WorksheetsQuiz 2
Total questions: 123
Worksheet time: 2hrs 50mins
Name
Class
Date
1.
permanganate
a)
MnO41-
b)
MnO32-
c)
MnO21-
d)
MnO1-
2.
carbonate
a)
CO32-
b)
CO22-
c)
CO3
d)
CO2
3.
CN1-
a)
cyanide
b)
cyanate
c)
carbon nitride
d)
cyanite
4.
perchlorate
a)
ClO41-
b)
ClO31-
c)
ClO21-
d)
ClO1-
5.
ClO21-
a)
chlorite
b)
chlorate
c)
hypochlorite
d)
hypochlorate
6.
ClO1-
a)
hypochlorite
b)
chlorate
c)
chlorite
d)
perchlorate
7.
hydrogen phosphate
a)
HPO42-
b)
H2PO42-
c)
HPO32-
d)
H2PO41-
8.
hydroxide
a)
HO-1
b)
OH-1
c)
HO
d)
OH
9.
acetate
a)
C2H3O2-1
b)
Ac-1
c)
CH2COO-1
d)
C4H4O62-
10.
peroxide
a)
O22-
b)
O2-
c)
O21-
d)
O1-
11.
nitrite
a)
NO21-
b)
NO31-
c)
NO3
d)
NO2
12.
nitrate
a)
NO3-1
b)
NO2-1
c)
NO3
d)
NO2
13.
sulfite
a)
SO32-
b)
SO42-
c)
SO3
d)
SO4
14.
Sulfate
a)
SO42-
b)
SO32-
c)
SO4
d)
SO3
15.
chromate
a)
CrO42-
b)
Cr2O72-
c)
CrO41-
d)
Cr2O71-
16.
ammonium
a)
NH4+
b)
NH4
c)
NH3
d)
NH3-
17.
What atom matches this electron configuration?
1s22s22p63s2
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
18.
1. What is the shape of an s orbital?
a)
sphere
b)
dumbbell
c)
double dumbbell
d)
TOO COMPLEX TO KNOW IT.
19.
Which is associated with more energy?
a)
2p
b)
2s
c)
3p
d)
1s
20.
Electrons occupy orbitals of lowest energy first is part of what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
21.
Which is a correct orbital box diagram?
a)
a
b)
b
c)
d
d)
e
22.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
23.
If a balloon is cooled what will happen to the volume?
a)
Volume will increase
b)
Volume will decrease
c)
Volume will not change
24.
The greater the speed of gas particles in a container, the:
a)
greater the pressure
b)
fewer collisions there will be
c)
lower the temperature
d)
lower the pressure
25.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
26.
How many electrons should Chlorine have around its Lewis dot model?
a)
5
b)
6
c)
7
d)
8
27.
Which of the following is an ionic bond?
a)
H3N
b)
CaCl2
c)
NO2
d)
SCl
28.
Draw the Lewis structure for OF2 and determine the number of lone pairs on the central atom.
a)
none
b)
1
c)
2
d)
it's ionic
29.
What is the electron configuration of Ag?
a)
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1 4d10
b)
[Kr] 5s2 4d9
c)
1s2 2s2 2p6 3s2 3p6 4s2 4p6 5s2 4d9
d)
1s2 2s2 2p6 3s2 3p6 3d10 4s2 4d10 4p6 5d10 5s2 4d9
30.
A diatomic element with a high ionization energy would most likely be a
a)
nonmetal with high electronegativity
b)
metal with high electronegativity
c)
nonmetal with low electronegativity
d)
metal with low electronegativity
31.
As we move down Group 1 elements of the Periodic Table, the first ionization energy of each element decreases. One reason for this is that
a)
the nuclear charge is decreasing
b)
the number of energy levels is decreasing
c)
distance between valence electrons and the nucleus increases
d)
the number of neutrons is increasing
32.
What is the molarity of a solution made from 325.4g of AlCl3 with enough water to make 500.0 mL?
a)
4.88 M
b)
4.880 M
c)
2.440 M
d)
2.44 M
33.
You have 286.7g of PbO. For lab, you need 2.50M PbO. How much PbO can you make?
a)
0.5140mL
b)
554 mL
c)
514 mL
d)
0.554 L
34.
