Chapter 9

Polarizable

- the ability of an electron cloud to distort - outer electrons are held less tightly in larger atoms, so heavier atoms are more polarizable Having electrons that are easily displaced toward a positive charge. Polarizable atoms can begin to form a bond at a relatively long distance.

Ammonia, NH3, is used as a refrigerant. At its boiling point of -33 °C, the standard enthalpy of vaporization of ammonia is 23.3 kJ/mol. What is the enthalpy change when 50.0 g of ammonia is condensed at -33 °C?

-68.4 kJ

What is the change in enthalpy (in kJ) when 83.9 g of ethanol (mw=46.07) is condensed at its boiling temperature? (specific heat = 2.46 J/g°C, ΔHvap = 48.6 kJ/mol)

-88.5 Vaporization is an endothermic process so the sign is positive. Condensation is an exothermic process so the sign is negative.

Freon-113, C2Cl3F3, has an enthalpy of vaporization of 27.0 kJ/mol and a normal boiling point of 48.0 °C. What is the vapor pressure (in atm) of Freon-113 at 22.0 °C? (R = 8.314 J/K⋅mol)

0.41 atm

Rank the following intermolecular forces by their typical energies, where 1 is the highest energy attractions and 4 is the lowest energy of attraction. ion-dipole interaction hydrogen bonding dipole-dipole interaction London dispersion

1. ion-dipole interaction (highest energy/strongest attraction) 2. hydrogen bonding 3. dipole-dipole interaction 4. London dispersion (Weakest attraction)

A 250 gram sample of water at the boiling point had 24.0 kJ of heat added. How many grams of water were vaporized? At the boiling point, the heat of vaporization for water is 40.6 kJ/mole.

10.6

A liquid has a ΔHvap of 35.5 kJ/mol and a normal boiling point of 122degrees C. What is its boiling point at the top of Pike's peak, where the barometric pressure is 457 mmHg?

104 degrees C

Calculate the enthalpy of vaporization for a compound Z (mw = 86 g/mol) in kJ/mol if 448 kJ are required to vaporize 292 g of Z.

132

How much heat is absorbed when 5.00g of ice at -20.0°C is heated until it reaches the gas phase with a temperature of 140°C? Use the following date: csolid = 2.09 J/gK cliquid: 4.18 J/gK cgas: 2.00 J/gK ΔHvap= 40.7 kJ/mol ΔHfus= 6.02 kJ/mol

15.7 kJ

Below is a phase diagram for compound Y. The normal melting point of Y is most likely:

18 degrees

For a 3.91 gram sample of ice at 0.00°C , what is the minimum amount of heat (in kJ) needed to convert the sample to liquid water at 47.5°C? Physical data for water: specific heat (ice) = 2.10 J/g°C specific heat (water) = 4.184 J/g°C heat of fusion = 0.335 kJ/g heat of vaporization = 2.258 kJ/g Enter you value in decimal format using two decimals (value ± 2%)

2.09

For a 7.23 gram sample of water at 0.98°C , what is the minimum amount of heat (in kJ) needed to convert the sample to water at 87.4°C? Physical data for water: specific heat (ice) = 2.10 J/g°C specific heat (water) = 4.184 J/g°C heat of fusion = 0.335 kJ/g heat of vaporization = 2.258 kJ/g Enter you value in decimal format using two decimals (value ± 2%)

2.61

A 135 g sample of carbon disulfide requires 43.2 kJ of heat to vaporize completely. What is the enthalpy of vaporization for carbon disulfide?

24.4 kJ/mol

How much heat (in kJ) is required to raise the temperature of 200.8 g of ethanol (mw=46.07) from 11.5 °C to its boiling point of 78.37 °C and then vaporize it completely creating ethanol gas at the boiling temperature? (specific heat = 2.46 J/g°C, ΔHvap = 48.6 kJ/mol)

244.9 First the liquid is warmed then the liquid is vaporized. Therefore, it is a two step calculation. Remember to convert the specific heat to units of kJ/g°C.

What is the change in enthalpy (in kJ) when 26 g of ethanol (mw=46.07) is vaporized at its boiling temperature? (specific heat = 2.46 J/g°C, ΔHvap = 48.6 kJ/mol)

27.43 Vaporization is an endothermic process so the sign is positive. Condensation is an exothermic process so the sign is negative.

