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Chemistry 2 Final > Chemistry 2 Final > Flashcards

Chemistry 2 Final Flashcards

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1
Q

Internal energy of the system, ΔE, is equal heat, q, in which part of the above diagram:

a. (a)
b. (b)
c. Both
d. Neither
e. None of the above

A

A

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2
Q

The name “Gibbs Free Energy” comes from the fact

a. It is a measure of the change in internal energy of a system
b. It is a measure of the disorder of a system
c. It is a measure of the spontaneousness of the system
d. It is a measure of the total energy available to do work
e. None of the above

A

D

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3
Q

Any property that does not depend on depend on the system’s history or future is called

a. Universal function
b. Adiabatic function
c. System function
d. State function
e. None of the above

A

D

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4
Q

The 1st Law Thermodynamics allows us to measure the total internal energy of a system by determining

a. its heat and work
b. its pressure-volume work
c. its enthalpy plus its pressure-volume work
d. the total internal energy of a system cannot be determined
e. None of the above

A

D

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5
Q

The SI unit of energy is called

a. volt
b. horsepower
c. calorie
d. joule
e. none of the above

A

D

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6
Q

The 2nd Law of Thermodynamics identifies specific properties that are necessary for a chemical reaction to occur spontaneously, they are:

a. Temperature, pressure, and volume
b. Temperature, enthalpy, pressure
c. Temperature, volume, enthalpy
d. Temperature, enthalpy, entropy
e. None of the above

A

D

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7
Q

The 2nd Law of Thermodynamics is based on what property?

a. enthalpy
b. temperature
c. entropy
d. pressure
e. none of the above

A

C

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8
Q

Conditions that ensure a chemical reaction is always spontaneous are:

a. Exothermic with increasing entropy
b. Endothermic with decreasing entropy
c. Endothermic with increasing entropy
d. Exothermic with decreasing entropy
e. None of the above

A

A

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9
Q

In the above illustration, the internal energy of the system depends on

a. The efficiency of the fan motor
b. which path is taken
c. How much heat is produced when the battery terminals are shorted out
d. Internal energy is completely independent of any path in the diagram
e. none of the above

A

D

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10
Q

The fact that it takes 4.184J of energy to raise 1g of water 1C is called

a. specific heat
b. specific energy
c. Molar heat of reaction
d. free energy
e. None of the above

A

A

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11
Q

To find the specific heat of something with a temperature change you use which equation?

A

q=msΔt

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12
Q

When calculating ΔS for the change in a reaction at equilibrium use which equation:

A

ΔG=ΔH-TΔS

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13
Q

When calculating the change in entropy that occurred during a chemical reaction use which equation?

A

ΔGt=ΔHt-TΔSt

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14
Q

ΔG means?

A

Free Energy

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15
Q

ΔH means?

A

enthalpy

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16
Q

ΔS means?

A

entropy

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17
Q

To calculate the equilibrium constant (k) for a reaction use which equation?

A

ΔG=-RTlnK

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18
Q

When finding the value of ΔHvap which equation do you use?

A

lnP2 -ΔHv 1 1
—–= ——— ( —– - —— )
P1 R T2 T1

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19
Q

To calculate ΔE use which equation?

A

ΔE=ΔH-ΔnRT

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20
Q

To find ΔH?

A

[ Product- Reactant]

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21
Q

to find Δn?

A

[ product-reactant]

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22
Q

To find the Activation energy use which equation?

A

lnk1 -Ea 1 1
—- = —— ( —– - —– )
k2 R T2 T2

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23
Q

First Order rate constant calculation is

A

e^-kt

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24
Q

Salts of weak acids effect the pH of the solution because

a. they do not effect the pH of the solution
b. once the sale ionizes, the cation acts as a weak acid by undergoing another reaction with water creating its conjugate base
c. acid salts actually raise the pH of a solution because they produce a stronger conjugate base
d. acid salts effect pH because a hydrogen ion is released when the salt ionizes
e. none of the above

A

C

25
Q

What value is most helpful when determining which buffer system to use at a given pH

a. concentration of weak acid/base
b. concentration of the salt of the weak acid/base
c. the ionization constant of the weak acid/base
d. capacity of the buffer system
e. none of the above

A

C

26
Q

Circle the stronger acid

a. H2S
b. H2Se
c. H2O
d. HBr
e. None because all bases

A

D

27
Q

The most basic pH on the pH scale is 14. Why?

a. it is the most concentrated a base can be and still be dissolved in water
b. it is based on the auto-ionization equilibrium constant for water
c. it is the pkw of water
d. all of the above
e. none of the above

A

D

28
Q

What is the conjugate acid of the reaction of CaO with H2O?

a. Ca+2
b. O-2
c. OH-
d. CaO does not react with water
e. none of the above

A

A

29
Q

Which has the weakest conjugate acid?

a. NH3
b. HCN
c. HOCl
d. NaOH
e. none have conjugate acids

A

D

30
Q

The fundamental chemical principle that explains why buffer systems work is

a. Mass action law
b. Bronsted-Lowry principle
c. Le Chateliers’ principle
d. Henry’s law
e. none of the above

A

C

31
Q

Substances that can be either actids or bases depending on the other substance present are called

a. semiprotic
b. amphoteric
c. ambiguous
d. a and b
e. none of the above

A

B

32
Q

Hydrogen peroxide, H2O2 is a weak acid with a ka=1.8 x 10^-12. What is the value of kb of it’s conjugate base?

