The solubility of CO2 in a salt water lake at 298 K and 750 torr pressure...

The solubility of CO2 in a salt water lake at 298 K and 750 torr pressure was found to be 1.0 x 10-5 moles CO2/liter of aqueous solution. The Henry’s Law constant in this case is 3.0 x 10-2 mol/L.atm.

A) Please find the partial pressure of CO2 (g) (PCO2, in atm) in the air above the lake.

B) Please use your answer to determine the percentage of CO2 in the atmosphere.

C) Given the percentage of CO2 in the atmosphere is constant at sea level and below, please calculate the solubility (moles/liter of aqueous solution) of CO2 in the Dead Sea at 298 K and a pressure of 800 torr.

Thank you!

Solutions

Expert Solution

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

Density of CO2 = 1.711 g/L Temperature of water: 23 Celcius Atmospheric Pressure: 738.8 torr Trial...

Density of CO2 = 1.711 g/L Temperature of water: 23 Celcius Atmospheric Pressure: 738.8 torr Trial Mass of Unknown Carbonate Used Volume of 6.00 M HCl Used Volume of CO2 produced I 1.00g 5.00 mL 211 mL II 1.00g 5.00 mL 241 mL 5. Determine the average volume of CO2 produced in the 2 trials of the experiment, and, using the density of CO2, determine the average mass of CO2 produced from the unknown in those 2 trials. 6. Using...

The vapor pressure of water at blood temperature is 47 Torr.

The vapor pressure of water at blood temperature is 47 Torr. What is the partial pressure of dry air in our lungs when the total pressure is 760 Torr? (1Torr = 133.3 Pa )

What is the molar solubility of Ag2CrO4 in water? The value of Ksp for this salt...

What is the molar solubility of Ag2CrO4 in water? The value of Ksp for this salt is 1.2 x 10-12.

At 35ºC, the vapor pressure of pure water is 42.2 torr. Calculate the vapor pressure of...

At 35ºC, the vapor pressure of pure water is 42.2 torr. Calculate the vapor pressure of water at this temperature in a solution that has a concentration of 6.5 M of NaCl. The density of the solution is 1.09 g/mL

Given that the vapor pressure of water is 17.54 Torr at 20 °C, calculate the vapor-pressure...

Given that the vapor pressure of water is 17.54 Torr at 20 °C, calculate the vapor-pressure lowering of aqueous solutions that are 2.50 m in (a) sucrose, C12H22O11, and (b) calcium chloride. Assume 100% dissociation for electrolytes.

Given that the vapor pressure of water is 17.54 Torr at 20 °C, calculate the vapor-pressure...

Given that the vapor pressure of water is 17.54 Torr at 20 °C, calculate the vapor-pressure lowering of aqueous solutions that are 2.30 m in (a) sucrose, C12H22O11, and (b) aluminum chloride. Assume 100% dissociation for electrolytes.

Calculate the cell potential and the equilibrium constant for the following reaction at 298 K: Co2+(aq)...

Calculate the cell potential and the equilibrium constant for the following reaction at 298 K: Co2+(aq) + 2I-(aq) Co(s) + I2(s) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant:

Consider the decomposition of barium carbonate: BaCO3(s)???BaO(s)+CO2(g) A) Calculate the equilibrium pressure of CO2 at 298...

Consider the decomposition of barium carbonate: BaCO3(s)???BaO(s)+CO2(g) A) Calculate the equilibrium pressure of CO2 at 298 K. B) Calculate the equilibrium pressure of CO2 at 1300K .

At 25 °C and 785 Torr, carbon dioxide has a solubility of 0.0351 M in water....

At 25 °C and 785 Torr, carbon dioxide has a solubility of 0.0351 M in water. What is its solubility at 25 °C and 2030 Torr?

The solubility product of Hg2Cl2 at T=298 K is 1.2 x 10-18. What is the molar...

The solubility product of Hg2Cl2 at T=298 K is 1.2 x 10-18. What is the molar solubility of this salt? 2.0 x 10-9 mol L-1 6.9 x 10-7 mol L-1 There is not enough information to answer this question

Subjects