A 250 gram sample of water at the boiling point had 64.0 kJ of heat added. How many grams of water were vaporized? At the boiling point, the heat of vaporization for water is 40.6 kJ/mole.

28.4

What is the change in enthalpy (in kJ) when 45.4 g of ethanol (mw=46.07) is vaporized at its boiling temperature? (specific heat = 2.46 J/g°C, ΔHvap = 48.6 kJ/mol)

47.9 Vaporization is an endothermic process so the sign is positive. Condensation is an exothermic process so the sign is negative.

Which of the following compounds will only have London dispersion intermolecular attractions? NaCl CO2 CH3OH OCl2 CH3F

CO2

Which of the following compounds will only have London dispersion intermolecular attractions?{Hint: look for non-polar molecules}. OCl2 NaCl C3H7OH SiH4 CH3F

SiH4

The phase diagram for Xenon has a solid-liquid curve with a positive slope. Which of the following is true?

Solid Xenon has a higher density than liquid xenon.

Which of the following compounds will exhibits dipole-dipole attraction between molecules?{Hint: look for polar molecules.} CCl4 H2O SiS2 BF3 H2

H2O

Place the following substances in order of decreasing boiling point. H2O N2 CO2

H2O > CO2 > N2

Which of the following compounds will exhibits dipole-dipole attraction between molecules?{Hint: look for polar molecules.} SiO2 H2S CCl4 BCl3 BCl3 Cl2

H2S

Choose the substance with the highest viscosity. HOCH2CH2CH2CH2OH C2H4Cl2 (CH3CH2)2CO C6H14 CF4

HOCH2CH2CH2CH2OH

Predict which liquid has the highest viscosity: CH3CH2CH2CH3 CH3CH2OCH2CH3 HOCH2CH2CH2OH

HOCH2CH2CH2OH CH3CH2CH2CH3: nonpolar, london dispersions CH3CH2OCH2CH3: polar, dipole-dipole (O has 2 lone pairs) HOCH2CH2CH2OH: Hydrogen bonds has the strongest IMF (H bonded to O)

Which of the following liquids has the greatest viscocity? A. hexane (C6H14) B. CH3OCH2CH3 C. CH3CH2OCH2CH3 D. CH3CH2OH E. HOCH2CH2OH

HOCH2CH2OH

Which of the following liquids has the greatest viscocity? C6H14 CH3OCH2CH3 CH3CH2OCH2CH3 CH3CH2OH HOCH2CH2OH

HOCH2CH2OH

Compare the boiling points of the noble gases

He: 4K... Rn 211 K boiling point increases as you go down London dispersion forces are stronger when there are more electrons presents (heavier atoms)

Place the following substances in order of increasing vapor pressure at a given temperature. NF3 NH3 BCl3

NH3 < NF3 < BCl3

viscosity

a liquid's resistance to flow how "thick" a liquid is Stronger IMFs = higher viscosity

height

Patm - Pvap

Which of the following atoms should have the greatest polarizability? F, Br, Po, Pb, He

Pb

Which of the following atoms should have the smallest polarizability? Si, S, Te, Bi, Br

S

ion-dipole forces

attractive forces between an ion and a polar molecule EX: aqueous solutions

Which of the following pairs of substances is arranged so that the one with higher viscosity is listed first?

b.

liquid-gas line

boiling/condensing point

Liquid to gas

boiling/vaporization

If a pure substance begins at point C on the phase diagram below and the pressure on the substance is increased until point B is reached, what process occurs?

condensation

gas to liquid

condensation

Consider the phase diagram below. If the dashed line at 184 °C is followed from 0.50 to 100 atom, what phase changes will occur (in order of low pressure to high pressure)?

condensation, followed by freezing

c

constant that depends on the substance

convex

curved outward cohesive forces > adhesive

concave

curving inward adhesive forces > cohesive

adhesive forces

force of attraction between liquid and container (glass is polar)

Intermolecular forces

forces of attraction between molecules

liquid to solid

freezing

Consider the phase diagram below for pure substance X. The letters indicate specific points in the phase diagram. In going from point A to H to C, what phase transitions does X undergo?

fusion followed by evaporation

Consider the phase diagram below. If the dashed line at 1 atm of pressure is followed from 100 to 500 °C, what phase changes will occur (in order of increasing temperature)?

