Question

a balloon filled with hydrogen gas (h₂) has a volume of 4.911 liters. squeezing the balloon causes the volume to decrease to 4.202 liters and the internal pressure to increase to 3.333 atmospheres (atm). what was the initial pressure of the h₂ gas in the balloon before it was squeezed? assume ideal gas behavior and a constant temperature. write your answer to the correct number of significant figures. round if necessary.

Explanation:

Step1: Recall Boyle's Law

$P_1V_1 = P_2V_2$

Step2: Identify given values

$V_1=4.911$ L, $V_2 = 4.202$ L, $P_2=3.333$ atm

Step3: Solve for initial pressure $P_1$

$P_1=\frac{P_2V_2}{V_1}=\frac{3.333\times4.202}{4.911}$
$P_1=\frac{13.905266}{4.911}\approx2.831$ atm

Answer:

2.831 atm