The solubility constant for CO2 in water at 25∘C is 3.40 x 10-2 M/atm. The solubility of CO2 is 34.164 mM in water that is exposed to a gas mixture in which the mole fraction of CO2 is 0.78. What is the total pressure of this gas mixture? Express your answer in units of atmospheres using at least three significant figures.
The solubility constant for CO2 in water at 25∘C is 3.40 x 10-2 M/atm. The solubility...
The solubility constant for CO2 in water at 25 celsius is 3.40 x 10-2 M/atm. The solubility of CO2 is 35.158 mM in water that is exposed to a gas mixture in which the mole fraction of CO2 is 0.67. What is the total pressure of this gas mixture? Express your answer in units of atmospheres using at least three significant figures.
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.
5. The solubility of CO2 in water at 25 °C and 1 atm is 0.034 mol/L, W CO2 in carbonated water, if CO2 has a partial pressure of 0.0003s solubility ot atmospheric conditions? (5 points) atm under normal 6. The atmosphere contains 0.93 mol% argon, what is the partial pressure of argon at normal conditions of 1 atm and 25 °C? If the solubility of argon in water is 0.0150 mo/L under normal atmospheric conditions, what is Henry's Law Constant...
Calculate the solubility (in M units) of ammonia gas in water at 298 K and a partial pressure of 8.00 bar . The Henry’s law constant for ammonia gas at 298 K is 58.0 M/atmand 1 bar=0.9869 atm. Express your answer in molarity to three significant figures.
6.) The solubility of CO2 (g) in water is 3.2 x 102 M at 25.0 °C and 1.0 atm pressure. a.) What is the Henry's Law constant for CO2 (g)? Cg = k P, ; Cg = concentration in M; k = Henry's Law constant in mol L atm*'; P. = pressure in atm. 3.2 x 10-2 M=k (1.0 atm) (3.2 x 10-2 M)/(1.0 atm) = k = 3.2 x 10-2 M/atm = 3.2 x 10-2 mol L atm" b.)...
7.0 L of O2 at 1.0 atm is mixed together with 8.0 L of N2 at 7.0 atm at a constant temperature of 25 C in a 25.0 L vessel. What is the mole fraction of N2 in the 25.0 L vessel? Assume the gases behave ideally. Express your answer as a unitless mole fraction using at least three significant figures.
4. The solubility of nitrogen gas in water at 25°C and a partial pressure of N2 of 0.78 atm is 5.5×10–4 mol/L. A. Calculate kH, Henry’s Law constant for nitrogen gas, at this temperature using the solubility at 0.78 atm. S = kH × P
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
A sample of He gas (3.0 L) at 5.6 atm and 25 °C was combined with 4.5 L of Ne gas at 3.6 atm and 25 °C at constant temperature in a 9.0 L flask. The total pressure in the flask was __________ atm. Assume the initial pressure in the flask was 0.00 atm. In a gas mixture of He, Ne, and Ar with a total pressure of 8.40 atm, the mole fraction of Ar is __________ if the partial...
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.