A SodaStream "sparkling water" home carbonation system pressurizes a 1L water bottle to a pressure of 4 bar (400 kPa) in order to dissolve CO2 gas into the liquid to produce carbonated water also known as "Fizzy-Water". Small bubbles are injected to promote mass transfer such that we can assume the liquid-gas system is at equilibrium with water at a typical refrigerator temperature of 2 °C = 275 K. Assuming that both CO2 and water are ideal gases and CO2 is minimally soluble in water such that Henry's Law is an appropriate model for behavior, what mass of CO2 is dissolved in a 1L water bottle and what would be the equivalent volume, in liters, of that mass if released at room temperature of T = 298 K and pressure of 4 bar (during pressurization) and at 1 bar (when drinking the water)? Assume solvent MH20 18.015 kg/kmol, Psat@2c = 2 kPa == solute Mco₂ = 44.01 kg/kmol, Rco₂ = 0.1889 kPa m³/kgK, Hco₂ = 510 bar, Hint: The mass fraction and mole fraction of a mixture are related to each other by (where the subscript m is for "mixture"). = Mi mi = Wi mm Ni Mi NmMm Yi Mm

A SodaStream "sparkling water" home carbonation system pressurizes a 1L water bottle to a pressure of 4 bar (400 kPa) in order to dissolve CO2 gas into the liquid to produce carbonated water also known as "Fizzy-Water". Small bubbles are injected to promote mass transfer such that we can assume the liquid-gas system is at equilibrium with water at a typical refrigerator temperature of 2 °C = 275 K. Assuming that both CO2 and water are ideal gases and CO2 is minimally soluble in water such that Henry's Law is an appropriate model for behavior, what mass of CO2 is dissolved in a 1L water bottle and what would be the equivalent volume, in liters, of that mass if released at room temperature of T = 298 K and pressure of 4 bar (during pressurization) and at 1 bar (when drinking the water)? Assume solvent MH20 18.015 kg/kmol, Psat@2c = 2 kPa == solute Mco₂ = 44.01 kg/kmol, Rco₂ = 0.1889 kPa m³/kgK, Hco₂ = 510 bar, Hint: The mass fraction and mole fraction of a mixture are related to each other by (where the subscript m is for "mixture"). = Mi mi = Wi mm Ni Mi NmMm Yi Mm

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

A quantity of methyl acetate is placed in an open, transparent, three-liter flask and boiled long enough to purge all air from the vapor space. The flask is then sealed and allowed to equilibrate at 30°C, at which temperature methyl acetate has a vapor pressure of 269 mm Hg. Visual inspection shows 10 mL of liquid methyl acetate present.(a) What is the pressure in the flask at equilibrium? Explain your reasoning.(b) What is the total mass (grams) of methyl acetate in the flask? What fraction is in the vapor phase atequilibrium?(c) The above answers would be different if the species in the vessel were ethyl acetate because methyl acetate and ethyl acetate have different vapor pressures. Give a rationale for that difference.
Gas from a coal bed percolates up to the shallow, permeable strata containing groundwater. Methane (CH,, 16.0 g/mol) in the gas has a partial pressure of 0.029 bar. What is the concentration of methane in groundwater if ky is 23 g-bar-1-m-3?
A gas mixture contains 10.0 mole% H 2O(v) and 90.0 mole% N 2. The gas temperature and absolute pressure at the start of each of the three parts of this problem are 50°C and 500 mm Hg. Ideal-gas behavior may be assumed in every part of this problem.(a) If some of the gas mixture is put in a cylinder and slowly cooled at constant pressure, at what temperature would the first drop of liquid form?(b) If a 30.0-liter flask is filled with some of the gas mixture and sealed and 70% of the water vapor in the flask is condensed, what volume (cm 3 ) would be occupied by the liquid water? What would be the system temperature?(c) If the gas mixture is stored in a rigid-walled cylinder and a low-pressure weather front moves in and the barometric (atmospheric) pressure drops, which of the following would change: (i) the gas density, (ii) the absolute pressure of the gas, (iii) the partial pressure of water in the gas, (iv)the gauge pressure of the gas, (v) the mole fraction of water in the gas, (vi)…
Calculate the following: (a) The bubble-point temperature of an equimolar mixture of liquid n-hexane and n-heptane at 1.0 atm and the composition (mole fractions) of the vapor in equilibrium with this mixture. (b) The dew-point temperature of a gas mixture with a molar composition of 30% n-hexane, 30% n-heptane, and 40% air at 1 atm and the composition (mole fractions) of the liquid in equilibrium with this mixture.
Hydrogen gas can be produced from the reaction of graphite and steam according to the following reaction: C(s, graphite) + H20(g) = CO(g) + H2(g) K= 2.77x10-4 at 650 K 6.27 bar of gaseous H20 and excess graphite are added to a sealed container and then heated to 650 K. What is the partial pressure of gaseous H2, in units of bar, when the system reaches dynamic equilibrium? Your Answer: Answer Answer units
The sealed containers of fizzy drinks contain dissolved CO2. This dissolved CO2 is in equilibrium with a small quantity of gaseous CO2 at the top of the container. (a) The partial pressure of CO2 gas in a 250 cm3 can of fizzy drink is 3.0 atm at 25 0C. What is the concentration of CO2 in the fizzy drink? (b) If the can contain only the mass of CO2 1.09g as a gas, calculate the pressure in the can when it is stored at 25 0C. (c) The maximum pressure that a can of fizzy drink can withstand is 7 atm. Using the graph below, determine the maximum temperature at which a can, can be stored safely. (concentration=0.093M
A mixture consisting of 1-mol-% ethane, 5-mol-% propane, 44-mol-% n-butane, and 50-mol-% isobutane is brought to a condition of 294.15 K (21°C) at pressure P. If the molar fraction of the system that is vapor is 0.2, what is pressure P (in bar), and what are the compositions of the vapor and liquid phases?
3. Fe and FeQ are in equilibrium with gas mixture of composition 71.8% CO-28.2%CO2 at 1273K. Which of the two solid phases disappears if the composition of the gas is held constant and temperature of the system is increased? Fe(s)+1/2O2(g)=FeO(s) AG=-2 0=-263700+64.35T ammmm C(s)+O2 (g)= CO2(g) AG=-394100-0.84T C(s) + 1/2O2 (g) = CO AG=-111700-87.65T
4G 72% 4:37 = bartleby Q&A Science / Chemistry / Chemic... / 11th Ed... : A student determined the molar m... A A student determined the molar mass of an unknown non-dissociating liquid by the method described in this experiment. She found that the equilibrium temperature of a mixture of ice and pure water was indicated to be +0.4°C on her thermometer. When she added 9.9 g of her sample to the mixture, the temperature, after thorough stirring, fell to -3.7°C. She then poured off the solution through a screen into a beaker. The mass of the solution was 84.2 g. a. What was the freezing point depression? °C b. What was the molality of the unknown liquid? m c. What mass of unknown liquid was in the decanted solution? d. What mass of water was in the decanted solution?
kPa is the dissociation vapor 608 pressure of AB salt at 427°C and at 459°C it has increased to 1115 kPa. Find (a) Kp, (b) AG° at the two temperatures as well as AHO. Assume the ideal behaves of gases and the AH is independent on above temperature, also every latm. = 101.323 kPa. AB(s) == A(g) + B(g) a) Kp =9.00 , 30.27 , AG° = -12.97 KJ/mol, -20.75 KJ/mol, AH° = + %3D 50.44 KJ/mol b) Kp =50.00 , 30.27 , AG° = -22.97 %3D KJ/mol, -20.75 KJ/mol, AH° = + %3D
Given the following vapor composition plot for a mixture of cyclohexane and toluene, determine (a) the boiling temperature of a 0.60 mole fraction toluene liquid mixture and (b) the composition of the vapor.
In the gas phase reaction 2 A(g) + B(g) 3 C (g) + 2 D (g), it was found that when 1.00 mol A, 2.00 mol B and 1.00 mol D were mixed and allowed to come to equilibrium at 25°C, the resulting mixture contained 0.9 mol C at a total pressure of 1.00 bar. Calculate the mole fractions of each species , Kx is , Kp is and A GO is