fusion, followed by vaporization

The phase diagram of a substance is shown below. What is the physical phase of the substance at T = 400 K and P = 2.0 atm?

gas

In condensed phases, kinetic molecular theory states that

gas molecules have no interactions

When you make ice cubes: a. it is an exothermic process b. it is an endothermic process c. the process is referred to scientifically as sublimation d. the heat of vaporization must be removed e. none of the above

it is an exothermic process

Based on the phase diagram below: What is the physical phase of the substance at T = 225 K and P = 1.1 atm?

liquid

Shown below is a phase diagram for compound Y. At 25°C and 1 atm Y will exist as a:

liquid

negative slope for solid-liquid line

liquid is more dense than the solid

temperature dependence of vapor pressure equation

ln(Pvap) = (-ΔHvap/R) (1/T) + c ln(P1/P2) = ΔHvap/R (1/T2 - 1/T1)

Which transition could occur if a solid is heated at a pressure above the triple point pressure?

melting

solid to liquid

melting

solid-liquid line

melting point/freezing point

metals are malleable

metal ions not tightly held in place, can slide through the electron sea

electrical/thermal conductivity of metals

metals are good conductors in the solid or liquid state-electrons are mobile

melting point of metals

moderate to high melting point increases across a period: higher charge = stronger attractions melting point decreases down a group: larger metal ions = weaker attraction to electron sea

Which best explains the following trend? Element b.p. (K) He 4 Ne 25 Ar 95 Kr 125 Xe 170 a. intramolecular forces b. dipole-dipole interaction c. hydrogen bonding d. Le Chatalier's principle e. none of these

none of these

Based on the phase diagram below, what phases can be present at 200°C and 0.75 atm pressure?

only the liquid phase

Hydrogen bonds

particularly strong dipole-dipole interactions in certain compounds

The reason that some insects can walk on water is due to a. vaporization b. surface tension c. weak adhesive forces d. low viscosity e. weak capillary action

surface tension

The tendency of a liquid that tends to minimize its surface area is called:

surface tension

Normal Melting/Boiling Points

surrounding pressure is 1 atm for normal BP: Pvap = 1 atm

vapor pressure increases as

temperature increases

Ion-Ion forces

the attraction between oppositely charged ions - holds ions together in ionic crystals classified more as "a bond" than an IMF

On a relative basis, the weaker the intermolecular forces in a substance,

the greater its vapor pressure at a particular temperature

On a relative basis, the weaker the intermolecular forces in a substance, A. the greater its heat of vaporization B. the more it deviates from ideal gas behavior C. the greater its vapor pressure at a particular temperature D. the higher its melting point E. none of these

the greater its vapor pressure at a particular temperature

stronger intermolecular forces

the higher the boiling point and melting point

Based on the phase diagram below, Based on the phase diagram below,

CB Line

How much energy (in kJ) is needed to convert 51.5 grams of ice at 0.00°C to water at 57.6 °C? specific heat (ice) = 2.10 J/g°C specific heat (water) = 4.184 J/g°C heat of fusion = 333 J/g heat of vaporization = 2258 J/g {Remember: a pure substance will either change phase or change temperature when heat is added, but not both at that same time}.

29.6 Since the ice is at 0° C, added heat caused it to melt to form liquid. After the ice completely melts the liquid then begins to warm. Therefore, it is a two step calculation.

For a 17.9 gram sample of ice at -81.1°C , what is the minimum amount of heat (in kJ) needed to convert the sample to ice at 0.00°C? Physical data for water: specific heat (ice) = 2.10 J/g°C specific heat (water) = 4.184 J/g°C heat of fusion = 0.335 kJ/g heat of vaporization = 2.258 kJ/g Enter you value in decimal format using two decimals (value ± 2%)

3.05

For a 17.9 gram sample of ice at -81.1°C , what is the minimum amount of heat (in kJ) needed to convert the sample to ice at 0.00°C? Physical data for water:specific heat (ice) = 2.10 J/g°Cspecific heat (water) = 4.184 J/g°Cheat of fusion = 0.335 kJ/gheat of vaporization = 2.258 kJ/g

3.05

For a 6.81 gram sample of ice at -69.8°C , what is the minimum amount of heat (in kJ) needed to convert the sample to liquid water at 0.00°C? Physical data for water:specific heat (ice) = 2.10 J/g°Cspecific heat (water) = 4.184 J/g°Cheat of fusion = 0.335 kJ/gheat of vaporization = 2.258 kJ/g

