PiQ Exam 2
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Review Test Submission: Additional Practice Exam 2 with feedback ( A Remix)
2021SP-22142-CHEM1332-Fundamentals of Chemistry 2
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2021SP-22142-CHEM1332-Fundamentals of Chemistry 2
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Additional Practice Exam 2 with feedback ( A Remix)
Started
4/2/21 5:36 PM
Submitted
4/2/21 6:40 PM
Status
Completed
Attempt
Score
21 out of 22 points Time
Elapsed
1 hour, 3 minutes out of 1 hour and 23 minutes
Instructions
For multiple choice questions, select the best answer from those provided.
For Ñll-in the blank questions, spelling counts, and atomic symbols must start with capital
letters.
For numerical entry problems:
The default scoring method checks that your input value
agrees within plus or minus 2% of the expected value. Therefore unless otherwise
speciÑed, you should report at least three signiÑcant Ñgures and enter your value with no
units.
Some questions may ask you to enter your answer in scientiÑc notation.
This must be
done as exponential notation, using
a capital "E"
.
For example, 1921 would be entered
as 1.921
E
3; 0.00789 would be 7.89
E
-3.
Some questions may specify the number of decimal places to be used for an answer.
For
example, the value 6789.123 has three decimal places.
Some questions may specify that the log-base 10 of the calculated values should be
entered as the answer with at least two decimal places.
For example, a calculated value
of
0.00789 would be entered as
log(0.00789) = -2.103.
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Please read and answer each question carefully following any formatting instructions
given:
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Displayed
Submitted Answers, Correct Answers, Feedback
Question 1
Selected Answer:
Correct Answer:
Response
Feedback:
The molecular geometry of the XeF
4
molecule is ________, and this molecule is ________. square planar, nonpolar
square planar, nonpolar
(Hint: start by drawing the Lewis dot structure, use the electronegativity
difference to determine the bond polarity, and finally consider how the dipoles
(vectors) combine to determine the overall molecular polarity.)
Question 2
Selected Answer:
Correct Answer:
Response Feedback:
Consider the following reaction and its equilibrium constant: 4 CuO(s) + CH
4
(g) CO
2
(g) + 4 Cu(s) + 2 H
2
O(g) K
c
= 1.10 A reaction mixture contains 0.22 M CH
4
, 0.67 M CO
2
and 1.3 M H
2
O. Which of the following
statements is TRUE concerning this system?
The reaction will shift in the direction of reactants.
The reaction will shift in the direction of reactants.
IF
Q
> K
reverse direction
1 out of 1 points
1 out of 1 points
Q
= K
at equilibrium
Q
< K
forward direction
Question 3
Selected Answer:
2.51E0
Correct Answer:
2.51E0 ± 2%
Response
Feedback:
At a given temperature, the K
eq
for the equilibrium below is 0.399. SO
2
(g) + O
2
(g) SO
3
(g) What is the value of K
eq
at this temperature for the following reaction? SO
3
(g) SO
2
(g) + O
2
(g) If you multiply an equation by a number, you raise the equilibrium
constant to that power.
If you reverse a reaction, you take the reciprocal of the equilibrium
constant.
If you add two equations, you multiply their equilibrium constants.
Question 4
Selected Answer:
6.18E-2
Correct Answer:
6.18E-2 ± 2%
Response Feedback:
Given the following reaction at equilibrium, if K
p
= 2.45 at 210 °C, K
c
= ________. PCl
5
(g) PCl
3
(g) + Cl
2
(g)
, with R = 0.0821 atm L / (mol K) and T in K.
Question 5
Selected Answer:
3.73E-5
At a given temperature, the reaction,
H
2
(g) + I
2
(g)
2HI (g), has a value of K
eq
= 771.
