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reaction rate of the aqueous route to oxidize SO2

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Consider the following aqueous route to oxidize SO2:
SO2(aq) + H2O2(aq) -> H2SO4(aq) k = 1.1 X 10^3 L/mols
a. The partial pressure and Henry's law constants for SO2 and H2O2 are 2.7 ppm (KH = 1.2 mol L-1atm-1) and 4.9 ppb (KH = 1.0E5 mol L-1atm-1), respectively. Calculate the reaction rate of this process.
b. Calculate the reaction rate (per liter of air) if the amount of liquid water in the atmosphere is 0.008 g L-1.

Hint: Calculate volume of water contaminated, length of time to do this, distance

I downloaded a study guide and attempted it 3 times but was wrong.

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It shows how to calculate the reaction rate of the aqueous route to oxidize SO2.

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I really do implore you to work your way through the thought process on the way to these answers.

Henry's Law is a an approximation of the amount of the gas in the vapor over the liquid that dissolves into the solvent . The molality of the solute gas is proportional in the limit of little solute gas in the solvent to the partial pressure of the gas in the vapor over the solvent The K's given in the relations of these gasses are the proportionality constants for the respective gasses in equilibrium with the solvent.

Also the total moles of things making up the liquid is the sum of the moles H2SO4 (aq) + moles SO2 (aq) + moles of H2O2 (aq) and the molality of a species is n moles species/total moles substance.

Also Henrys law is an ideal gas law such that the amount of solute in the overall atmospheric gas is dilute enough such that ideal gas relations apply. Thus PV=nRT for the partial pressures of the gasses in question.

Finally, in the case of gasses ppm and ppb are usually reported by volume rather than a mixed mass to volume as we see for liquids and as I have said before this can lead to some mass confusion when reporting calculated values.

I am pretty confused by this notation. I am going to look at a web site on environmental chemistry and see if I can shed light on this problem.
FIRST WEB SOURCE
The ultimate fate of all sulfur in the atmosphere is to be oxidized to the sulfate ion, usually as sulfuric acid (H2SO4). The most common base present in the ...

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