3.28

For a 8.24 gram sample of ice at -67.8°C , what is the minimum amount of heat (in kJ) needed to convert the sample to liquid water at 0.00°C? Physical data for water: specific heat (ice) = 2.10 J/g°C specific heat (water) = 4.184 J/g°C heat of fusion = 0.335 kJ/g heat of vaporization = 2.258 kJ/g

3.93

At its boiling point of 58.8 °C, 3.66 kJ of heat is required to vaporize 19.5 g of bromine (Br2). What is the molar enthalpy of vaporization of bromine?

30.0 kJ/mol

How much heat (in kJ) is required to raise the temperature of 302.3 g of ethanol (mw=46.07) from 18.53 °C to its boiling point of 78.37 °C and then vaporize it completely creating ethanol gas at the boiling temperature? (specific heat = 2.46 J/g°C, ΔHvap = 48.6 kJ/mol)

363.4 First the liquid is warmed then the liquid is vaporized. Therefore, it is a two step calculation. Remember to convert the specific heat to units of kJ/g°C.

At its boiling temperature, how much heat (in kJ) is needed to completely vaporize 23.4 g of H2O? The heat of vaporization for water at the boiling point is 40.6 kJ/mole.

52.8

How much heat (in kJ) is required to raise the temperature of 454.2 g of ethanol (mw=46.07) from 25.91 °C to its boiling point of 78.37 °C and then vaporize it completely creating ethanol gas at the boiling temperature? (specific heat = 2.46 J/g°C, ΔHvap = 48.6 kJ/mol)

537.8 First the liquid is warmed then the liquid is vaporized. Therefore, it is a two step calculation. Remember to convert the specific heat to units of kJ/g°C.

Diethyl ether has a ΔHvap of 29.1 kJ/mol and a vapor pressure of 0.703 atm at 25°C. What is its vapor pressure at 95°C?

6.56 atm

R

8.314 J/mol K

What is the change in enthalpy (in kJ) when 84 g of ethanol (mw=46.07) is vaporized at its boiling temperature? (specific heat = 2.46 J/g°C, ΔHvap = 48.6 kJ/mol)

88.6

From the data below, calculate the total heat in J when 0.333 mol of gaseous ethanol at 300°C and 1 atm is cooled to liquid ethanol at 25°C and 1 atm: BP at 1 atm: 78.5°C ΔHvao = 40.5 kJ/mol cgas = 1.43 J/gK cliquid = 2.45 J/gK

?

Assign the appropriate labels to the phase diagram shown below.

A = gas, B = solid, C = liquid, D = triple point

Based on molecular mass and dipole moment of the five compounds in the table below, which should have thelowest boiling point?

CH3CH2CH3

Which substance below has the strongest intermolecular forces? DX2, ΔHVAP = 23.3 kJ/mol C3X2, ΔHvap = 36.4 kJ/mol BY2, ΔHvap = 26.7 kJ/mol EY3, ΔHvap = 21.5 kJ/mol A2X, ΔHvap = 39.6 kJ/mol

A2X, ΔHvap= 39.6 kJ/mol

Which of the following liquids is expected have the highest surface tension at a given temperature? CH4 CF4 CCl4 CBr4 CH3Cl

CH3Cl

Place the following substances in order of increasing boiling point. Ar Cl2 O2

Ar < O2 < Cl2

Which one of the following substances will not have hydrogen bonding as one of its intermolecular forces? A. CH3COCH3 B. HOOH C. CH4CH2OH D. NH2NH2 E. CH3NH2

CH3COCH3 When you draw the Lewis structure, you are looking for a hydrogen bonded to an O, N, or F, and a lone pair on the electronegative atom.

Compare the boiling points of CO2 and COS. Which has the higher boiling point?

CO2 = nonpolar, only has London Dispersion forces COS = polar, net dipole towards the O london dispersion forces and dipole-dipole forces COS has the higher boiling point

In which of the following groups of substances would dispersion forces be the only significant factors in determining boiling points? I. Cl2 II. HF III. Ne IV. KNO2 V. CCl4

Cl2, Ne, CCl4

Choose the substance with the lowest boiling point. NBr3 H2O2 F2 H2S CF2H2

F2

Rank the halogen (X2) molecules from lowest to highest melting points

F2 < Cl2 < Br2 < I2 stronger IMFs = higher melting point heavier molecules = stronger london dispersion forces

Hydrogen bonding is a type of London dispersion force.

