Chem Final:

Front 1

the internal energy of a system increased by___.

Back 1

volume compression

Front 2

When a system ___, delta E is always negative.

Back 2

absorbs heat and does work

Front 3

___solids consist of atoms or molecules held together by dipole-dipole forces, London dispersion forces, and/or covalent network

Back 3

ionic

Front 4

a real gas will behave most like an ideal gas under condition of_____.

Back 4

low temperature and high pressure

Front 5

of the following, ___ is a valid statement of Charles' law:

Back 5

V= constantX P

Front 6

the strongest inter particle attractions exist between particles of ___ and the weakest inter article attractions exist between particles of a ___.

Back 6

solid, gas

Front 7

A gas is___ and assumes___ of its container whereas a liquid is ___ and assumes ___ of its container.

Back 7

condensed, the volume and shape, condensed, the volume and shape

Front 8

the property responsible for the "beading up" of water is ____

Back 8

hydrogen bonding

Front 9

in which of the following molecules is hydrogen bonding most likely to e the most significant component of the total intermolecular forces?

A) CH4 B) C6H13NH2

c) CO2 D) C5H11OH

E) CH3OH

Back 9

C5H11OH

Front 10

in general, the vapor pressure of a substance increases as _____ increases

Back 10

hydrogen bonding

Front 11

crystalline solids differ from amorphous solids in that crystalline solids have_____

Back 11

a long range repeating pattern of atoms, molecules, or ions.

Front 12

Of the following substances only __ has London dispersion forces as its ONLY intermolecular force.

A) NH3 B) CH3OH C) HCL D) CH4 E) H2S

Back 12

HCL

Front 13

as a solid element melts, the atom become ___ and they have ____ attraction for one another.

Back 13

more separated, less

Front 14

A solid has a very high melting point, great hardness, and poor electrical conduction. This is a(n) ___ solid.

Back 14

metallic and covalent network

Front 15

Elemental iodine is a solid at room temperature. what is the major attractive force that exists among different iodine molecules in the solid?

Back 15

London dispersion forces

Front 16

which one of the following exhibits dipole dipole attraction between molecules?

A) AsH3 B) Cl2 C) CO2 D) BCl3 E) XeF4

Back 16

XeF4

Front 17

metallic solids do not exhibit:

Back 17

excellent thermal conductivity

Front 18

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.

Back 18

(ii) and (iii)

Front 19

of the following which is the weakest acid?

Back 19

HIO2

Front 20

in the gas phase reaction, NH3 is acting as a(n) _____ base but not as a(n)____ base.

Back 20

Arrhenius, Lewis

Front 21

of the following acids, ___ is not a strong acid:

A) H2SO4 B) HCL C) HNO2 D) HCLO4 E) HNO3

Back 21

HNO3

Front 22

which of the following is a bronsted-lowry acid:

A) HF B) CH3COOH C) (CH3)3NH+

D) HNO2 E) all of the above

Back 22

HF

Front 23

A Bronsted-lowry base is defined as a substance that ______

Back 23

acts as a proton acceptor

Front 24

which on of the following is the weakest acid:

A) HNO2 (Ka= 4.5X10^-4)

B) HClO (Ka=3.0X10^-8)

C) HCN (Ka= 4.9X10^-10)

D) HF (Ka= 6.8X10^-4)

E) Acetic Acid (Ka= 1.8X10^-5)

Back 24

HNO2 (Ka= 4.5X10^-4)

Front 25

Le Chateliers principle predicts that ___ will result in an increase in the number of moles of SO3(g) in the reaction container.

Back 25

decreasing the pressure

Front 26

at equilibrium, ______.

Back 26

the value of the equilibrium constant is 1

Front 27

how is the reaction quotient used to determine whether a system is at equilibrium?

Back 27

at equilibrium, the reaction quotient is undefined.

Front 28

which of the following aqueous solution has the highest [OH-]

Back 28

a solution with oH of 3.0

Front 29

le chateliers principle predicts that an increase in temperature will result in _____?

Back 29

no changes in equilibrium partial pressure.

Front 30

In the arrhenius equation: K=Ae^-Ea/RT

______ is the frequency factor.

Back 30

K

Front 31

of the following, all are valid units for a reaction rate except_____.

A) mol/L-hr B) mol/hr C) M/s D)mol/L E) g/s

Back 31

A) mol/L-hr

Front 32

_____ are used in automotive catalytic conveyers.

Back 32

homogeneous catalysts

Front 33

A 25.0 mL sample of an unknown solution compound is titrated with a 0.115M NaOH solution. The titration curve above was obtained. The unknown compound is _____

Back 33

strong acid

Front 34

what change will be caused by addition of small amount of HCL to a solution containing fluoride ions and hydrogen fluoride ?

