Chemistry Homework Solutions
Problem
#29389

Problem with Henry's constants and partial pressures

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 2.1 ppm (KH = 1.2 mol L-1atm-1) and 4.8 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 0.02 g L-1.

Hint:  Convert ppm and ppb to partial preferences, calc rate.

Please give a specific answer, and show me how to work it out. Thanks!

Solution
What is this?
By OTA - Overall OTA Rating
Ewen McLaughlin, MSc - 4.7/5
Purchase Cost Now
$2.19 CAD (was ~$3.99)
Included in Download
  • Plain text response
$2.19 Instant Download
Add to Cart
Why you can trust BrainMass.com
  • Your Information is Secure
  • Best Online Academic Help Service
  • Students find real academic Success
Related Solutions
  • Determining the atmospheric pressure of partial pressures. - What is the atmospheric pressure if the partial pressures of nitrogen, oxygen, and argon are 77.75 kPa, 19.94 kPa, and 1.99 kPa, respectively?
  • Concentration of nitric oxide - At combustion temperatures, the equilibrium constant for the reaction N2 + O2 -> 2NO is about 4.0E-14. Calculate the concentration(atm) of nitric oxide that is in equilibrium with atmospheric levels o ...
  • Henry's Law, need rxn rate of diff measurements given volume - 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 mo ...
  • given k1 & k2, calculate equilibrium constant - H20(l) f/r H+(aq) + OH-(aq) k1 is forward and K_1 is reverse if k1 = 2.4 x 10^-5 s^-1 and K_1=1.3 x 10^11/M *s calculate the equilibrium constant K calculate k=[H+][OH-] and [H+] and [OH-]. shoul ...
  • Equilibrium - In the reaction N2O4(g) <-----> 2 NO2(g), equilibrium is reached at a temperature at which P(of)NO2 = 3(P(of)N2O4)^1/2. What must be the value of Kp at this temperature?
Browse