Determine the solubility of carbon dioxide in water at 25 degrees C exposed to air at 1.0 atm. Assume a partial pressure for carbon dioxide of 9.3x10^-3 atm. (kH,CO2=3.4×10−2M/atm.)
Solution :-
Using the Henrys law we can calculate the solubility of the gas
C= kH* Pgas
C= 3.4*10^-2 M/atm * 9.3*10^-3 atm
C= 3.162*10^-4 M
Therefore the solubility of the CO2 gas is
3.162*10^-4 mol per L * 44.01 g per mol =0.0139 g/L
Determine the solubility of carbon dioxide in water at 25 degrees C exposed to air at...
Determine the solubility of N2 in water exposed to air at 25°C if the atmospheric pressure is 1.2 atm. Assume that the mole fraction of nitrogen is 0.78 in air and the Henry's law constant for nitrogen in water at this temperature is 6.1 × 10-4 M/atm.
What is the solubility of carbon dioxide (in units of grams per liter) in water at 25 °C, when the CO2 gas over the solution has a partial pressure of 156 mm Hg? kH for CO2 at 25 °C is 3.36×10-2 mol/L·atm.
Question 15 4 pts Determine the solubility of CO2 in soda water at 25°C if the pressure of CO2 is 4.4 atm. The Henry's law constant for carbon dioxide in water at this temperature is 3.4 x 10-2 M/atm. O 0.65 M 0.57 M O 0.15 M O 0.18 M
The partial pressure of carbon dioxide in air is approximately 10^-3.42 atm. In temperate regions the pressure of CO2 in gas can be as high as 10^-1.5 atm. For each of these two cases, calculate the mass of carbon dioxide (in grams) in 1.0 m^3 of gas at 25 Celsius.
1- At 25 oC the Henry’s Law constant for carbon dioxide (CO2) dissolved in water is 3.3 x 10-2 mol/L atm. Calculate the solubility of CO2 if the partial pressure of carbon dioxide gas inside a bottle of Fizzy Cola Drink is 6 atm at 25 C 2- Using Raoult’s Law, calculate vapor pressure lowering, DP = C · Po, when 14.0 mL of glycerol (C3H8O3) is added to 496.0 mL of water at 50.0 C. The density of glycerol...
(8 pts) Carbon dioxide in the atmosphere dissolves in water to establish an equilibrium that can increase the acidity of aqueous solutions in the environment. This equilibrium is CO2 (g) ⇌ CO2 (aq), Kh = 3.1 * 10^2 at 25°C. Kh is called the Henry’s law constant, which relates the solubility of the gas CO2 in the aqueous solution, [CO2], to the partial pressure of CO2 over the solution, p(CO2): [CO2] (M) = Kh * p(CO2) (atm) During the preceding...
Calculate the solubility of carbon dioxide in water at 10.0 C and a pressure of 3.00 atm. The solubility of carbon dioxide is 0.0791 mol/L water at 10.0 C and 1.00 atm
The solubility of CO2 in water at 25°C and 1 atm is 0.034 mol/L. What is its solubility at a partial pressure in air of 0.00049 atm? Assume that CO2 obeys Henry's law.
The solubility of CO2 in water at 25°C and 1 atm is 0.034 mol/L. What is its solubility at a partial pressure in air of 0.00047 atm? Assume that CO2 obeys Henry's law.
Calculate the solubility of carbon dioxide in water at an atmospheric pressure of 0.420 atm (a typical value at high altitude). Calculate the solubility of carbon dioxide in water at an atmospheric pressure of 0.420 atm (a typical value at high altitude). Atmospheric Gas Mole Fraction N2 7.81 x 10-1 ky mol/(L*atm) 6.70 x 10-4 1.30 x 10-3 02 2.10 x 10-1 Ar 9.34 x 10-3 1.40 x 10-3 CO2 3.33 x 10-4 3.50 x 10-2 CH4 2.00 x 10-6...