Principles of Modern Chemistry
8th Edition
ISBN: 9781305079113
Author: David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Related questions
Question
PLEASE ANSWER ALL PARTS!!!
![7.66 (a) Consider a two-phase system, where one phase is pure
liquid A and the second phase is an ideal gas mixture of A vapor
with inert gas B (assumed insoluble in liquid A). The presence of
gas B changes μA, the chemical potential of liquid A, because B
increases the total pressure on the liquid phase. However, since
the 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 vapor
pressure of A. Imagine an isothermal infinitesimal change dP in
the total pressure P of the system. Show that this causes a change
dPA in the vapor pressure of A given by
А
dPA
V¹m.A
Vm.APA
const. T
(7.38)
dP
V8
m,A
RT
Equation (7.38) is often called the Gibbs equation. Because V
m,A'
m,A
is 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. Calculate
the vapor pressure of water at 25°C in the presence of 1 atm of
inert ideal gas insoluble in water.](https://content.bartleby.com/qna-images/question/9d7dc701-b654-4339-995f-9e7ccdd48dfe/3a6c3d0f-280a-47e8-8de4-ac5a060f31b0/3hqd3d_processed.png)
Transcribed Image Text:7.66 (a) Consider a two-phase system, where one phase is pure
liquid A and the second phase is an ideal gas mixture of A vapor
with inert gas B (assumed insoluble in liquid A). The presence of
gas B changes μA, the chemical potential of liquid A, because B
increases the total pressure on the liquid phase. However, since
the 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 vapor
pressure of A. Imagine an isothermal infinitesimal change dP in
the total pressure P of the system. Show that this causes a change
dPA in the vapor pressure of A given by
А
dPA
V¹m.A
Vm.APA
const. T
(7.38)
dP
V8
m,A
RT
Equation (7.38) is often called the Gibbs equation. Because V
m,A'
m,A
is 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. Calculate
the vapor pressure of water at 25°C in the presence of 1 atm of
inert ideal gas insoluble in water.
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by stepSolved in 2 steps with 3 images
Knowledge Booster
Similar questions
- 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=0.093Marrow_forwardThe 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)arrow_forwardThe 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?arrow_forward
- 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 -394arrow_forwardOsmotic 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/mLarrow_forwardHenry’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?arrow_forward
- 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¬!.arrow_forwardState 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.arrow_forwardAt 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)?arrow_forward
- 6.35 If 68.4 g of sucrose (M 342 g mol-¹) is dissolved in 1000 g of water, (a) what is the vapor pressure at 20 °C? (b) What is the freezing point? The vapor pressure of water at 20°C is 2.3149 kPa. =arrow_forwardQuestion 5 5.1 The normal boiling temperature of benzene is 353.24 K and the vapour pressure of liquid benzene is 1.19x104 Pa at 20 °C. (a) Calculate AyapH (kJ.mol) for benzene. (b) What is the AvapS for benzene in kJ.mol-!? 5.2 Water boils at 100 °C at 1 atm and its enthalpy of vaporization is 40.7 kJ.mol. In some chemistry experiment, it is desired that the water boils at temperature of 89 °C. Calculate what external pressure should be (in atm) in this case.arrow_forward13.21 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?arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning
Principles of Modern Chemistry
Chemistry
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:Cengage Learning