**Write down the equation and numbers! Write and balance the equation for a reaction between potassium bromide and calcium.
a)
2KBr + Ca --> CaBr2 + 2K
b)
KBr + Ca --> CaBr + K
c)
2KBr + Ca --> CaBr2 + K2
d)
3KBr + Ca --> CaBr3 + 3K
35.
Sodium nitrate
a)
soluble
b)
insoluble
36.
Cr3(PO4)2
a)
soluble
b)
insoluble
37.
ammonium hydroxide
a)
soluble
b)
insoluble
38.
copper (II) chloride
a)
soluble
b)
insoluble
39.
What are the spectator ions in the reaction of sodium chloride with silver nitrate?
a)
silver and nitrate
b)
sodium and chlorine
c)
sodium and nitrate
d)
silver and chlorine
40.
What is Solubility?
a)
What is dissolved
b)
What does the dissolving
c)
A measure of how much solute can dissolve in solvent
d)
a charged ion
41.
What is the precipitate formed when you mix silver nitrate with copper chloride?
a)
copper nitrate
b)
copper chloride
c)
silver chloride
d)
silver nitrate
42.
Which list contains only precipitates?
a)
copper hydroxide, lead iodide, calcium carbonate
b)
calcium nitrate, lead sulfate, barium phosphate
c)
sodium nitrate, calcium hydroxide, iron (III) hydroxide
43.
This electrode in a voltaic cell gains mass
a)
anode
b)
cathode
44.
Reactions in voltaic cells are
a)
spontaneous, redox reactions
b)
non-spontaneous, redox reactions
c)
spontaneous, non-redox reactions
d)
non-spontaneous, non-redox reactions
45.
In a voltaic cell, the half cell that receives anions from the salt bridge is
a)
cathode
b)
anode
46.
Which energy conversion shown below takes place in a galvanic cell?
a)
electrical to chemical
b)
mechanical to chemical
c)
mechanical to electrical
d)
chemical to electrical
47.
Consider the following numbered processes:
1. A -> 2B
2. B -> C + D
3. E -> 2D
ΔH for the process A -> 2C + E is
1. A -> 2B
2. B -> C + D
3. E -> 2D
ΔH for the process A -> 2C + E is
a)
ΔH1 + ΔH2 + ΔH3
b)
ΔH1 + ΔH2
c)
ΔH1 + ΔH2 - ΔH3
d)
ΔH1 + 2ΔH2 - ΔH3
48.
How many valence electrons in this structure?
a)
6
b)
5
c)
4
d)
7
49.
Which one of the following is a first order, overall reaction
a)
k1= 1.000 M s-1
b)
k1= 5403.2 M½ s½
c)
k1= 1.23 x 10-6 M-1 s-1
d)
k1= 10.7 s-1
50.
a)
A. is most exothermic
b)
B. is most exothermic
c)
C. is most exothermic
d)
D. is most exothermic
51.
Consider the following rate law: Rate = k[A]n[B]m
How are the exponents n and m determined?
How are the exponents n and m determined?
a)
by using balanced chemical equation
b)
By using the subscripts for the formulas
c)
By educated guess
d)
By experiment
52.
a)
A. has largest Ea
b)
B. has largest Ea
c)
C. has largest Ea
d)
E. has largest Ea
53.
What would be my the overall order of this rate law?
Rate=[A]2[B]1
Rate=[A]2[B]1
a)
0 Order
b)
1st Order
c)
2nd Order
d)
3rd Order
54.
a)
A. is the slowest reaction
b)
B. is the slowest reaction
c)
C. is the slowest reaction
d)
E. is the slowest reaction
55.
a)
A. is the fastest reaction
b)
B. is the fastest reaction
c)
C. is the fastest reaction
d)
E. is the fastest reaction
56.
The reaction of (CH3)3CBr with hydroxide ion proceeds:
(CH3)3CBr(aq) + OH-(aq) → (CH3)3COH(aq) + Br-(aq)
What will the initial rate (in mol/L*s) be in Experiment 4?
(CH3)3CBr(aq) + OH-(aq) → (CH3)3COH(aq) + Br-(aq)
What will the initial rate (in mol/L*s) be in Experiment 4?
a)
0.003
b)
0.006
c)
0.009
d)
0.018
57.