If the hydrogen concentration is 0.00541 M
and the hydrogen iodide concentration is 0.01248
M, what is the molar concentration of the iodine at equilibrium? 1 out of 1 points
1 out of 1 points
1 out of 1 points
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Correct Answer:
3.73E-5 ± 2%
Response
Feedback:
The equilibrium constant is equal to the products over the reactants raised to
the stoichiometric ccoeÔcients (leaving out pure liquids and solid). Once your
write the equilibrium equation, you then substitute in the given values and
solved for the unknown concentration.
Question 6
Selected Answer:
9.352E1
Correct Answer:
9.35E1 ± 2
Response
Feedback:
Iodine and bromine react as shown below:
I
2
(g) + Br
2
(g) 2IBr (g). If 0.531 mol of I
2
and 0.531 mol of Br
2
are placed into a sealed 1.00 L Òask, and at
equilibrium the Òask contains 0.88 mol of IBr, what is the
value of the equilibrium constant,
K
eq
? (Hint: you will needed to Ñgure out the amounts of each substance at equilibrium using
stoichiometry, before you can substitute into the equilibrium expression. An ICE table can
help you organize this type of data. )
First calculate the concentrations at equilibrium using stoichiometry. They
substitute the concentrations into the equilibrium expression to Ñnd the value
of K
eq
.
Question 7
Selected Answer:
Correct Answer:
Response
Feedback:
The equilibrium constant is given for two of the reactions below. Determine the value of the
missing equilibrium constant. A(g) + 2B(g) AB
2
(g) Kc = 59 AB
2
(g) + B(g) AB
3
(g) K
c
= ? A(g) + 3B(g) AB
3
(g) K
c
= 478
8.1
8.1
If you multiply an equation by a number, you raise the equilibrium
constant to that power.
If you reverse a reaction, you take the reciprocal of the equilibrium
constant.
If you add two equations, you multiply their equilibrium constants.
1 out of 1 points
1 out of 1 points
Question 8
Selected
Answer:
Correct
Answer:
Response
Feedback:
Consider the following reaction at equilibrium. What eÖect will adding some graphite have on
the system? CO
2
(g) + C(graphite) 2 CO(g)
No eÖect will be observed since C is not included in the equilibrium
expression.
No eÖect will be observed since C is not included in the equilibrium
expression.
Because the equilibrium is heterogeneous, the solid does not appear in the
equilibrium expression and therefore adding and subtracting graphite will not
shift the equilibrium.
Question 9
Selected Answer:
Correct Answer:
Response
Feedback:
An aqueous solution of ________ will produce an acidic solution.
NH
4
NO
3
NH
4
NO
3
Conjugate bases of strong acids are neutral (i.e. not bases).
(Based on the list of seven strong acids, this mean the ions HSO
4
-
, NO
3
-
, I
-
, Br
-
,
Cl
-
, ClO
3
-
, and ClO
4
-
can form neutral salts.
Group I and II cations form neutral salts, but since ammonium is the conjugate
base of a weak acid (ammonia) it forms an acidic salt.
Anions that are conjugate bases of weak acids form basic salts.
Question 10
Selected Answer:
Correct Answer:
Response
Feedback:
What is the conjugate acid of HCO
3
-
?
H
2
CO
3
H
2
CO
3
An acid donates a proton which is accepted by the lone pair of the
base.
Therefore,
the substance with the added proton is the
conjugate
acid.
1 out of 1 points
1 out of 1 points
1 out of 1 points
Question 11
Selected Answer:
4.66
Correct Answer:
4.66 ± 0.02
Response
Feedback:
What is the expected pH of a nitric acid solution , HNO
3
, with a concentration of 2.21 x 10
-5
M?
Enter your answer in decimal format with two decimal places (value ± 0.02).
