Problem 2: a) Find the dimensionless Henry's Law constant for (i) phenanthrene and (ii) TCE (hint:...
Estimate the Henry’s law constant of TCE using its water solubility and vapor pressure using the temperature dependent values listed below. MW=131.38g/mol, Water solubility=1.1*10^3mg/L, T=25 degrees cel.
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...
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?
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At 298 K, the Henry's law constant for oxygen is 0.00130 M/atm. Air is 21.0% oxygen. At 298 K, what is the solubility of oxygen in water exposed to air at 1,00 atm? Number At 298 K, what is the solubility of oxygen in water exposed to air at 0.893 atm? Number If atmospheric pressure suddenly changes from 1.00 atm to 0.893 atm at 298 K, how much oxygen will be released from...
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...
1.) Explain why I, is insoluble in water, but soluble in CCI: (5 pts) 2.) The partial pressure of carbon dioxide inside a bottle of cola is 4.0 atm at 25°C. What is the solubility of CO,? The Henry's law constant for CO, in water is 3.3 x 10 mol/L(atm) at 25 °C. (5 pts)
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-Kor Cor The Henry's law constant of oxygen in water at 25 °C is 773 atm mol'' kg of water. Calculate the molality of oxygen in water under a partial pressure of 0.20 atm. Assume that the solubility of oxygen in blood at 37 °C is roughly the same as that in water at 25 °C, comment on the prospect for our survival without hemoglobin molecules. The total volume of blood in the human body is about...
student question: 75 mL, of water and 0.10 moles of CO.(g) are added to a on vessel at 25 °C. A) What concentration of CO.(aq) do you expect to find at equilibrium? Henry's law constant-2 4x102 mol/L atm (12 pts) I mal-o B) Modified student question: If all the dissolved Co.(aq) reacts fully with water, then what is the pH of the water after equilibrium is reached? H2CO3 Kal = 4.2x10", Ka2-4.8×10-11. (12 pts) C) If you add CaCl2 to...
i need help with the last four questions along with
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he appropriate gas law to solve questions 1-6. Show work. (2 pts) A certain amount of a gas at a constant temperature has a pressure of 5.50 atm and a volume of 10.0 mL. If the volume is decreased to 125.0 mL, what is the resulting pressure of the gas? : 924 a4m 125 O P v (2 pts) If 0.722 L of a certain gas at...
b) The current (Year 2017) atmospheric CO2 concentration is 370 ppm. It is estimated that if we continue to exploit the world’s fossil fuel reserves at the same rate, the atmospheric CO2 concentration will reach 1,100 ppm in Year 2400 (Williams, 2001). Justify your answer in (1) quantitatively by calculating the pHs when CO2 concentrations are 370 ppm (Year 2017) and 1,100 ppm (Year 2400), respectively. Assuming: I. Pure water is in equilibrium with CO2 at 25oC. II. Water vapor...