Question

a sample of chlorine gas (cl₂) at a pressure of 1.685 × 10⁴ torr is transferred from a 12.34 - liter cylinder to an empty tank. after transfer, the pressure of the gas in the tank is 1.273 × 10⁴ torr. what is the final volume of the cl₂ gas inside the tank? assume ideal gas behavior and a constant temperature. write your answer to the correct number of significant figures. round if necessary.

Explanation:

Step1: Identify Boyle's Law formula

$P_1V_1 = P_2V_2$

Step2: Define the given values

$P_1=1.685\times 10^{4}$ torr, $V_1 = 12.34$ L, $P_2=1.273\times 10^{4}$ torr

Step3: Rearrange the formula to solve for $V_2$

$V_2=\frac{P_1V_1}{P_2}$

Step4: Substitute the values

$V_2=\frac{(1.685\times 10^{4}\text{ torr})\times(12.34\text{ L})}{1.273\times 10^{4}\text{ torr}}$
$V_2=\frac{1.685\times12.34}{1.273}\text{ L}$
$V_2=\frac{20.7929}{1.273}\text{ L}$
$V_2 = 16.34$ L

Answer:

16.34