False

T/F: Dipole-dipole forces result from instantaneous dipoles that form in atoms and nonpolar molecules

False

T/F: Methane (CH4) exhibits stronger hydrogen bond interactions than ammonia (NH3).

False

T/F: The energy of a hydrogen bond is greater than that of a typical covalent bond.

False

When do you have hydrogen bonds?

In molecules with H-F, H-O, or H-N bonds EX: HF, H2O, CH3OH, NH3

What happens in condensed phases to real gases, liquids, and solids?

Interacting forces hold atoms and molecules together

Ranking of intermolecular forces from weakest to strongest

London Dispersion < Dipole-Dipole < Hydrogen Bonds

Attraction between an instantaneous dipole and an induced dipole on a neighboring atom or molecule, do to the distortion of the electron shape surrounding the atoms.

London dispersion

Neon atoms are attracted to each other by

London dispersion forces

What is the strongest (most attractive) intermolecular force in CF4?

London dispersion forces

Which of the following statements about liquids is true? a. The boiling point of a solution is dependent solely on the atmospheric pressure over the solution. B. Substances that can form hydrogen bonds will display lower melting points than predicted from periodic trends. C. Liquid rise within a capillary tube because of the small size lowers the effective atmospheric pressure over the surface of the liquid. D. London dispersion forces arise from a distortion of the electron clouds within a molecule or atom. E. Droplet formation occurs because of the higher stability associated with increased surface area

London dispersion forces arise from a distortion of the electron clouds within a molecule or atom.

Octane is a component of fuel used in internal combustion engines. The dominant intermolecular forces in octane are

London dispersion forces.

Condensation

The change of state from a gas to a liquid

vaporization

The change of state from a liquid to a gas

When a nonpolar liquid displays a convex meniscus, which of the following explains this behavior? a. it has a low surface tension, therefore clings to the glass b. The cohesive forces are stronger than the adhesive forces to the glass. c. The adhesive forces to the glass are stronger than the cohesive forces d. The liquid's viscosity is low. e. none of these

The cohesive forces are stronger than the adhesive forces to the glass.

Based on your knowledge of intermolecular forces and trends, select the statement that most accurately compares HCl and HBr.

The intermolecular attraction between HBr molecules are stronger than between HCl molecules mainly to due larger London dispersion forces.

Based on your knowledge of intermolecular forces and trends, select the statement that most accurately compares HCl and SiH4.

The intermolecular attraction between HCl molecules are stronger than between SiH4 molecules mainly to due larger dipole-dipole forces. HCl and SiH4 have approximately the same London dispersion forces, but only HCl has a dipole.

London dispersion forces

The intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles

surface tension

The resistance of a liquid to increase its surface area.

Consider the phase diagram shown. Choose the statement below that is TRUE. -at 10 atm of pressure, there is no temperature where the liquid phase of this substance would exist -the triple point of this substance occurs at a temperature of 31 degrees -the solid phase of this substance is higher in density than the liquid phase -the line separating the solid and liquid phases represents the ΔHvap -none of the above are true

The solid phase of this substance is higher in density than the liquid phase.

T/F: Intermolecular forces are weaker than intramolecular bonds

True

T/F: Intermolecular forces are weaker than intramolecular bonds.

True

T/F: Liquids with large intermolecular forces tend to have high surface tension.

True

supercooling

When you cool something below its normal freezing point and it does not freeze it takes some period of time for the molecules to organize and solidify

A supercritical fluid refers to a substance - at its triple point - that is in the liquid crystal state - with a viscosity of zero - above both its critical temperature and its pressure

above both its critical temperature and its critical pressure.

