Answer:
45.0 L is the volume of gas will the balloon contain at 1.35 atm and 253 K.
Explanation:
Using Ideal gas equation for same mole of gas as
Given ,
V₁ = 25.0 L
V₂ = ?
P₁ = 2575 mm Hg
Also, P (atm) = P (mm Hg) / 760
P₁ = 2575 / 760 atm = 3.39 atm
P₂ = 1.35 atm
T₁ = 353 K
T₂ = 253 K
Using above equation as:
Solving for V₂ , we get:
<u>V₂ = 45.0 L</u>
45.0 L is the volume of gas will the balloon contain at 1.35 atm and 253 K.
Answer: D
Explanation: I got it wrong on my test :( and got this answer as correct.
Answer:
Yes, it does, although only physically and not chemically.
Explanation:
If a volume of gas is way spread out, it won't collide with the other gas particles as often, reducing pressure and temperature because they lose kinetic energy to their surroundings when they don't collide.
If it is compressed, it increases temperature and pressure because the gas particles collide with each other and the walls of the container way more often than if they had more space.
Hope this answers your question.
P.S.
Fun fact, gas particles are actually moving at 300-400 meters per second at room temperature, they only slow down to walking speed at very low temperatures, like 10 Kelvin
