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# partial pressures of SO2 and N2

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3.00 g of SO2(g) is originally in a 5.00 L vessel at 21 degrees Celsius and is transferred to a 10.0 L vessel at 26 degrees Celsius. 2.35 g N2(g) is originally in a 2.50 L vessel at 20 degrees Celsius and is transferred to the same 10.0 L vessel.

- what is the partial pressure of SO2(g) in the larger container?
- what is the partial pressure of N2(g) in this vessel
- what is the total pressure of the vessel?

https://brainmass.com/chemistry/physical-chemistry/partial-pressures-so2-n2-210271

#### Solution Summary

It finds out the partial pressures of SO2 and N2 in the vessel, respectively.

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## reaction rate of the aqueous route to oxidize SO2

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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