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Chem 1046 Final Exam > Chem 1046 Final Exam > Flashcards

Chem 1046 Final Exam Flashcards

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1
Q

What 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 reaction
c. it can be found from the rate determining step or elementary process
d. the rate cannot be determined theoretically
e. none of the above

A

a. It can be found from the molar coefficients in a balanced equation of the reaction.

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2
Q

Activation energy can be described as

a. the measure of energy released in an exothermic reaction
b. the amount of kinetic energy a population of molecules contain before a reaction will occur
c. the amount of kinetic energy a molecular reaction releases
d. the amount of energy a reaction produces
e. none of the above

A

b. the amount of kinetic energy a population of molecules contain before a reaction will occur

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3
Q

Raising the temperature of a reaction may make the reaction go faster, why?

a. by raising the temperature a larger population of molecules has sufficient kinetic energy to form the activated complex when they collide and hence, faster reaction.
b. by raising the temperature, the pressure increases creating more molecules and therefore, a faster reaction.
c. by raising the temperature the molecules become more likely to self-catalyze and internally speed up the reaction
d. raising the temperature effects equilibrium but not the reaction rate.
e. none of the above

A

a. by raising the temperature a larger population of molecules has sufficient kinetic energy to form the activated complex when they collide and hence, faster reaction.

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4
Q

One reason the rate of a reaction changes over the course of some reaction is because

a. the products interfere and tend to slow the reaction down
b. as the reactants are consumed, the population becomes smaller and less likely to collide
c. the rate of reaction is always constant
d. the molar proportions of the reactants change over the course of the reaction.
e. none of the above

A

b. as the reactants are consumed, the population becomes smaller and less likely to collide

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5
Q

Consider the reaction 2NO N2O2 at equilibrium. Which of the follow is not true?

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

A

d. kf=kr

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6
Q

You must consider a chemical reaction that yields a variety of products. Product A yields 20%, Product B yields 70% and C yields 10%. Which statement is false concerning product B?

a. it has the lowest activation energy
b. its transition state is more stable than products A or C.
c. it experiences the largest number of collisions of reactant molecules
d. it transition state goes to product more often
e. all of the above are true

A

c. it experiences the largest number of collisions of reactant molecules

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7
Q

Of the following statements, which is true regarding the following one step chemical reaction?
2HI -> H2 + I2
a. the rate of the H2 production cannot be determined relative to the rate of HI decay
b. this is a first order reaction
c. the rate of HI decay is twice the rate of production of I2
d. the rate law expression for this reaction is, Rate=k[HI]
e. none of the above is correct

A

c. the rate of HI decay is twice the rate of production of I2

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8
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

b. a plat of the natural log of the concentration as a function of time

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9
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. ninth

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10
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. 225 years
b. 450 years
c. 675 years
d. 900 years
e. none of the above

A

c. 675 years

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11
Q

In the above diagram, work is done by which system

a. (a)
b. (b)
c. both
d. neither
e. none of the above

A

(b)

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12
Q

Internal energy of the system, ΔE, is equal heat, q, in which part of the above diagram, a, b, or both?

a. (a)
b. (b)
c. both
d. neither
e. none of the above

A

a. (a)

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13
Q

Any property that does not 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. state function

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14
Q

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

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. the total internal energy of a system cannot be determined

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15
Q

The SI unit of energy is called ________

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

A

d. joule

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16
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 and pressure
c. temperature, volume, enthalpy
d. temperature, enthalpy, entropy
e. none of the above

A

d. temperature, enthalpy, entropy

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17
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. exothermic with increasing entropy

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18
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. all of the above

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19
Q

Which statement is false concerning the free-radical bromination of propane?

a. the rate can be determined from the rate-determining step
b. Br2 must be split into Br atoms for the reactions to produce product
c. the frequency factor demonstrates that the brominated central carbon product will have the greatest abundance
d. Bromination of the central carbon proceeds faster than bromination of the terminal carbons atoms in the propane molecule
e. none of the above

A

c. the frequency factor demonstrates that the brominated central carbon product will have the greatest abundance

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20
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. entropy

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21
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. it is a measure of the total energy available to do work

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22
Q

In the above diagram, 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. internal energy is completely independent of any path in the diagram

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23
Q

The fact that it takes 4.184 J 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. specific heat

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24
Q

Collision theory identifies which events must occur before a chemical reaction can take place?

