Moles of CO₂ after it has gone flat is 4.69×10⁶ mol
Given,
Pressure of Carbon Dioxide= 4atm
Volume of Can of soda=355ml
Henry's Constant of CO₂ = 3.3 ×10² mol/L.atm
Now,
We know that
C = [tex]k_{H}[/tex]×P
where
C= concentration of CO₂
C= 3.3 ×10² mol/L.atm×4atm
Hence ,
Concentration of CO₂= 0.132 mol/L
Given
Volume of soda = 355ml=0.355L
Hence,
No. of moles of Carbon Dioxide = 0.132 mol/L×0.355L
= 0.047 mol
b) When we open the can, Carbon Dioxide will realease the pressure in the can will equal to the pressure of Carbon Dioxide in air.
According to Henry's Law
We know that ,
C = [tex]k_{H}[/tex]×P
partial pressure of CO₂ = 4×10⁻⁴ atm
Hence ,
C = 3.3 ×10² mol/L.atm×4×10⁻⁴ atm
= 1.32 ×10⁻⁵mol/L
Hence in 355 ml of can moles of CO₂ = 1.32 ×10⁻⁵mol/L × 0.355L
= 4.69×10⁶ mol of CO₂ after the soda has gone flat.
From the above conclusion we can say that , Moles of CO₂ after it has gone flat is 4.69×10⁶ mol.
Learn more about Henry's Law here: https://brainly.com/question/23204201
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