In any first order reaction, as the reaction proceeds at constant temperature, which describes the corresponding effects on k (the rate constant) and rate?
a)
k remains the same; rate decreases
b)
k and rate both remain the same
c)
k remains the same; rate increases
d)
k decreases; rate remains the same
58.
A compound has a half-life of 14 min. How much time will it take a 12 mol sample to decay to 1.5 mol?
a)
14 min
b)
28 min
c)
42 min
d)
56 min
59.
Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from 6 moles H2?
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from 6 moles H2?
a)
4 moles Fe
b)
6 moles Fe
c)
9 moles Fe
d)
2 moles Fe
60.
2 NaClO3 (s) --> 2NaCl (s) +3 O2 (g)
12.00 moles of NaClO3 will produce how many grams of O2?
12.00 moles of NaClO3 will produce how many grams of O2?
a)
256 g of O2
b)
576 g of O2
c)
288 g O2
61.
What is the limiting reactant if 10 moles of NH3 react with 30.0 moles of NO?
4NH3+6NO --> 5N2 + 6H2O
4NH3+6NO --> 5N2 + 6H2O
a)
NH3
b)
NO
c)
N2
d)
water
62.
What is the strongest type of intermolecular force present in HF?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
63.
H2S has what kind of intermolecular force?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
64.
Intermolecular forces are the forces
a)
within molecules
b)
between molecules
65.
Which of the following has the lowest boiling point?
a)
CaCl2
b)
PH3
c)
Cl2
d)
N2
66.
Which of the following will take the longest to evaporate?
a)
CH3CH2OH
b)
CH3OH
c)
CH3CH3
67.
Rank these in order of strength:
covalent bond
London forces
hydrogen bond
dipole-dipole attraction
covalent bond
London forces
hydrogen bond
dipole-dipole attraction
a)
dipole-dipole>covalent bond>hydrogen bond>London
b)
London>dipole-diple>hydrogen bond>covalent bond
c)
covalent bond>hydrogen bond>dipole-dipole>London
d)
hydrogen bond>dipole-dipole>London>covalent bond
68.
All molecules have London forces between them, but dipole-dipole and hydrogen bonding are so much stronger that when they are present we can ignore London forces. Which of these has ONLY London forces?
a)
I2
b)
NH3
c)
OCl2
d)
SH2
69.
Which of the following elements is not present in a hydrogen bond?
a)
F
b)
N
c)
O
d)
C
70.
Which of these causes the U-shaped meniscus when water is placed in a glass graduated cylinder?
a)
surface tension of water
b)
adhesive properties of water
c)
cohesive properties of water
d)
the high viscosity of glass
71.
What is surface tension?
a)
a measure of the energy required to increase the surface area of a liquid
b)
a measure of the ability of a liquid to form a meniscus
c)
a measure of the adhesive properties of a liquid
d)
resistance to flow of a liquid
72.
Which of these is a result of capillary action?
a)
water "beads up" on a waxed car
b)
cotton wicks away moisture from the body
c)
certain insects "float" on water
d)
mercury's meniscus is an inverted U
73.
What is viscosity?
a)
a measure of inward forces at the surface of a liquid
b)
a measure of the cohesive properties of a liquid
c)
a measure of the adhesive properties of a liquid
d)
resistance of a liquid to flow
74.
When molar masses and polarities are similar, _____________ molecules tend to have higher IMF's.
a)
long, chain-like
b)
compact, spherical
c)
hydrocarbon
d)
hydrogen-containing
75.
Which of these typically increases when IMF's increase?
a)
boiling point
b)
melting point
c)
viscosity
d)
all of these
76.
Which type of solid is hard, brittle, and nonconducting unless dissolved in H2O?
a)
Ionic Crystal
b)
Covalent Molecular Crystal
c)
Metallic Crystal
d)
Covalent Network Crystal
77.
Which is less compressible?
a)
Amorphous Solid
b)
Crystalline Solid
78.
What property gives metallic solids the ability to conduct electricity well, but not covalent network solids?
a)
Electrons in metallic solids are strongly bound in place
b)
Electrons in covalent network solids are freely moving around
c)
Covalent network solids are not bound to other atoms
d)
Metallic solids have many electrons that are not bound and can move about the solid
79.