a. molecules must collide with the right orientation and break apart
b. molecules must collide with enough energy and break apart
c. molecules must collide with the right orientation and sufficient kinetic energy
d. molecules must collide and form a stable complex, then another molecule breaks it apart
e. none of the above

A

c. molecules must collide with the right orientation and sufficient kinetic energy

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25
A light bulb is an example of an a. insulated system b. adiabatic system c. closed, insulated system d. closed, non-insulated system e. none of the above
d. closed non-insulated system
26
Which is the stronger acid? a. H2S b. H2Se c. H2O d. HBr e. none because these are all for bases
d. HBr
27
``` Name the Bronstad-Lowry base in the following reaction N2H4 + H2O ? a. H2O b. N2H4 c. N2H5 d. OH- ```
d. OH-
28
The fundamental chemical principle that explains why buffer systems work is a. mass action law b. bronsted-lowery principle c. Le Chateliers Principles d. Henry’s law e. none of the above
c. Le Chateliers Principles
29
Which acid has the weakest conjugate base? a. NH4+ b. HOCL c. HNO2 d. HBr e. CH3COOH
d. HBr
30
The bronstad-lowry definition of a base is a. any compound containing a hydroxide ion b. any compound that acts as a proton acceptor c. any compound that acts as a proton donator d. any compound that contains an ammonium ion e. none of the above
a. any compound containing a hydroxide ion
31
Which of the following compounds will have the highest molar solubility in pure water? a. AgI, ksp=8.51 X 10-17 b. PbSO4, ksp=1.82 x 10-8 c. FeS, ksp= 3.72 x 10-19 d. PbS, ksp= 9.04 x 10-29 e. MgCO3 ksp= 6.82 x 10-6
e. MgCO3 ksp= 6.82 x 10-6
32
Which is not a reason oxy-acids containing more oxygen atoms are stronger acids? a. the electronegativity of the central atom is always higher b. the high electronegativity of the oxygen atoms stabilizes the negative charge on the anion c. the oxygen atoms share the overall negative charge on the anion d. higher numbers of oxygen atoms mean each oxygen atom supports a lower fractional charge e. none of the above
a. the electronegativity of the central atom is always higher
33
Which of the following acids (listed with ka values) and their conjugate base would be best to form a buffer with a pH of 2.34? a. HCN ka=4.9 x 10-10 b. HC7H5O2 ka=6.5 x 10 -5 c. HF ka= 3.5 x 10-4 d. HClO ka= 2.9 x 10-8 e. HClO2 ka= 1.1 x 10-2
e. HClO2 ka= 1.1 x 10-2
34
Which of the following is not a reason that the highest pH on the pH scale is 14? a. the auto-ionization of water demonstrates the maximum OH- concentration is 10-14 b. the kw for the auto ionization of water is 10-14 c. on average 1 out of 10-14 water molecules dissociate d. the pH of an acid solution is less than 7 e. none of the above
d. the pH of an acid solution is less than 7
35
Which of the following will form an acidic solution in water? a. NaF b. LiI c. KNO3 d. NH4Cl e. none of the above will be acidic
d. NH4Cl
36
If the pKa of HCHO¬2 is 3.74 and the pH of an HCHO2/NaCHO2 solution is 3.1, which of the following is true? a. [HCHO2] [NaCHO2] d. [HCHO2] = [NaCHO2] e. it is not possible to make a buffer of this pH from HCHO2 and NaCHO2.
c. [HCHO2] > [NaCHO2]
37
Salts of weak acids effect the pH of the solution because a. they do not effect the pH of the solution b. once the salt ionizes, the cation acts as a weak acid by undergoing another reaction with water creating a conjugate base. c. acid salts actually raise the pH of the 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
c. acid salts actually raise the pH of the solution because they produce a stronger conjugate base
38
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
c. the ionization constant of the weak acid/base
39
What is the conjugate base of N2H4 when it reacts with an acid? a. N2H4+ b. N2H3- c. N2H5+ d. all the above e. none of the above
b. N2H3-
40
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
c. OH-
41
Which has the weakest conjugate acid a. NH3 b. HCN c. HOCl d. NaOH e. none have a conjugate acid
d. NaOH
42
Solid and liquid concentrations can be ignored in the mass action expression because a. they do not enter into the reaction at equilibrium b. they have an almost constant mole to volume relationship during reaction c. they actually must be included in the mass action expression d. they are NOT ignored in the mass action expression, but are incorporated into the equilibrium constant e. none of the above
