K = [He] /pHe
3.70*10^-4 M/atm = [He]/1.1
[He] = 4.1*10^-4 M
Answer: 4.1*10^-4 M
Use Henry's law to determine the molar solubility of helium at a pressure of 1.1 atm...
Use Henry's law to determine the molar solubility of helium at a pressure of 1.3 atm and 25 ∘C. Henry’s law constant for helium gas in water at 25 ∘C is 3.70⋅10−4M/atm. I am having trouble figuring out the partical pressure of He is. I know that I use this equation: s=kp
please help I don't understand Using Henry's Law to calculate the solubility of a gas At 25.0 °C the Henry's Law constant for hydrogen sulfide (HS gas in water is 0.087 M/atm grams of HS gas that can be dissolved in 150. mL of water at 25.0 °C and a H,S partial pressure of 1.53 atm Calculate the mass Be sure your answer has the correct number of significant digits. X Check Explanation Using Henry's Law to calculate the solubility...
Number 5 sc Review | Constants 1 Per You may want to reference (Pages 582-585) section 13.4 while completing this problem Part A Use Henry's law to determine the molar solubility of hellum at a pressure of 20 atm and 25 °C. Henry's law constant for helium gas in water at 25°C is 3.70 - 10 Express your answer using two significant figures. M/atm. V AEROB? S-
The partial pressure of O2 in air at sea level is 0.21 atm. The solubility of O2 in water at 20 ∘C , at 1 atm gas pressure, is 1.38×10−3 M. Using Henry's law and the data in the introduction, calculate the molar concentration of O2 in the surface water of a mountain lake saturated with air at 20 ∘C and an atmospheric pressure of 660 torr .
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?
TUTOR Henry's Law Oxygen gas has a Henry's law constant of 1.66x10 M/mmHg at 25.0 °C when dissolving in water. If the total pressure of gas (O2 gas plus water vapor) over water is 1.00 atm, what is the concentration of O2 in the water in grams per milliliter? Pressure of the water vapor at 25.0 °C-23.8 mmHg. g/mL
Problem 3 [10 points] (a) Using the following table of Henry's law constants (kB(atm)-PB/XB) calculate the solubility (in M) of each gas in water at 25°C if PO2-0.2 atm , PNzー0.75 atm, and Pco2-0.05 atm Gas Temp. (25°c) N2 O2 CO2 85 × 103 43 × 103 1.61 x 103 b) What will the vapor pressure of water be in this solution if Raoult's law holds? The vapor pressure of pure water at this temperature is 23.756 torr
The Henry's law constant at 25 °C for CO₂ in water is 0.035 M/atm. What would be solubility of CO₂, in molarity units, be in 1.0 L of water when the partial pressure of CO₂ is 3.1 atm?
QUESTION 1 The following graph (fig. 10-7 from your textbook) displays the molar solubility of carbon dioxide at a pressure of 1.00 atm as a function of temperature. Methane 2.0 Oxygen (T/OU-01) Agnpos Carbon monoxide Nitrogen Helium 0 10 20 30 Temperature (°C) Read the graph to determine the molar concentration of carbon dioxide dissolved at 20 °C and 1 atm carbon dioxide pressure. Then use Henry's law to predict the molar concentration of carbon dioxide dissolved at 20 °C...
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...