A certain soft drink is bottled so that a bottle at 25 oC contains CO2 gas at a pressure of 5.0 atm over the liquid. Assuming that the partial pressure of CO2 in the atmosphere is 4.0 x 10-4 atm, calculate the equilibrium concentrations of CO2 in the soda both before and after the bottle is opened. The Henry’s law constant for CO2 in aqueous solution is 32 L atm/mol at 25 oC.

Question

A certain soft drink is bottled so that a bottle at 25 oC contains CO2 gas at a pressure of 5.0 atm over the liquid.  Assuming that the partial pressure of CO2 in the atmosphere is 4.0 x 10-4 atm, calculate the equilibrium concentrations of CO2 in the soda both before and after the bottle is opened.  The Henry’s law constant for CO2 in aqueous solution is 32 L atm/mol at 25 oC.

perl · Answer

i have to see the equations

joannablackwelder · Answer

Henry's law:
partial pressure = Henry's law constant * concentration

joannablackwelder · Answer

For the concentration before the bottle is opened, use the partial pressure of the bottled CO2.

joannablackwelder · Answer

And after the bottle is opened, the partial pressure would be the atmospheric pressure of CO2.

anonymous · Answer

[8*10^{-5} M\] that is what i camr up with