d. they are NOT ignored in the mass action expression, but are incorporated into the equilibrium constant
43
Substances that can be either acids or bases depending on the other substance present are called ___________ a. semiprotic b. amphoeteric c. ambiguous d. A and B e. none of the above
b. amphoeteric
44
Hydrogen peroxide, H2O2, is a weak acid with a ka=1.8x10-12. what is the value of kb of its conjugate base? a. 5.6x10-3 b. 1.8x10-12 c. 1.47x10-11 d. 7.4x10-5 e. none of the above
a. 5.6x10-3
45
if an 0.15M solution of latic acid has a lacate ion, C3H5O2, concentration of 4.6x10-3M. what is its percent ionization a. 1.3 b. 3.1 c. 5.16 d. 2.0 e. none of the above
b. 3.1
46
Wht is the conjugate acid ofmethylamine, Ch3NH2 a. CH3NH- b. CH3NH3+ c. CH3NH2 d. CH3NH3Cl e. none of the above
b. CH3NH3+
47
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 NOCl 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
c. 3.3
48
At the temperature of the human body, 37C, the value of Kw is 2.4x10-14. what is the [H=] of water at that temperature? a. 1.6x10-7M b. 1.0x10-7M c. 4.0x10-8M d. cannot be calulated e. none of the above
a. 1.6x10-7M
49
If the pOH of a solution is 13.6m calculate the pH of that solution? a. 4.0 b. 0.4 c. 7.0 d. 0.4056 e. none
b. 0.4
50
What is the [H+] of a 0.03M solution of the strong acid HNO3? a. 13.6M b. 0.03 M c. 0.06M d. 0.60M e. none of the above
b. 0.03
51
``` What is the conjugate acid of the reaction Cao with H2o? a. Ca+2 b. O-2 c. OH- CaO does not react with water e. none of the above ```
a. Ca+2
52
what part of a redox reaction occurs at the cathode? a. oxidation b. reduction c. electrolysis d. resistance e. none
b. reduction
53
a galvanic cell will not function without a salt bridge, why? a. it provides the solutions with the 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
d. it balances the ionic charge of the solutions
54
what is the coordination number of nickel in [Ni(en)2(NO2)2]-4 a. 2 b. 4 c. 6 d. 8 e. none
c. 6
55
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. 3 d. -1 e. -2
c. 3
56
which is not a use of electrolytic cells a. cooper purification b. chlorine gas production c. aluminum production d. production of electricity e. they are all applications for electrolytic cells
d. production of electricity
57
what are the units of ampere x volts x seconds? a. coulombs b. ohms c. seconds d. joules e. none
d. joules
58
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
b. -0.34
59
what is the coordination number of nickel in [Ni(C2O4)2(NO2)2]-4 a. 2 b. 4 c. 6 d. 8
c. 6
60
two enantomers are _____ of each other a. structure isomers b. geometric isotopes c. optical isomers d. low spin complexes e. none o
c. optical isomers
61
the formula for a metal complex consisting of Cr+3, two NH3 and 4 NO2- ligands is a. [CrNH3NO2]+3 b. [(NH3)3(NO)4Cr]-1 c. [Cr(NH3)2(NO2)4]-1 d. [Cr(NO2)4(NH3)2]-1 e. none
d. [Cr(NO2)4(NH3)2]-1
62
Iron rusts because a galvanic cell between iron metal and the dissolved oxygen in the water to which the iron is exposed is established. What is produced at the anode? a. O2 b. Fe(s) c. Fe+2 d. OH- e. none
c. fe+2
63
From the reduction potential table, what is the substance most likely to be formed at the cathode of an electrolytic cell consisting of two inert platinum electrodes dipped into a solution of K2SO4? a. K(s) b. H2SO3 c. O2 d. H2 e. none
d. H2
64
In the following galvanci cell, Fe(s)|Fe+3||Ag+|Ag(s) which is the anode? a. Fe(s) b. Fe+3 c. Ag+ d. Ag(s) e. none
a. Fe(s)
65
``` Reduction potentials are determined in galvanic cells using an a reference cathode b. hydrogen electrode c. metal electrode d. cathodic electrode e. none ```
b. hydrogen
66
the flow of ions through the wires connecting the cells of a galvanic cell is called a. galvanic conduction b. metallic conduction c. electrolytic conduction d. electrical conduction e. none
b. metallic conduction
67
the battery in your car becomes a ____ when the engine is running a. galvanic cell b. electric cell c. battery d. electrolytic cell e. none
d. electrolytic cell
68
will reaction occur spontaneously if silver metal is dipped into HI solution? a. yes b. no c. only if the HI is in low enough concentrations d. depends on the voltage e. none
