The commercially available charger for soda water siphon contains 8 gram of carbon dioxide CO2 After being dispensed to the standard siphon with volume 0.7 L partially filled with water, the pressure of CO2 inside the siphon is 6 atm Using the Henry law, estimate the molar concentration of CO2 in the carbonated water produced by such siphon at 25 °C. 4)

The commercially available charger for soda water siphon contains 8 gram of carbon dioxide CO2 After being dispensed to the standard siphon with volume 0.7 L partially filled with water, the pressure of CO2 inside the siphon is 6 atm Using the Henry law, estimate the molar concentration of CO2 in the carbonated water produced by such siphon at 25 °C. 4)

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

Lithium chloride has a solubility of 45.80 g in 100. g of water at 25°C. Express this solubility in terms ofmass percent molality mole fraction
A nonvolatile solute is dissolved in benzene and the resulting solution has a vapor pressure of 18.7 torr. What is the mole fraction of the solute? (P° of benzene is 26.5 torr).
7) A 300.0 mL aqueous solution containing 0.512 g of an unknown polymer has an osmotic pressure of 32.9 torr at 29.5°C. What is the molar mass of the polymer? 29.5°C +273 =303.5K
The colligative molality of seawater is approximately 1.10 m. Calculate the vapor pressure of sea water at 20 °C. The vapor pressure of pure water at 20 °C is 17.54 Torr.
The Rast camphor method is a cryoscopic technique for molar mass determination. Exactly 1.00 g of an isoprenoid of known formula (C5H8)n was dissolved in 5.00 g of camphor. The freezing point of the resulting solution decreased by 27.7 ℃ relative to pure camphor. Knowing that the Kf of camphor is 37.7 deg·kg/mol: Calculate for the molar mass of the isoprenoid. Calculate the value of n in the given formula of the isoprenoid. Report in whole number. The normal freezing point of camphor is 178.4 ℃. At what temperature did the isoprenoid-camphor solution freeze?
Consider a body of water in equilibrium with solid calcium sulfate, CaSO4, for which Ksp = 3.0 * 10^-5 at 35 degrees C. Calculate the solubility, in g/L of calcium sulfate in water assuming that other reactions are negligible.
The solubility of Ne in water at 25 °C is 2.1 × 10⁻⁴ M when the partial pressure of Ne is 0.20 atm. What is the value of the Henry's law constant for Ne?
At 45 °C, a solution is prepared by mixing 48.0 g Na2SO4 with 240.0 g water. The vapor pressure of water at 45 °C is 71.9 torr. Assuming total dissociation of the salt, determine: (a) mole fraction of Na2SO4; (b) mole fraction of water; (c) vapor pressure of the solution. (molar mass, g/mol: Na2SO4= 142.04; water = 18.02) (a) XNa2s04 = (b) Xwater = (d) Psoln =
Calculate the solubility of O, in water at a partial pressure of O2 of 120 torr at 25°C. The Henry's law constant for 0, is 1.3 x 10-8 mol/L· atm for Henry's law in the form C= kP, where Cis the gas concentration (mol/L).
L 16
It says the answer should be 22.98 torr but I have no clue how to reach the answer. Any hints are great. Thanks!
The organic compounds chloroform and dichloromethane form ideal solutions when mixed together; at 25 �C the total vapor pressure from a mixture of these two compounds was 345.322 torr. What is the mole fraction of chloroform? Given that the vapor pressure of pure chloroform and pure dichloromethane are 205 torr and 415 torr, respectively, at 25�C. 0.6682 0.4430 0.3318 0.5570