1. The Henry’s Law constant for O2 is 770 L atm mol-1 at 25 °C. What mass of oxygen would be dissolved in a 40-L aquarium at 25 °C, assuming an atmospheric pressure of 1.00 atm, and that the partial pressure of O2 is 0.21 atm?
2.The carbon dioxide concentration in a bottle of club soda is 0.12 mol L-1 at 25 °C. What is the pressure of carbon dioxide in the headspace? The Henry’s Law constant for CO2 at 25 °C is 3.4 x 10-2 mol L-1 bar-1 .
1. The Henry’s Law constant for O2 is 770 L atm mol-1 at 25 °C. What...
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...
A bottle of soda is opened and allowed to equilibrate at 25°C, at partial pressure= 0.95 6. atm. (Hint: refer to Henry's Law) a. (1pt) Calculate the concentration, in moles/L, of CO2 in the drink. Given ko02= 3.4 x 102 mol/(Latm) Ans. b.(Apt) If the partial pressure were higher, would you expect the concentration of carbon dioxide in the soda to be higher or lower than the answer to part a? Explain.
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...
The Henry's law constant (kH) for O2 in water at 20°C is 1.28e-3 mol/l atm. How many grams of O2will dissolve in 3.5 L of H2O that is in contact with pure O2 at 2.4 atm?
The concentration of dissolved CO2 gas in seawater is 5.00 x 10^–3 mol L–1 . The Henry’s law constant for CO2 at 298 K is 3.13 x 10^–7 mol L–1 Pa–1 . Calculate the partial pressure of carbon dioxide gas in the atmosphere above the ocean. (A) 16.0 kPa (B) 6.30 x 10–5 Pa (C) 1.57 x 10–9 Pa (D) 6.30 x 108 kPa
Henry’s law states that the solubility of a gas is directly proportional to the partial pressure of the gas if the temperature is constant. Hyperbaric chambers, which provide high pressures (up to 6 atm) of either air or pure oxygen, are used to treat a variety of conditions, ranging from decompression sickness in deep-sea divers to carbon monoxide poisoning. Look up the Henry’s Law Constant (kH) for N2, O2, and CO2 in the textbook. a) Calculate the solubility (concentration in...
The log Henry's law constant (units of L-atm/mole and measured at 25 C) for trichloroethylene is 1.03; for tetrachloroethylene, 1.44; for 1, 2-dimethylbenzene, 0.71; and for parathion, -3.42. (a) What is the dimensionless Henry's law constant for each of these chemicals? (b) Rank the chemicals in order of ease of stripping from water to air. If needed use ideal gas Law (pV= nRT). R = 0.08205 (atm times L)/(mole times K). The dimensionless Henry's law constant is equal to K_H(L_H_2...
1. What statement is true about Henry’s Law A. The concentration of a gas dissolved in a liquid is directly proportional to the concentration of the gas over the liquid. B. The Henry’s law constant for every gas is the same as long as it dissociates completely. C. Henry’s law is used to determine how dissolved salts change the vapor pressure over a liquid in a sealed container. D. The partial pressure of an individual gas over a liquid is...
The Henry's Law constant of methyl bromide, CH3Br, is k = 0.159 mol/(L • atm) at 25°C. What is the solubility of methyl bromide in water at 25°C and at a partial pressure of 270. mm Hg?
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.