b. no
69
if the molar solubility of a salt exceeds the solubility product of that salt ______ a. the salt will precipitate b. the salt will not precipitate c. molar solubility and solubility product are not related d. the solution will be saturated with respect to the salt e. none
a. the sale will precipitate
70
the molar solubility of salt it a. the concentration of the salt in solution b. the total mass of the salt added to solution c. the saturated concentration of salt in solution d. all e. none
c. the saturated concentration of salt in solution
71
if salt is added to a solution containing an ion in common with the salt being added, the solubility of the salt will a. increase b. decrease c. not change d. all b. none
b. decrease
72
Metal hydroxide salts become more soluble as the pH of the solution is lowered, why? a. the more acidic solution strips electrons from the metal creating higher charged metal cations which are more soluble b. lowering the pH actually removes product, thus shifting the reaction equilibrium to the right or productions c. acids corrodes metal d. metal hydroxides are not more soluble in acid solution e. none
b. lowering the pH actually removes product, thus shifting the reaction equilibrium to the right or productions
73
The solubility of metal sulfides and metal carbonates is said to represent simultaneous equilbria. why? metal sulfides and metal carbonates react with each other simultaneously b. metal sulfides and metal carbonates always come to equilibrium in the amount of time c. metal sulfides and metal carbonates do no represent simultaneous equilibria d. metal sulfides and metal carbonates contain anions that react with water thus creating several simultaneous controlling reactions e. none of the above
d. metal sulfides and metal carbonates contain anions that react with water thus creating several simultaneous controlling reactions
74
The solubility of metal sulfides is dependent on pH as well as salt concentration. Why? a. sulfide anions react with metal ions to produce hydrogen ions b. sulfide anions react with water c. sulfide anions react with hydrogen d. metal sulfide solubility does not depend on pH e. none
b. sulfide anions react with water
75
CaO lime, is used in agriculture to raise pH of soil. how does this happen? a. CaO forms CaCO3 in the soil b. CaO forms Ca(NO3)2 in the soil thus providing nitrogen to plants c. CaO does nothing to pH d. CaO reacts with water within soil releasing OH- ions which effectively raise soil pH e. none
d. CaO reacts with water within soil releasing OH- ions which effectively raise soil pH
76
The kspa for metal sulfide salts differs by a constant number from the ksp of the same sulfide salts. why? a. the sulfide ion from metal sulfides reacts with water the same way regardless of the metal ion b. the kspa is actually the ksp of the metal sulfide divided by the ka1 and ka2 of the weak acid H2S c. metal sulfides equilibrate with metal ions and the reaction of sulfide ions with water d. all e. none
b. the kspa is actually the ksp of the metal sulfide divided by the ka1 and ka2 of the weak acid H2S
77
If the pH of a solution consisting of 0.10M of NiS is reduced sufficiently, will all the NiS precipitate a. yes b. no c. only if you lower the concentration of NiS d. only if it's heated e. none
b. no
78
the free energy of a galvanic cell is _____ a. positive b. negative c. depends on farradays constant d. all e. none
b. negative
79
What is the first order rate equation?
[NO3]=e^-kt[NO3}o
80
What is the second order rate equation?
1/[B] - 1/[B]o = kt
81
What is the zero order rate equation?
[A]= -kt + [A]o
82
What is the two point solution to the Clausius Clapyron Equation?
lnp2/p1= -ΔHvap-/R (1/t2-1/t1)
83
What is the first law of thermodynamics?
ΔE=q+w
84
What is enthalpy?
ΔH, heat , kj/mole
85
What equation is used when finding ΔE for gases?
ΔE=ΔH-Δnrt
86
What is entropy?
Δs, measure of disorder
87
What is free energy?
ΔG
88
What is the second law of thermodynamics?
ΔG=ΔH-TΔS
89
To find the equilibrium constant use what equation?
ΔG= ΔGo-rtlnk or k=-e^ΔG/rt
90
What is the Arrhenius Equation?
K=Ae^-E/rt
91
What is the two point solution for the arrehenius equation?
lnk2/k2=-E/R(1/t2-1/t1)

Chem 1046 Final Exam (1 decks)

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