Question

a balloon filled with neon gas (ne) has an internal pressure of 1.145 bar when squeezed. releasing the balloon causes the pressure to decrease to 1.099 bar and the volume to increase to 4.250 × 10³ milliliters. what volume did the ne gas occupy before the balloon was released? assume ideal gas behavior and a constant temperature. write your answer to the correct number of significant figures. round if necessary. milliliters

Explanation:

Step1: Identify Boyle's Law formula

Boyle's Law is $P_1V_1 = P_2V_2$, where $P_1$ and $V_1$ are initial - pressure and volume, and $P_2$ and $V_2$ are final - pressure and volume.

Step2: Rearrange the formula to solve for $V_1$

$V_1=\frac{P_2V_2}{P_1}$.

Step3: Substitute the given values

$P_1 = 1.145$ bar, $P_2 = 1.099$ bar, $V_2=4.250\times 10^{3}$ mL.
$V_1=\frac{1.099\times4.250\times 10^{3}}{1.145}$.

Step4: Calculate the value of $V_1$

$V_1=\frac{4670.75}{1.145}=4088$ mL.

Answer:

$4088$ mL