Question

a sealed syringe contains 37.55 milliliters of oxygen gas (o₂) at a pressure of 1.203 bar. the plunger of the syringe is pulled back until the volume inside the syringe is 43.33 milliliters. what is the final pressure of the o₂ gas in the syringe? 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

$P_1=1.203$ bar, $V_1 = 37.55$ mL, $V_2=43.33$ mL

Step3: Solve for $P_2$

$P_2=\frac{P_1V_1}{V_2}=\frac{1.203\times37.55}{43.33}$
$P_2=\frac{45.17265}{43.33}\approx1.043$ bar

Answer:

1.043 bar