Answer:
7.37 L is the new volume
This can be understood as a system that maintains its constant T ° and if the moles of the gas are not modified, the pressure varies inversely proportional to the volume.
Explanation:
We can apply the Ideal Gases Law, to solve this problem. Moles are the same in both cases, the T° also keeps on constant.
P . V = n . R . T For this first situation
P . V = n . R . T For the second situation
V = n . R . T / P
n . R . T will be the same, because n is the number of moles, T means T° and R is a physic constant, so for the first case we can define:
P₁ . V₁, and for the second case, P₂ . V₂
We match both equations, and we replace data
6.20L. 1.10 atm = 0.925 atm . V₂
(6.20L. 1.10 atm) / 0.925 atm = V₂
V₂ = 7.31 L
If the volume decreases, the pressure increases more because the molecules collide more with the walls of the container but the opposite happens where if the volume increases (<u>as in the case of exercise</u>), the pressure will be lower. Gas molecules will not collide so much with the walls
