Answer to Question #138342 in Inorganic Chemistry for junaide

Question

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?

Answer 1

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=?

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