Practice Exam 2.2
Practice Exam 2.2
Question 12
Selected Answer:
Correct Answer:
Use the following table of data in answering the question below the table:
Acid Name
Formula
pK
a
pK
b
Conjugate
Base
Hydrofluoric acid
HF
3.17
10.83
F
-
Nitrous acid
HNO
2
3.25
10.75
NO
2
-
Hypochlorous acid
HOCl
7.54
6.46
OCl
-
Hypobromous acid
HOBr
8.62
5.38
OBr
-
Hydrocyanic acid
HCN
9.21
4.79
CN
-
Ammonium
NH
4
+
9.24
4.76
NH
3
The acid HN
3
has a pK
a
of 4.72. How many of the conjugate bases shown in the table are stronger
bases than the base N
3
-
?
4
4
1 out of 1 points
1 out of 1 points
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Response
Feedback:
Practice exam 2.4
Practice exam 2.4
Question 13
Selected Answer:
12.34
Correct Answer:
12.34 ± 0.02
Response
Feedback:
At 25º C , what is the pH of a solution prepared by dissolving 0.00823 mol of Ca(OH)
2
in water to give
756.5 mL of solution?
Enter your answer in decimal format with two decimal places (value ± 0.02).
Practice exam 2 5
Practice exam 2 5
Question 14
A weak acid, HA, is dissolved in water given a solution concentration of 0.152 M. The percent dissociation
(ionization) is measured and found to be 8.4%. Based on these data, what is the value of K
a
for this weak
acid?
1 out of 1 points
1 out of 1 points
Selected Answer:
1.17E-3
Correct Answer:
1.17E-3 ± 5%
Response
Feedback:
Enter your answer in exponential format using a capital "E"
(example 1.23E-4) and no units (value ± 5%).
Practice exam 2 6
Practice exam 2 6
Question 15
Selected Answer:
12.26
Correct Answer:
12.27 ± 0.02
Response
Feedback:
Calculate the pH of a 0.362 M solution of a base with a base dissociation constant of K
b
= 9.78 x 10
-4
.
Enter your answer in decimal format with two decimal places (value ± 0.02).
Practice exam 2 7
Practice exam 2 7
1 out of 1 points
Question 16
Selected Answer:
11.12
Correct Answer:
11.12 ± 0.02
Response
Feedback:
At 25º C, what is the pOH of a buÖer that consists of 0.651 M HA and 0.472 M NaA?
HA represents a weak acid with a K
a
of is 9.45 x 10
-4
and NaA represents the conjugate base.
Enter your answer in decimal format with two decimal places (value ± 0.02). Practice exam 2 8
Practice exam 2 8
Question 17
Selected Answer:
8.16
Correct Answer:
8.16 ± 0.02
Response
Feedback:
At 25º C, what is the pH of a 0.152 M aqueous solution of potassium Òuoride (KF) given that the K
a
of
hydroÒuoric acid (HF) is 7.24 x 10
-4
.
Enter your answer in decimal format with two decimal places (value ± 0.02).
1 out of 1 points
1 out of 1 points
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Practice exam 2 9
Practice exam 2 9
Question 18
Selected Answer:
False
Correct Answer:
False
Response
Feedback:
True or false:
The pH at the equivalence point is always pH = 7.
If a weak acid is titrated with a strong base, at the equivalence point, the pH will be greater
than 7, (pH > 7).
If a strong acid is titrated with a strong base, at the equivalence point, the pH will be equal
to 7, (pH = 7).
If a weak base is titrated with a strong acid, at the equivalence point, the pH will be less
than 7, (pH < 7).
Practice exam 2.10
Practice exam 2.10
Question 19
1 out of 1 points
1 out of 1 points
Selected Answer:
25.51
Correct Answer:
25.51 ± 1%
Response
Feedback:
Determine the volume in mL of 0.378 M HClO
4
(aq) needed to reach the half-equivalence (stoichiometric)
point in the titration of 53.71 mL of 0.359 M ammonia, NH
3
. The K
b
of ammonia is 1.8 x 10
-5
.
Enter your answer in decimal format with two decimal places (value ±1%).
