Question

a balloon filled with carbon dioxide gas (co₂) has a volume of 0.0045 cubic meters and an internal pressure of 1.33 bar when squeezed. releasing the balloon causes the volume of the balloon to increase to 0.0061 cubic meters. what is the final pressure of the co₂ 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: Rearrange formula for $P_2$

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

Step3: Substitute given values

$P_1 = 1.33$ bar, $V_1=0.0045$ m³, $V_2 = 0.0061$ m³. So $P_2=\frac{1.33\times0.0045}{0.0061}$

Step4: Calculate $P_2$

$P_2=\frac{1.33\times0.0045}{0.0061}=\frac{0.005985}{0.0061}\approx0.98$ bar

Answer:

$0.98$ bar