Back 34

the concentration of fluoride ions will increase as will the concentration of hydronium ions.

Front 35

a catalyst can increase the rate of reaction _____.

Back 35

by increasing the overall activation energy (Ea) of the reaction

Front 36

of the following, which is the strongest acid?

A) HIO

B) HIO4

C) HIO2

D) HIO3

E) the acid strength of all of the above is the same.

Back 36

HIO

Front 37

a solution containing which one of the following pairs of substances will be a buffer solution?

A) NaI, HI

B) RbCl, HCL

C) KBr, HBr

D) CsF, HF

E) None of the above

Back 37

E) none of the above

Front 38

the mechanism for formation of the product X:

A+B---> C+D (slow)

B+D---> X (Fast)

the intermediate reactant in the reaction is _____

Back 38

D

Front 39

as the temperature of a reaction is increased, the rate of the reaction increases because the ____.

Back 39

reactant molecules collide more frequently and with greater energy per collision.

Front 40

the rate law of the overall reaction

A+B--->C

is rate = K[A]^2. Which of the following will Not increase the rate of reaction?

Back 40

increasing the temperature of the reaction

Front 41

which of the following is true?

Back 41

since intermediate compounds can be formed, the chemical equations for the elementary reactions in a multistep mechanism do not always have to add to give the chemical equation of the overall process

Front 42

in the energy profile of a reaction, the species that exists at the maximum on the curve is called the _____.

Back 42

enthalpy of reaction

Front 43

which one of the following conditions would always result in an increase in the internal energy of a system?

Back 43

the system gains heat that has work done on it by the surroundings

Front 44

of the following which is a state function?

A) w B) H C) q D) heat E) none of the above

Back 44

B) H

Front 45

A _____ delta H corresponds to an ___ process

Back 45

negative, exothermic

Front 46

a chemical reaction that absorbs heat from the surroundings is said to be___ and has a ___ Delta H at constant pressure

Back 46

endothermic, positive

Front 47

the units of heat capacity are ____

Back 47

J/K or J/g-degree C

Front 48

which of the following is a statement of Hess's Law

Back 48

if a reaction is carried out in a series of steps, the delta H for the reaction will equal the sum of the enthalpy changes for the individual steps

Front 49

with references to enthalpy changes, the term standard conditions means____.

A) P=1 atm

B) some common temperatures, usually 298K

C) V=1L

A) a only B) b only C) c only D) a&c E) a&b

Back 49

E) a&b

Front 50

which of the following statements about gases is false?

Back 50

all gases are colorless and odorless at room temperature

Front 51

one significant difference between gases and liquids is that______

Back 51

a gas assumes the volume of its container

Front 52

which of the following equations shows an incorrect relationship between pressures given in terms or different units?

A) 0.760 atm = 578 mmHg

B) 1.0 torr = 2.00 mmHg

C)1.00 atm= 760 torr

D) 1.20 atm = 122 kPa

E) 152 mmHg = 2.03X10^4 Pa

Back 52

1.0torr=2.00mmHg

Front 53

of the following, only ____ is impossible for an ideal gas.

A) V1/V2= T1/T2=0

B) V1/T1=V2/T2

C) V1/V2=T1/T2

D) V2=(T2/T1)V1

E) V1T1=V2T2

Back 53

E) V1T1=V2T2

Front 54

the average kinetic energy of the particles of a gas is directly Proportional to ______.

Back 54

the square of the rms speed

Front 55

the kinetic molecular theory predicts that pressure rises as the temperature of gas increases because______.

Back 55

both the gas molecules collide more frequently with the wall and the gas molecules collide more energetically with the wall

Front 56

Arrange the following gases in order of increasing average molecular speed at 25 C

He, O2, CO2, N2

Back 56

CO2

Front 57

a real gas will behave most like an ideal gas under conditions of ______.

Back 57

high temperature and low pressure.

Front 58

hydration is a specific example of the phenomenon known generally as ____

Back 58

solcation

Front 59

the dissolution of gases in water is virtually always exothermic because_____

Back 59

ine of the two endothermic steps ( separation of solute particles) in the solution- formation process in unnecessary

Front 60

the phrase " like dissolves like" refers o the fact that _____

Back 60

polar solvents dissolve polar solutes and non-polar solvents dissolve non-polar solutes

Front 61

a saturated solution ______.