Practice Exam 2 11
Practice Exam 2 11
Question 20
Selected Answer:
4.07
Correct Answer:
4.07 ± 0.02
Response
Feedback:
A 25.00 mL sample of 0.150 M monoprotic organic acid is titrated with aqueous sodium hydroxide. After
6.42 mL of 0.150 M NaOH is added, what is the pH of the solution?
The K
a
of the acid is 2.97 x 10
-5
.
Enter your answer in decimal format with two decimal places (value ± 0.02).
1 out of 1 points
Practice Exam 2 12
Practice Exam 2 12
Question 21
Selected Answer:
10.42
Correct Answer:
10.61 ± 0.04
Response
Feedback:
One liter of a buÖer is prepared with concentrations of 0.250 M C
2
H
5
NH
2
and 0.250 M C
2
H
5
NH
3
Cl. If
2.13 g of NaOH is then added, what is the resulting pH?
Assume the solution volume does not change
and that K
b
of C
2
H
5
NH
2
is 2.64 x 10
-4
.
Enter your answer in decimal format with two decimal places (value ± 0.04).
Practice exam 2 13
Practice exam 2 13
Question 22
0 out of 1 points
1 out of 1 points
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Thursday, May 6, 2021 3:37:55 PM CDT
Selected Answer:
5.55
Correct Answer:
5.55 ± 0.02
Response
Feedback:
The weak base methylamine, CH
3
NH
2
, is titrated with HI
. What is the pH at the equivalence point, if the
concentration of methylammonium iodide, CH
3
NH
3
I
, is known to be 0.348 M?
The K
b
of CH
3
NH
2
is 4.4 x 10
-4
.
Enter your answer in decimal format with two decimal places (value ± 0.02).
Practice exam 2 14
Practice exam 2 14
←
OK
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How would each of the following change the rate the reaction shown here?
2NO (g) + 2H2 (g)
(8)
a. Adding some NO (g)
, N2(g)+2H,0(g)
(8)
b. Decreasing the temperature
C.
Removing some H2 (g)
d. Adding a catalyst
D Focus
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Alchemy Lesson 20 & 21 Worksheet
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Andres Carrillo - Alchemy Lessons 20 & 21 Worksheet
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AIV-20: Getting Connected (Writing lonic Compounds)
Part 1: Putting together lonic Compounds
lonic compound
Metal
Number of
cation
nonmetal
number of
anion
total
total charge = 0
valence
valence
number of
electrons
electrons
valence
electrons
NaF, sodium fluoride
Na
Na +
(+1)+(-1) = 0
F-
8.
MgO, magnesium oxide
Mg
02-
(+2) + (-2) = 0
MgCl2, magnesium
chloride
Mg
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7
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(+2) + 2(-1) = 0
Ne, neon
Ne
8
BeF2, beryllium fluoride
Be
MgS, magnesium sulfide
CaCl,, calcium chloride
Na
Br
K
Se
Al
Al203, aluminum oxide
Al
Al
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Using a chemical equation to find moles of product from moles ...
with
Ammonium phosphate ((NH4), PO4)
is an important ingredient in many solid fertilizers. It can be made by reacting aqueous phosphoric acid (H, PO,)
liquid ammonia. Calculate the moles of ammonium phosphate produced by the reaction of 0.10 mol of ammonia. Be sure your answer has a unit symbol, if
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Write the corresponding letters to the following descriptions. Each proposal can be associated with 0 or
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a. [Ar] 4s?
b. 1s 2s2p63s23p3
c. 1s2s2p2
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HN-HO-HƆ
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Group-12 )436 9 10 11 12 13 14 15 16 17 10
Irerlod
The Perlodic Table of the Elements
Elements in the same group tend to have similar characteristics, but some things like tendency to gain or lose electrons can still vary
even within a group Which of the following is true regarding the elements in group 2?
O A Be, Beryllium is the largest and has the greatest tendency to gain electrons.
