At 25 °C and standard pressure, a hydrogen sulfide solution can be made by bubbling H,S(g) into water; the result is a 0.11 molarsolution. Since H2S(g) is more dense than air we can assume that a layer of pure H,S(g) at atmospheric pressure covers the solution.What is the value of Henry's law constant?kH=gL-latm 1iIs the solubility of H2S(g) much greater or smaller than nitrogen and oxygen? If so, suggest a reason for the difference.O Hydrogen sulfide is more soluble in water than nitrogen and oxygen, because hydrogen sulfide doesn't react with thewater.O Oxygen is more soluble in water than hydrogen sulfide, because oxygen reacts with the water to form peroxide.O Hydrogen sulfide is less soluble in water than nitrogen and oxygen.O Hydrogen sulfide is more soluble in water than nitrogen and oxygen, because hydrogen sulfide reacts with the water toform hydronium ions and HS.MacBook AirDIIDD888F7F6F10F3F42#%&

Since you have posted multiple questions as per guidelines we can answer one per session. If you…

At 25 °C and standard pressure, a hydrogen sulfide solution can be made by bubbling H,S(g) into water; the result is a 0.11 molar solution. Since H2S(g) is more dense than air we can assume that a layer of pure H2S(g) at atmospheric pressure covers the solution. What is the value of Henry's law constant? kH= gL-latm 1

At 25 °C and standard pressure, a hydrogen sulfide solution can be made by bubbling H,S(g) into water; the result is a 0.11 molar solution. Since H2S(g) is more dense than air we can assume that a layer of pure H2S(g) at atmospheric pressure covers the solution. What is the value of Henry's law constant? kH= gL-latm 1

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Which of the following phenomena is best described by Henry’s Law?a. Increasing temperature favors an endothermic process.b. The solubility of NaCl(s) in water increases with increasing temperature.c. The solubility of MgCl2(s) in water is unaffected by pressure.d. The vapor pressure of an aqueous solution of glucose, C6H12O6, is lower than the vapor pressure of pure water.e. The solubility of O2(g) in water increases with increasing pressure.
b) Write a definition of Henry's Law. Note: "Write a definition" implies that the answer should be in the form of a sentence. ii) The Henry's Law constant for the solubility of O₂ in water is 0.0013 mol/L*atm. Assume that the partial pressure of O₂ is 20 % of the total pressure. Calculate the solubility of O₂ in water at sea level (1.0 atm, 25 °C) and on top of Mt. Everest. Note: the 20% partial pressure of O₂ at 1 atm means that the pressure of O₂ at sea level is 0.20 atm (1.0 atm* 0.20 0.20 atm). The same reasoning needs to be applied to the pressure of O₂ on Mt. Everest. iii) Based on the solubility of O₂ in water on Mt. Everest, what would happen to the solubility of O₂ in the blood of an untrained mountain climber? action pr 5
At 25.0 °C the Henry's Law constant for hydrogen sulfide (H,S) gas in water is 0.087M/atm. Calculate the mass in grams of H,S gas that can be dissolved in 925. mL of water at 25.0 °C and a H,S partial pressure of 4.84 atm. Be sure your answer has the correct number of significant digits.
At 25.0 °C the Henry's Law constant for hydrogen sulfide (H, S) gas in water is 0.087M/atm. Calculate the mass in grams of H, S gas that can be dissolved in 1325. mL of water at 25.0 °C and a H, S partial pressure of 1.58 atm. Be sure your answer has the correct number of significant digits. x10
10.0 g ZnCl2 is dissolved in 100.0 g of water at 23.6 °C. The solution reaches a temperature of 36.5 °C. What is the molar heat of dissolution for ZnCl2? Assume the specific heat capacity of the solution is the same as pure water, 4.184 J/g·°C.
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? solubility: M At 298 K, what is the solubility of oxygen in water exposed to air at 0.893 atm? solubility: M If atmospheric pressure suddenly changes from 1.00 atm to 0.893 atm at 298 K, how much oxygen will be released from 3.20 L of water in an unsealed container? amount: mol
Magnesium chloride is often used to melt ice on sidewalks. Considering that the solubility of magnesium chloride (95.21 g/mol) in water is 54.3 g per 100.0 g of water, what is the lowest temperature that you would expect to be able to melt ice with magnesium chloride? Assume ideal behavior. (Kf(water)= 1.86°C/m) A. -29.2°C B. -31.8°C C. -25.0°C D. -10.6°C E. -41.0°C
What would be the theoretical freezing point of a solution made by dissolving 10.43 g of NiCl 2 in 365.0 g of water? The freezing point constant of water is 1.86 °C/molal. The molar mass of NiCl 2 is 129.5994 g/mol. 1.230 °C 1.506 °C 0.8128 °C -1.230 °C 1.022 °C
The partial pressure of CO2 gas above the liquid in a bottle of champagne at 20°C is 4.3 atm. What is the solubility of CO2 in champagne? Assume the Henry's law constant is the same for champagne as it is for water: at 20°C, kH = 3.7 × 10−2 mol/(L·atm).
2. Using the data in Appendix A of Benjamin's Water Chemistry, answer the following questions a. What is the Henry's law constant (KH) at 25 °C for the exchange of hydrogen sulfide between the gas and aqueous phases? H₂S (g) H₂S (aq) b. What is the Henry's law constant for the reaction in part a) at a temperature of 5 °C?
Complete combustion of 8.653 g of a compound of carbon, hydrogen, and oxygen yielded 21.83 g CO₂ and 3.831 g H₂O. When 18.00 g of the compound was dissolved in 288 g of water, the freezing point of the solution was found to be -0.952 °C. For water, Kfp = = 1.86 °C/m. What is the molecular formula of the compound? Enter the elements in the order C, H, O molecular formula =
Calculate the solubility of O2 in water at a partial pressure of O₂ of 150. torr at 25°C. The Henry's law constant for O₂ is 1.3 x 10-3 mol/L atm for Henry's law in the form C = KP, where C js the gas concentration (mol/L). Solubility= mol/L