Question

a balloon filled with hydrogen gas (h₂) has an internal pressure of 1.268 bar and a volume of 5.000 × 10⁻³ cubic meters when squeezed. releasing the balloon causes the pressure to decrease to 1.100 bar. what is the final volume of the h₂ gas in the balloon? 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: Assign values

$P_1=1.268$ bar, $V_1 = 5.000\times10^{-3}$ m³, $P_2 = 1.100$ bar

Step3: Solve for $V_2$

$V_2=\frac{P_1V_1}{P_2}=\frac{1.268\times5.000\times 10^{-3}}{1.100}$
$V_2=\frac{6.34\times10^{-3}}{1.100}\approx5.764\times 10^{-3}$ m³

Answer:

$5.764\times 10^{-3}$