) In addition to ongoing sources, such as car engines, pollutants can also be introduced into the air through isolated incidents like the rupture of a gas storage tank. Most
gases are stored and transported at high pressures. A common laboratory cylinder of
methane, for example, has a volume of 49.0 L and is filled to a pressure of 154 atm.
Suppose that all the CH4 from this cylinder is released and expands until its pressure
falls to 1.00 atm. What volume would the CH4 occupy?

V₂ =  7546  L

Explanation:

Given data:

Initial volume = 49.0 L

Initial pressure = 154 atm

Final pressure = 1 atm

Final volume = ?

Solution:

The given problem will be solved through the Boyle's law,

"The volume of given amount of gas is inversely proportional to its pressure by keeping the temperature and number of moles constant"

Mathematical expression:

P₁V₁ = P₂V₂

P₁ = Initial pressure

V₁ = initial volume

P₂ = final pressure

V₂ = final volume  

Now we will put the values in formula,

P₁V₁ = P₂V₂

154 atm × 49.0 L = 1.00 atm × V₂

V₂ = 7546 atm. L/1 atm

V₂ =  7546  L

fire could start, buildings collapsing, and ash falling from the sky.

explanation:

this is because the buildings or plants could catch on fire and the buildings would most likely collapse. lastly ash would fall because all the burning would cause ash to fall from the sky.

hope this .

pv=nrt

explanation: