PLEASE ANSWER ALL PARTS!!! 7.66 (a) Consider a two-phase system, where one phase is pureliquid A and the second phase is an ideal gas mixture of A vaporwith inert gas B (assumed insoluble in liquid A). The presence ofgas B changes μA, the chemical potential of liquid A, because Bincreases the total pressure on the liquid phase. However, sincethe vapor is assumed ideal, the presence of B does not affect μg,the chemical potential of A in the vapor phase [see Eq. (6.4)].Because of its effect on μ¼, gas B affects the liquid-vapor equi-librium position, and its presence changes the equilibrium vaporpressure of A. Imagine an isothermal infinitesimal change dP inthe total pressure P of the system. Show that this causes a changedPA in the vapor pressure of A given byАdPAV¹m.AVm.APAconst. T(7.38)dPV8m,ARTEquation (7.38) is often called the Gibbs equation. Because Vm,A'm,Ais much less than Vg the presence of gas B at low or moder-ate pressures has only a small effect on the vapor pressure of A.(b) The vapor pressure of water at 25°C is 23.76 torr. Calculatethe vapor pressure of water at 25°C in the presence of 1 atm ofinert ideal gas insoluble in water.

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Answered: 7.66 (a) Consider a two-phase system,…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter11: Solutions

Section: Chapter Questions

Problem 46P

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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
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 calculated in part (ii) 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)
The Henry’s law constant for CO2 in water at 25 °C is3.1x 10-2 M atm-1. (a) What is the solubility of CO2 inwater at this temperature if the solution is in contact withair at normal atmospheric pressure? (b) Assume that all ofthis CO2 is in the form of H2CO3 produced by the reactionbetween CO2 and H2O:CO2(aq) + H2O(l)------>H2CO3(aq)What is the pH of this solution?
What is AG for the decomposition of CaCO3 at 298 K and a partial pressure of CO2 of 4.00x10-4 bar? CaCO3(s) → CaO(s) + CO2(g) AGrxn (298 K, Pco2 = 0.400 mbar) = ??? CO2(g) Compound AG°; (kJ mol·1) CACO3(s) СаО(s) -1129 -604 -394
Osmotic pressures are often reported in units of atmospheres or mm Hg. The latter impliesthat the height of a column of liquid can be used as a measure of pressure. This is, in fact, thebasis of the torricellian barometer from which the units of “torr” come. The pressure, P, isrelated to the height of the column by:P = ρghwhere ρ is the density of the liquid, g is the acceleration due to gravity and h is the height. Whatwill be the height (in mm) of a column of aqueous solution with a density of 0.9987 g/mL, if theosmotic pressure of the solution at 25 °C is 1.4 mm Hg? The density of mercury at thistemperature is 13.8 g/mL
Henry’s law constant for CO2 in the water at 25 °C is 3.1 * 10-2 M atm-1. (a) What is the solubility of CO2 in the water at this temperature if the solution is in contact with air at normal atmospheric pressure?
2.28(b) Set up a thermodynamic cycle for determining the enthalpy of hydration of Ca?+ ions using the following data: enthalpy of sublimation of Ca(s), +178.2 kJ mol-1; first and second ionization enthalpies of Ca(g), 589.7 kJ mol-1 and 1145 kJ mol¬1; enthalpy of vaporization of bromine, +30.91 kJ mol-1; dissociation enthalpy of Br,(g), +192.9 kJ mol-1; electron gain enthalpy of Br(g), –331.0 kJ mol-1; enthalpy of solution of CaBr,(s), –103.1 kJ mol-'; enthalpy of hydration of Br¯(g), –337 kJ mol¬!.
State whether the entropy of the system increases or de-creases in each of the following processes:(a) Pure gases are mixed to prepare an anesthetic.(b) Electronic-grade silicon is prepared from sand.(c) Dry ice (solid CO₂) sublimes.
At 20 °C, the vapor pressure of benzene (C6H6) is 75 torr,and that of toluene (C7H8) is 22 torr. Assume that benzeneand toluene form an ideal solution. (a) What is thecomposition in mole fraction of a solution that has a vaporpressure of 35 torr at 20 °C? (b) What is the mole fractionof benzene in the vapor above the solution describedin part (a)?
13.21 Two nonpolar organic liquids, hexane (C6H14) and heptane (C7H16), are mixed. (a) Do you expect AHsoln to be a large positive number, a large negative number, or close to zero? Explain. (b) Hexane and heptane are miscible with each other in all proportions. In making a solution of them, is the entropy of the system increased, decreased, or close to zero, compared to the separate pure liquids?
State whether the entropy of the system increases or decreases in each of the following processes:(a) Gasoline burns in a car engine.(b) Gold is extracted and purified from its ore.(c) Ethanol (CH3CH2OH) dissolves in 1-propanol (CH3CH2CH2OH).
The following table presents the solubilities of severalgases in water at 25 °C under a total pressure of gas andwater vapor of 1 atm. (a) What volume of CH4(g) understandard conditions of temperature and pressure is containedin 4.0 L of a saturated solution at 25 °C? (b) Thesolubilities (in water) of the hydrocarbons are as follows:methane < ethane < ethylene. Is this because ethyleneis the most polar molecule? (c) What intermolecularinteractions can these hydrocarbons have with water?(d) Draw the Lewis dot structures for the three hydrocarbons.Which of these hydrocarbons possess p bonds?Based on their solubilities, would you say π bonds aremore or less polarizable than s bonds? (e) Explain whyNO is more soluble in water than either N2 or O2. (f) H2S is more water-soluble than almost all the other gasesin table. What intermolecular forces is H2S likely to havewith water? (g) SO2 is by far the most water-soluble gasin table. What intermolecular forces is SO2 likely to havewith…

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