The atmospheric concentration of CO2 gas is presently 390 ppm (parts per million, by volume; that is, 390 L of every 106 L of the atmosphere are CO2). What is the mole fraction of the gas in the atmosphere?

The Henry's Law constant for CO2 at 25 C is 0.033363 mole/L-atm,the atmospheric CO2 content is 390 ppm calculate the concentrationof dissolved CO2 (in mol/L and in mgCO2/L) in a body of water whichis in equilibrium with the atmosphere

Given the concentration of CO₂ in the atmosphere is 407 ppm (= 0.000407 mol fraction), determine the equilibrium concentration of CO₂ in water, [CO₂] at 10°C in mol/L.

Henry's constant for CO2 is: 0.104 E^-4 atm

For Part B, Your K_H is 0.042 mol/(L*atm), K₁=4.47 x 10^-7, and K₂= 4.68 x 10^-11

B) If you have a pH of 8.2 and an atmospheric concentration of 280 ppm CO₂ (which is a partial pressure of CO₂ of 280 x 10^-6 atm), what are your concentrations of [CO₂]_(aq), and [HCO₃^-] and what is your total dissolved carbon (the sum of these two carbon ions) in mol/L. Recalculate this if your atmospheric concentration of CO₂ is 400 ppm and pH is 8.1.

C) If there is 1.3 x 10²¹ L of water in the world's oceans, how much more carbon (in kg) can be stored in the oceans today at equilibrium (with 400 ppm CO₂ in the atmosphere and ocean pH of 8.1) compared to pre-industrial revolution (when it was 280 ppm CO₂ in the atmosphere and pH of 8.2). convert the mol/L in part B to kg C (0.012 kg C/mol C)