Mountain Dew is bottled so that a bottle at 25 °C contains CO2 gas at a pressure of 6.304 atm over the liquid. Assuming that the partial pressure of CO2 in the atmosphere is 4.461×10-4 atm, the Henry’s Law constant for CO2 in aqueous solution is 0.03003 mol/L.atm at 25 °C. 1) Please calculate the equilibrium concentrations of CO2 (molarity) in the Mountain Dew solution before the bottle is opened. _________ M 2) Please calculate the equilibrium concentrations of CO2 (molarity) in the Mountain Dew solution after the bottle is opened. ___________ mM 3) The size of a Mountain Dew bottle is 591.5 mL, how many grams of CO2 is released when the bottle is opened? ___________ g
Mountain Dew is bottled so that a bottle at 25 °C contains CO2 gas at a pressure of 6.304 atm over the liquid.
Assuming that the partial pressure of CO2 in the atmosphere is 4.461×10-4 atm, the Henry’s Law constant for CO2 in aqueous solution is 0.03003 mol/L.atm at 25 °C.
1) Please calculate the equilibrium concentrations of CO2 (molarity) in the Mountain Dew solution before the bottle is opened. _________ M
2) Please calculate the equilibrium concentrations of CO2 (molarity) in the Mountain Dew solution after the bottle is opened. ___________ mM
3) The size of a Mountain Dew bottle is 591.5 mL, how many grams of CO2 is released when the bottle is opened? ___________ g
Given that the Henry's law constant for CO2 is
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