[mug3n]

Problem is given as such

A water carbonating plant is available for use in the home and operates by providing
carbon dioxide at 5.0 atm.  Estimate the molar concentration, m (in mol/kg), of the soda
water it produces.  The Henry's law constant for CO2 in water at 25 °C is 1650 atm.  Use
the following representation of Henry' law:
 
pB = xBKB
 
where pB is the vapor pressure of the solute; xB is the mole fraction of the solute (mole
per mole); and KB is the proportionality constant. 
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I've never really worked with Henry's Law constants where it isn't given as L*atm/mol, so I'm not sure if my approach is right here.

So I first find mole fraction of the CO2 as a gas which is 5/1650 = 0.00303.  Assuming everything is ideal, that means the mole fraction of the gas dissolved in water should be 1-0.00303=0.997.  Then I work out the # of moles of the CO2 in solution assuming there is 100g of dissolved CO2 total, and use the # of moles divided by weight of the CO2 in the dissolved solution.

I don't really care about the answer, just wanna know if my train of thought is off anywhere.  Appreciate any help/comments.