Volume occupied by Carbon Dioxide is 1.15L
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.
c) Now,
volume can be calculated by using Ideal Gas Equation:
PV= nRT
Hence ,
V= (nRT/P)
P= pressure of Ideal gas = 1atm
R= 0.082 L.atm/ mol.K
T= (25+273)K = 298K
n= Number of moles of carbon dioxide = 0.047 mol
V= Volume occupied by Carbon Dioxide
Hence,
V= (0.047×0.082×298/1)L
Volume occupied by Carbon Dioxide = 1.15L
From the above conclusion we can say that, Volume occupied by Carbon Dioxide is 1.15L
Learn more about Ideal Gas Equation here:https://brainly.com/question/3637553
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Disclaimer : The question given was incomplete on portal, Here is the complete question.
Question : Soft drinks are canned under 4 atm of CO₂ and release CO₂ when opened.
(a) How many moles of CO₂ are dissolved in a 355-mL can of soda before it is opened?
(b) After it has gone flat?
(c) What volume (in L) would the released CO₂ occupy at 1.00 atm and 25°C ( kH for CO₂ at 25°C is 3.3x10⁻² mol/L?atm; PCO₂in air is 4x10⁻⁴ atm)?