During a phase change what happens to temperature?
a)
it increases
b)
it decreases
c)
depends; if being heated it increases, if being cooled it decreases
d)
stays constant
80.
All changes in the state of matter of a substance requires a change in
a)
mass
b)
temperature
c)
intermolecular forces
d)
energy
81.
When the temperature of matter increases the particles...
a)
speed up and move closer
b)
speed up and move farther apart
c)
slow down and move closer together
d)
slow down and move farther apart
82.
Which segment represents the heat of fusion?
a)
A-B
b)
B-C
c)
C-D
d)
D-E
83.
Which of the following is exothermic?
a)
melting
b)
freezing
c)
boiling
84.
Many kinetics equations fit a slope intercept form. The Arrhenius equation is k = A e−(Ea/RT). The slope of a plot of ln k vs. 1/T is equal to:
a)
-k
b)
k
c)
activation energy
d)
-Ea/ R
85.
A chemical reaction can occur:
a)
if the particles collide with enough energy
b)
if the particles collide with sufficient activation energy
c)
if the particles collide with correct orientation
d)
all of the above
86.
In a chemical reaction which goes forward:
a)
typically all reactants go forward toward the products
b)
typically some of the reactants go forward toward the products
c)
typically all reactants have just the right amount of activation energy to go forward toward the products
d)
typically all reactants have just the right orientation to go forward toward the products
87.
The mechanism of a chemical reaction is the sequence of actual events that take place as reactant molecules are converted into products.
Which of the following is true?
Which of the following is true?
a)
Each of these events constitutes an elementary step that can be represented as a coming-together of discrete particles ("collision").
b)
Each of these events constitutes an elementary step that can be represented as the breaking-up of a molecule ("dissociation") into simpler units.
c)
The molecular entity that emerges from each step may be a final product of the reaction, or it might be an intermediate.
d)
all of the above are true
88.
Consider the decomposition of nitrogen dioxide into nitric oxide and oxygen. The net balanced equation is: 2NO2(g)→2NO(g)+O2(g)
The mechanism of this reaction is believed to involve the following two elementary steps:
1st: 2NO2→NO3+NO
2nd: NO3→NO+O2
The mechanism of this reaction is believed to involve the following two elementary steps:
1st: 2NO2→NO3+NO
2nd: NO3→NO+O2
a)
NO3 has only a transient existence and does not appear in the net equation. It is an intermediate.
b)
NO3 has a permanent existence and does appear in the overall net equation.
c)
NO3 would appear at the highest point of an Time Vs. Energy Curve when graphed.
d)
NO3 is known as an activated complex or transition state.
89.
A useful reaction mechanism consists of a series of elementary steps (defined below) that:
a)
can be written as chemical equations, and whose sum gives the net balanced reaction equation.
b)
must agree with the experimental rate law.
c)
may be different under different conditions.
d)
all of the above
90.
Elementary reactions differ from ordinary net chemical reactions. Which of the following statements is false?
a)
A bimolecular process always follows the second-order rate law.
b)
Elementary steps often involve unstable or reactive species that do not appear in the net reaction equation.
c)
Net reactions may have different proposed elementary steps, and all are viable if they solve simultaneously to the overall net reaction, unless proved experimentally false.
d)
Some net reactions do proceed in a single elementary step, at least under certain conditions. The presence of a catalyst however cannot enable an alternative mechanism that greatly speeds up the rate of a reaction.
91.
Which type of elementary reaction is most common?
a)
unimolecular
b)
bimolecular
c)
termolecular
d)
none of the above, they are all equally common
92.
Multi-step (Consecutive) Reactions:
Mechanisms in which one elementary step is followed by another are very common.
step 1: A + B → Q
step 2: B + Q → C
net reaction: A + 2B → C
Which of the following is false?
Mechanisms in which one elementary step is followed by another are very common.
step 1: A + B → Q
step 2: B + Q → C
net reaction: A + 2B → C
Which of the following is false?
a)
The net reaction is just the sum of its elementary steps.
b)
The species Q is an intermediate, usually an unstable or highly reactive species.
c)
Intermediates such as Q can appear in the rate law of a net reaction.
d)
If both steps proceed at similar rates, rate law experiments on the net reaction would not reveal that two separate steps are involved here.The rate law for the reaction would berate=k[A][B]2
93.
