1. Assume that carbon dioxide in a 2.00 L soda bottle is dissolved at a pressure
ID: 1074598 • Letter: 1
Question
1. Assume that carbon dioxide in a 2.00 L soda bottle is dissolved at a pressure of 2.07 bar. At 2.2 °C, the Henry's law constant for carbon dioxide dissolved in water is 0.068 Calculate the concentration of dissolved carbon dioxide in mol/L and the mass of carbon mol L bar dioxide that can be dissolved in the bottle of soda at the given pressure. 2. Now assume that you open that bottle of soda at the same temperature and allow the ressure to equilibrate to the atmospheric pressure which is 0.993 bar. Calculate the concentration of dissolved carbon dioxide in mol/L and the mass of carbon dioxide that can be dissolved in the bottle of soda at this new pressure.Explanation / Answer
given Henry's law constant,KH = 0.068 mole/L.bar
pressrue of CO2,P= 2.07 bar, concentration = P*KH= 0.068*2.07 mole/L=0.141 moles/L
volume of bottle= 2L, moles of CO2= concentration* volume in L=0.141*2= 0.282 moles
mass of CO2= moles* molar mass =0.282*44 =12.41 gm
when pressure is 0.993 bar, concentration= 0.068*0.993 mol/l=0.0675 mol/l
moles=0.0675*2=0.135 moles, mass of CO2=0.135*44=5.94 gm
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