a. 5.6x10^-3
b. 1.8 x 10^-12
c. 1.47 x 10^-11
d. 7.4 x 10^-5
e. none of the above

A

A

33
Q

If a 0.15M solution of lactic acid has a lactate ion, C3H5O2, concentration of 4.6x10^-3M. What is it’s percent ionization?

a. 1.3%
b. 3.1%
c. 5.16%
d. 2.0%
e. none of the above

A

B

34
Q

What is the conjugate acid of methylamine, CH3NH2?

a. CH3NH-
b. CH3NH3+
c. CH3NH2
d. CH3NH3Cl
e. none of the above

A

B

35
Q

Liquid chlorine bleach is really nothing more than a solution of sodium hypochlorite, NaOCl, in water. if the standard concentration of NaOCl in bleach is 0.67M, making the HOCl concentration in the solution, 4.7x10^-4M, what is the pH of the solution?

a. 7.0
b. 2.5
c. 3.3
d. 10.7
e. none of the above

A

D

36
Q

If the pOH of a solution is 13.6, calculate the pH of that solution

a. 4.0
b. 0.4
c. 7.0
d. 0.4056
e. none of the above

A

B

37
Q

Consider the reaction 2NO-N2O2, which of the following is not true?

a. Rate=kf[NO]^2
b. Rate=kr[N2O2]^
c. kf[NO}^2=kr[N2O2]
d. kf=kr
e. all of the above

A

D

38
Q

if a radioactive isotope had a half life of 225 years how long would it take for 1/8 of the isotope to remain?

a. 112.5 years
b. 225 years
c. 450 years
d. 900 years
e. none of the above

A

E

39
Q 
2N2O5--> 2N2O4+O2
from the above reaction find the rate of the formation of O2, when the rate of N2O5, decomposition is 0.020 moles/Ls. 
a. 0.005 moles/Ls 
b. 0.010 moles/Ls
c. 0.020 moles/Ls
d. 0.030 moles/Ls
e. none of the above
A

B

40
Q

the free-radical bromination of propane leads to tow products of very unequal abundances, 96% of product “a” and 4% of product “b”. Why is this?

a. the activation energy of product “a” is significantly lower than product “b”.
b. Product “a” has the more stable intermediary compound in the transition state
c. Product “a” has a much higher production rate than product “b”
d. All of the above
e. None of the above

A

D

41
Q

Which statement is false concerning the determination of the rate law expression?

a. it can be found from the molar coefficients in a balanced equation of the reaction
b. it can be found from the mechanism of the raction
c. it can be found from the rate determining step
d. the rate cannot be determined theoretically
e. none of the above

A

A

42
Q

A graphical representation of the rate law expression would be

a. a plot of concentration as a function of time
b. a plot of the natural log of the concentration as a function of time
c. a plot of concentration as a function of rate
d. a plot of the natural log of the rate constant as a function of the reciprocal of the temperature
e. none of the above

A

C

43
Q

A reaction with the following rate law expression would be a _____ order reaction. Rate=k[A]2[B]4[C]3

a. second
b. fourth
c. sixth
d. ninth
e. none of the above

A

D

44
Q

Anode does the

A

oxidizing

45
Q

Cathode does the

A

reduction

46
Q

Amps are in what units

A

sec

47
Q

What equation is used to find the overall cell potential

A

Ecell=EoCell-RT [k2]
—– ln ——
nF [k1]

48
Q

To calculate Standard free energy ΔG at equilibrium use which equation

A

ΔG=-nFEoCell

49
Q

When finding the equilibrium constant Kc what equation do you use

A

EoCell=RT
—– lnk
nF

50
Q

What part of a redox reaction occurs at the cathode?

a. oxidation
b. reduction
c. electrolysis
d. resistance
e. none of the above

A

B

51
Q

A galvanic cell will not function without a salt bridge, why?

a. it provides the solutions with a right pH
b. it conducts electricity
c. it neutralizes excess acid
d. it balances the ionic charge of the solutions
e. none of the above

A

d

52
Q

what is the coordination number of nickel in [Ni9en)2(NO2)2]-4

a. 2
b. 4
c. 6
d. 8
e. none of the above

A

C

53
Q

What is the net charge on a complex ion comprised of Fe(III) and 3 water and 3 ammonia ligands?

a. 1
b. 2
c. c
d. -1
e. -2

A

C

54
Q

Which is NOT a use of electrolytic cells

a. copper purification
b. chlorine gas production
c. aluminum production
d. production of electricity
e. they are all applications for electrolytic cells

A

D

55
Q

What are the units of ampres x volts x seconds?

a. coulombs
b. ohms
c. seconds
d. joules
e. none of the above

A

D

56
Q

What would be the reduction potential at a hydrogen electrode if the reduction of copper was chosen as the standard reference potential of 0.00 volts?

a. +0.34
b. -0.34
c. -0.25
d. +0.00
e. none of the above

A

B

57
Q

What is the coordination number of nickel in [Ni(C2O4)2(NO2)2]-4 ion

a. 2
b. 4
c. 6
d. 8
e. none of the above

A

C

58
Q

Two enantomers are ____ of each other

a. structure isomers
b. geometric isotopes
c. optical isomers
d. low spin complexes
e. none of the above

A

C

59
Q

The formula for a metal complex consisting of Cr+3, two NH3, and 4No2_ ligands is

A

[Cr(NO2)4(NH3)2]-1

Chemistry 2 Final (1 decks)

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