Back 61

contains dissolved solute n equilibrium with undissolved solute.

Front 62

in a saturated solution of a salt in water, ______.

Back 62

the rate of crystallization = the rate of dissolution

Front 63

the principle reason for the extremely low solubility of NaCl in benzene is the ____

Back 63

weak salvation of Na+ and Cl- by C6H6

Front 64

which one of the following substances would be the most soluble in CCl4?

A) H2O B) Ch3Ch2OH C) NaCl D) C10H22

E) NH3

Back 64

C10H22

Front 65

which of the following substances is more likely to dissolve in water?

Back 65

HOCH2CH2OH

Front 66

which on of the following substances is more likely to dissolve in benzene (C6H6)

A) CH3CH2OH

B) CCl4

C) NH3

D) HBr

E) NaCl

Back 66

B) CCl

Front 67

which on of the following is most soluble in hexane (C6H14)

A) CH3CH2OH

B) CH3CH2CH2CH2OH

C) CH3CH2CH2CH2CH2OH

D) CH3OH

E) CH3CH2CH2OH

Back 67

C) CH3CH2CH2CH2CH2OH

Front 68

which of the following statements is false?

Back 68

the weaker the attraction between molecules the solute and solvent molecules, the greater the solubility.

Front 69

calculate the molarity of a 17.5%(by mass) aqueous solution of nitric acid.

Back 69

the density of the solution is needed to solve the problem

Front 70

a solution contains 15 ppm of benzene. the density of the solution is 1.00g/ml. this means that ______.

Back 70

there are 15mg of benzene in a 1.0L of this solution

Front 71

A 0.1oom solution of which one of the following solutes will have the lowest vapor pressure.

Back 71

Al(ClO4)3

Front 72

a 1.35m aq solution of compound X had a boiling point of 101.4 C. which on elf the following could be compound X? the boiling point elevation constant for water is 0.52C/m.

Back 72

KCL

Front 73

the ideal value of i (cant hoff factor) for (NH4)3PO4.

Back 73

4

Front 74

which of the following cannot be a colloid

Back 74

homogenous mixture

Front 75

WHICH ONE OF THE FOLLOWING SUBSTANCES WOULD BE THE MOST SOLUBLE IN CCl4

Back 75

C10H22

Front 76

a reaction that is spontaneous as written_____.

Back 76

will proceed without outside intervention

Front 77

which one of the following is always positive when a spontaneous process occurs?

Back 77

delta S universe

Front 78

Formation of solutions where the process is endothermic can be spontaneous provided that ______>

Back 78

they are accompanied by an increase in disorder

Front 79

Consider pure crystalline solid that is heated from absolute zero to a temperature above the boiling point of the liquid. which of the allowing processes produces the greatest increase in the entropy of the substance?

Back 79

vaporizing the liquid

Front 80

a0.100m solution of which of the following solutes will have the highest vapor pressure?

Back 80

sucrose

Front 81

which of the following choices has the compounds correctly arranged in order of increasing solubility in water? (least to most soluble )

Back 81

CCl4< CHCl3<NaNO3

Front 82

of the following in a 0.1M aq solution of ____ will have the lowest freezing point.

Back 82

AL(NO3)3

Front 83

which of the following statements is true?

Back 83

spontaneity can depend on the temperatures

Front 84

which of the following usbtances is more likely to dissolve in benzene (C6H6)

A) CH3Ch2OH

B) NH3

C) NaCl

D) HBr

E) CCl4

Back 84

E) CCl4

Front 85

delta S is positive for the reaction _____.

A) BaF2(s)---> Ba2+(aq) +2F-(aq)

B) 2NO2(g)--->N2O3(g)

C) 2H2(g)+ O2(g)--> 2H20(g)

Back 85

A) BaF2(s)---> Ba2+(aq) +2F-(aq)

Front 86

the largest value of henrys constant for the liquid solvent H2O will be obtained with ____ gas as the solute and a temperature of _____ degree C.

Back 86

HCL, 49

Front 87

Calculate the molarity of a 25.4 %(by mass) aq solution of phosphoric acid (H3PO4).

Back 87

the density of this solution is needed to solve the problem.

Front 88

the principle reason for the extremely low solubility of NaCL in benzene (C6H6) is the ____.

Back 88

weak salvation of NA+ and CL- by C6H6

Front 89

in a saturated solution of a salt in water, _____.

Back 89

the rate of crystallization = the rate of dissolution.