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: $21.0 °C = 294.15 K$ and $38.0 °C = 311.15 K$. Then, rearrange the formula to solve for $V_2$: $V_2 = \frac{P_1V_1T_2}{P_2T_1}$. Plugging in the given values: $V_2 = \frac{660 \, \text{torr} \times 1.83 \, \text{L} \times 311.15 \, \text{K}}{500 \, \text{torr} \times 294.15 \, \text{K}}$, which calculates to approximately 2.56 liters.

A Sample of Gas Collected at 21