Question

a sealed syringe contains 0.0450 liters of carbon dioxide gas (co₂). the plunger of the syringe is depressed until the gas occupies a volume of 0.0350 liters at a pressure of 1.140×10³ torr. what was the initial pressure of the co₂ gas in the syringe before the plunger was depressed? 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 for initial pressure $P_1$

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

Step3: Substitute given values

$P_1=\frac{(1.140\times 10^{3}\text{ torr})\times0.0350\text{ L}}{0.0450\text{ L}}$

Step4: Calculate result

$P_1=\frac{1.140\times 10^{3}\times0.0350}{0.0450}\text{ torr}\approx887\text{ torr}$

Answer:

887 torr