if someone takes a breath and the lungs expand from 4.5 L to 5.6 L in volume, and the intial pressure inside the lungs is 756mm Hg, what was the pressure inside the lungs before any additional air is pulled in

P₂ = 607 mmHg

Explanation:

Given data:

Initial volume = 4.5 L

Final volume = 5.6 L

Initial pressure = 756 mmHg

Final pressure = ?

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

756 mmHg × 4.5 L = P₂ × 5.6 L

P₂ = 3402 mmHg. L/5.6 L

P₂ = 607 mmHg

c is having 4 valence electrons and is bonded to three hydrogens and one sulphur atom, therefore, the number of bond pair is equal to four. as all the valence electrons are used in forming the bonds so, there is no lone pair left on carbon.

s is having 6 valence electrons and is bonded to one other sulfur atom and one carbon atom, therefore, the number of bond pair is equal to 2. as only two valence electrons are used in forming the bonds so, four electrons are left. therefore, two lone pairs are present on s.