The rate of vaporization of a liquid can be increased by 1. increasing the surface area 2. increasing the temperature 3. decreasing the strength of the intermolecular forces

all of the above

Which molecule below has hydrogen bonding? a. CH3CH2OH b. CH3NH2 c. H2O d. HF e. all of the above

all of the above

Which statements about viscosity are true? (i) Viscosity increases as temperature decreases. (ii) Viscosity increases as molecular weight increases. (iii) Viscosity increases as intermolecular forces increase.

all of the above

what compounds have london dispersion forces?

all of them; anything with electrons

The triple point of iodine is at 90 torr and 115°C. This means that liquid I2 - is more dense than I2(s) - cannot have a vapor pressure less than 90 torr - can exist at pressure of 10 torr d. cannot exist at 1 atm e. cannot exist above 115 degrees C

cannot have a vapor pressure less than 90 torr

intermolecular forces have nothing to do with

chemical bonds

Based on the slope of the BC line segment, the solid phase ________.

is more dense than the liquid phase.

Attractions between oppositely charged ends of two or more polar molecules.

dipole-dipole

What is the strongest (most attractive) intermolecular force in PCl3?

dipole-dipole attraction

In hydrogen iodide __________________ are the most important intermolecular forces.

dipole-dipole forces

enthalpy of vaporization

enthalpy change associated with vaporizing 1 mole of substance always endothermic (+)

enthalpy of melting point

enthalpy of fusion endothermic

associated enthalpy of boiling point

enthalpy of vaporization (ΔHvap)

boiling point of metals

high difficult for cations and valence electrons to break away from the others

The critical temperature of a substance is the -temperature above which the compound decomposes -temperature at which sublimation occurs -highest temperature at which the liquid phase can exist in equilibrium with the gas phase -temperature at which all three phases can exist in equlibrium

highest temperature at which the liquid phase can exist in equilibrium with the gas phase.

Attraction between a partially positively charged H-atom attached to a highly electronegative atoms (i.e. N, O, or F) and the lone pair of another electronegative atom.

hydrogen bond

Ammonia's unusually high melting point is the result of

hydrogen bonding

The strongest intermolecular interactions between ethyl alcohol (CH3CH2OH) molecules arise from

hydrogen bonding

The strongest intermolecular interactions between hydrogen fluoride (HF) molecules arise from

hydrogen bonding

What is the strongest (most attractive) intermolecular force in methanol, CH3OH?

hydrogen bonding

To convert liquid water into steam, you must break

hydrogen bonds

To convert liquid water into steam, you must break a. ionic bonds 2. nonpolar covalent bonds 3. polar covalent bonds 4.hydrogen bonds e. none of these

hydrogen bonds

cohesive forces

intermolecular forces of the liquid itself

dipole-dipole forces

intermolecular forces that exist between polar molecules. Active only when the molecules are close together. The strengths of intermolecular attractions increase when polarity increases

Attraction between a charged ion and the end of a dipole with the opposite partial charge.

ion-dipole

What is the dominant attractive force in MgF2?

ionic bonding

What is the dominant attractive force in NaNO3?

ionic bonding

What is the dominant attractive force in RbBr?

ionic bonding

critical point

point where vapor can no longer be liquifided beyond this point, the liquid and gas phases are indistiguishable and exist as a superficial fluid

When the electron cloud of a molecule is easily distorted, the molecule has a high _____________. A. polarity B. polarizability C. dipole moment D. van der Waals radius E. compressibility

polarizability

Sublimation

process of converting a solid directly into a gas.

Based on the phase diagram below: What is the physical phase of the substance at T = 100 K and P = 0.1 atm?

solid

positive slope for solid-liquid line

solid is more dense than liquid

Which of the following factors contributes to a low viscosity for a liquid? A. low temperature B. spherical molecular shape C. hydrogen bonding D. high molecular weight E. high boiling point

spherical molecular shape

capillary action

spontaneous rising of a liquid in a glass tube

relationships between IMFs and ΔHvap

stronger IMFs = larger ΔHvap

relationship between IMFs and vapor pressure

stronger IMFs = lower vapor pressure

triple point

the point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another

superheating

the process of heating a liquid above its boiling point without its boiling -uneven heating -surface tension

The meniscus of mercury in a glass capillary tube is convex because of

the smaller attraction of mercury atoms to the glass than to each other.

melting point

the temperature at which the vapor pressures of the solid and liquid are equal

boiling point

the temperature at which vapor pressure is equal to atmospheric pressure T when Pvap = Patm

What is responsible for capillary action, a property of liquids? A. viscosity B. two of these C. surface tension D. adhesive forces E. cohesive forces

two of these: adhesive forces & cohesive forces

Enthalpy of condensation

ΔHcond = (-)ΔHvap