The rate-determining step is also known as the rate-limiting step. Consider a 3 elementary step proposed mechanism.
1st step: fast
2nd step: slow
3rd step: fast
Which of the following is false?
1st step: fast
2nd step: slow
3rd step: fast
Which of the following is false?
a)
The rate law for the overall net reaction must simply include concentration(s), reaction orders, and a rate constant for that rate-determining step.
b)
We can generally expect that one of the elementary reactions in a sequence of consecutive steps will have a rate constant that is smaller than the others.
c)
The effect is to slow the rates of all the reactions.
d)
The overall rate law must include information from both the slow step and any step(s) before it.
94.
A "zeroth" order reaction for A-->B, will show:
a)
a straight line for a graph: time vs. ln [A]
b)
a straight line for a graph: time vs. [A].
c)
a straight line for a graph: time vs. 1/[A]
d)
none of the above
95.
A first order rate law for reaction A--> B will match a graph:
a)
which looks linear and positive in slope for time vs. ln [A].
b)
which looks non-linear and positive in slope for time vs. ln [A].
c)
which looks non-linear and negative in slope for time vs. ln [A].
d)
which looks linear and negative in slope for time vs. ln [A].
96.
A 2nd order rate law for reaction A--> B will match a graph:
a)
which looks linear and positive in slope for time vs. 1/ [A].
b)
which looks linear and negative in slope for time vs. 1/ [A].
c)
which looks non-linear and positive in slope for time vs. 1/ [A].
d)
which looks non-linear and negative in slope for time vs. 1/[A].
97.
For a 1st order reaction, the half-life ("t1/2") is equal to:
a)
t1/2 = 0.693/k
b)
t1/2 = k/0.693
c)
t1/2 = 1/k[A]o
d)
t1/2 = k
98.
What is true of the half-life of a chemical reaction?
a)
For a 1st order reaction, the half-life ("t1/2") is not dependent upon initial concentration.
b)
Half-life is a good estimate of reaction rate.
c)
Half-life helps us determine how long it takes for half of the starting concentration to change into product.
d)
All of the above are true
99.
Rate constants are:
a)
part of rate laws
b)
temperature dependent
c)
usually part of the slope in the slope-intercept equation form of a line
d)
all of the above
100.
For an overall reaction order of 1, what will rate constant "k" have for its units?
a)
1/s or s -1
b)
M/s or M x s-1
c)
1/Mxs or M-1 x s-1
d)
1/M2 x s or M-2 x s-1
101.
If temperature in increased,
a)
k is higher
b)
activation energy is lowered
c)
the speed of reaction goes up
d)
all of the above
102.
If we have two gases combining in a reaction to give a new product C: A + B --> C, how can we speed up the reaction?
a)
increase pressure of A
b)
decrease pressure of A
c)
cool A until it is a liquid
d)
none of the above
103.
How do you calculate the overall reaction order of a chemical reaction?
a)
add up the coefficients of the slow step of a reaction mechanism
b)
take the largest concentration reactant's coefficient
c)
add up all coefficients of all slow and fast steps in a proposed reaction mechanism
d)
add up the reaction orders of all elementary steps including only the slow step and any earlier steps
104.
Which one of the following changes would alter the rate constant (k) for a chemical reaction?
a)
A. increasing the concentration of A
b)
B. increasing the concentration of B
c)
C. increasing the temperature
d)
D. measuring k again after the reaction has run for a while
105.
Consider the reaction: P4 + 6 H2 → 4 PH3. A rate study of this reaction was conducted at 298 K. The data that were obtained are shown in the table on your paper. What is the reaction order with for P4?
a)
zero
b)
1st
c)
2nd
d)
none of the above
106.
Consider the reaction: P4 + 6 H2 → 4 PH3. A rate study of this reaction was conducted at 298 K. The data that were obtained are shown in the table on your paper. What is the reaction order with for H2?
a)
0
b)
1st
c)
2nd
d)
none of the above
107.
The rate law for a reaction is rate = k [A][B]2 Which one of the following statements is false?
a)
A) If [B] is doubled, the reaction rate will increase by a factor of 4.
b)
B) The reaction is second order in B.
c)
C) The reaction is first order in A.
d)
D) The reaction is second order overall.
