Answer to Question #138342 in Inorganic Chemistry for junaide

Question #138342
Sulfur dioxide (SO2
), a gas that plays a central role in the formation of acid rain, is found in the exhaust of
automobiles and power plants. Consider a 1.53-L sample of gaseous SO2 at a pressure of 5.6x103 Pa. If the
pressure is changed to 1.5x104 Pa at a constant temperature, what will be the new volume of the gas?
Expert's answer

the temperature does not change. hence we do so on the basis of the Boyle Marriott law. 

Boyle Marriott's law: the pressure of a gas at constant temperature is inversely proportional to its volume. that is,

P1 / P2 = V 2/ V1

where, P1 —is the initial pressure, P2 —is the next pressure, V1 —is the initial volume, and V2—is the next volume

according to the circumstances of the case

V1=1.53 L

P1=5.6*103 Pa

P2=1.5*104 Pa = 15*103 Pa


V2=P1*V1/P2= 5.6*103* 1.53/15*103= 0.5712 L or 571.2 ml

ANSWER: 0.5712 L or 571.2ml

Need a fast expert's response?

Submit order

and get a quick answer at the best price

for any assignment or question with DETAILED EXPLANATIONS!


No comments. Be the first!

Leave a comment

Ask Your question

New on Blog