108.
If the concentration of a reactant has zeroth order, it means:
a)
the multiple of the concentration change affects the reaction rate by the same multiple
b)
the multiple of the concentration change affects the reaction rate by a multiple of 2
c)
the multiple of the concentration change affects the reaction rate by a multiple of 4
d)
there is no effect of the concentration change on the reaction rate
109.
The rate of a reaction depends on __________.
a)
A) collision frequency
b)
B) collision orientation
c)
C) collision energy
d)
D) all of the above
110.
Activation energy when graphed can be calculated by:
a)
finding the difference in energy between the reactants and the transition state
b)
finding the energy between the transition state and the products
c)
finding the difference in energy between the reactants and products
d)
none of the above
111.
In an energy profile of: Time Vs. Energy, where are the intermediates found?
a)
at the far left start of the curve
b)
at the top of the hill of the curve(s)
c)
at the bottom of the valleys of the curve(s)
d)
none of the above
112.
The mechanism for formation of the product X is:
A + B -> C + D (slow)
B + D -> X (fast)
The intermediate reactant in the reaction is ___.
A + B -> C + D (slow)
B + D -> X (fast)
The intermediate reactant in the reaction is ___.
a)
A
b)
B
c)
C
d)
D
113.
Consider the following mechanism.
Step 1: O3 → O2 + O (fast)
Step 2: O3 + O → 2 O2 (slow)
What is the overall balanced equation?
Step 1: O3 → O2 + O (fast)
Step 2: O3 + O → 2 O2 (slow)
What is the overall balanced equation?
a)
4 O3 → 3 O2
b)
O3 → 3 O2
c)
3 O3 → 2 O2
d)
2 O3 → 3 O2
114.
Consider the following mechanism.
Step 1: O3 → O2 + O (fast)
Step 2: O3 + O → 2 O2 (slow)
What is the order with respect to each reactant?
Step 1: O3 → O2 + O (fast)
Step 2: O3 + O → 2 O2 (slow)
What is the order with respect to each reactant?
a)
1st
b)
2nd
c)
3rd
d)
0
115.
If the reaction: 2HI-->2H2 + I2 HI is first order, which of the following will yield a linear plot?
a)
a. log [HI] vs time
b)
b. 1/[HI] vs time
c)
c. [HI] vs time
d)
d. ln [HI] vs time
116.
Intermolecular forces can interfere with the speed of a reaction.
a)
true
b)
false
117.
Factors affecting speed of reaction include:
a)
a. boiling point
b)
b. change is mass
c)
c. pressure
118.
Most reactions are more rapid at high temperatures than at low temperatures. This is consistent with:
(I) an increase in the activation energy with increasing temperature.
(II) an increase in the rate constant with increasing temperatures.
(III) an increase in the percent of "high energy" collisions with increasing temperature.
(I) an increase in the activation energy with increasing temperature.
(II) an increase in the rate constant with increasing temperatures.
(III) an increase in the percent of "high energy" collisions with increasing temperature.
a)
only I
b)
only II
c)
only I and II
d)
only II and III
119.
Rate of reaction can be calculated by dividing molarity or pressure by:
a)
mass
b)
volume
c)
temperature
d)
time
120.
Kinetics studies:
a)
the disappearance of reactants
b)
the appearance of products
c)
both of the other answers
121.
Which statement is false?
a)
(a) If a reaction is thermodynamically spontaneous, it must have a low activation energy
b)
(b) If a reaction is thermodynamically spontaneous it may occur slowly.
c)
(c) Activation energy can be overcome by increasing the frequency of reactant collision with the presence of a catalyst.
d)
(d) If a reaction is thermodynamically non-spontaneous, it will not occur spontaneously.
122.
The half-life for a first-order reaction is 32 s. What was the original concentration if, after 2.0 minutes, the reactant concentration is 0.062 M?
a)
a. .84 M
b)
b. .069 M
c)
c. .091 M
d)
d. .075 M
123.
If I wanted steel wool to oxidize or "burn" quicker, I could:
a)
increase the amount of oxygen
b)
limit the amount of interacting or colliding particle collision
c)
ball up the steel wool more
d)
limit the number of places I light steel wool and add activation energy
100 %