OB Be Beryllium and Ba, Barium will have the same tendancy to lose electrons
OC Ra, Radium is the smallest and will have the greatest tendency to lose electrons.
O D. Ba, Barium will have a greater tendency to lose electrons than Mg, Magnesium.
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C12H22O11 + O₂
CO₂ + H₂O
Mg(OH)2 + H₂SO4
MgSO4 + H₂O
NaOH + CuSO4 -Na2SO4 + Cu(OH)2
CH2 + Oz = H2O + CO2
Fe + 0₂ Fe₂O3
Mg3(PO4)2 + H₂ Mg + H3PO4
NH4NO3-N₂O + H₂O
Cl₂ + KBr KCI + Br₂
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Solving for a reactant using a chemical equation
Green plants use light from the Sun to drive photosynthesis. Photosynthesis is a chemical reaction in which water (H,0) and carbon dioxide (CO, chemically
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What mass of carbon dioxide is consumed by the reaction of 8,82 g of water?
Be sure your answer has the correct number of significant digits.
Explanadon
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4. Determine and draw the structure corresponding to the spectral information provided
below. As you make this determination, complete the table below. Explain what clues you
used to determine the structure.
B
C10H12O
Signal
б
ABCDE
~7.8
~7.2
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O GASES
Calculating partial pressure in a gas mixture
Jacqueline v
A 7.00 L tank at 21.9 °C is filled with 5.47 g of sulfur hexafluoride gas and 5.98 g of boron trifluoride gas. You can assume both gases behave as ideal gases
under these conditions.
Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits.
mole fraction:
sulfur hexafluoride
partial pressure:
atm
mole fraction:
boron trifluoride
partial pressure:
atm
Total pressure in tank:
atm
Explanation
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Calculating partial pressure in a gas mixture
Jacqueline
A 5.00 L tank at 7.37 °C is filled with 18.2 g of chlorine pentafluoride gas and 3.28 g of boron trifluoride gas. You can assume both gases behave as ideal gases
under these conditions.
Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits.
圖
mole fraction:
chlorine pentafluoride
partial pressure:
| atm
mole fraction:
boron trifluoride
partial pressure:
| atm
Total pressure in tank:
| atm
Explanation
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1400 -
1200 -
-C
dlo
1000 -
800
Ar
energy (z)
B
600 -
-A
400.
200-
Use this diagram to complete the table below.
What is the energy of the electron in the ground state?
What is the energy of the electron in the first excited
state?
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CHEM 3428 Worksheet 3
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use complete sentences. Use correct units when applicable.
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1. (3 pts) Draw a scheme for the epoxidation with Oxone reaction. Include all reagents and
reaction conditions.
2. (3 pts) What is the theoretical yield of this reaction as described in the procedure section
of the module page in mmol and in g? Report the theoretical yield using proper format.
Show all your calculations.
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It takes 155 s for an unknown gas to effuse through a porous wall and 97 s for the same volume of N2
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If 24.0 g of NaOH is added to 0.650 L of 1.00 M
Cu(NO:)2, how many grams of Cu(OH)2 will be
formed in the following precipitation reaction?
2 NaOH(aq) + Cu(NO:)>(aq) → Cu(OH)2 (s) + 2
NaNO:(aq)
g
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BIUA
三===|= |=▼=-EE|X
Nomal text
Calibri
12
1.
2 I 3. I 4 I 5 I 6 7 8 I 9 10
Potassium,
Calcium,
Gallium,
Germanium
Bromine,
Krypton,
Kr
Arsenic,
Selenium,
Ca
Ga
Ge
As
Se
Br
Alchemy Lesson 18: Life on the Edge & Lesson 19: Noble Gas Envy (Valence & Core Electrons)Page 3 of 4
PART 2: Use your completed table to answer the questions below.
1. List three things that all the atoms of the elements in period 3 have in common.
2. Explain why the number of electrons in the third shell changes from 8 to 18 between the element calcium, Ca, and the element gallium, Ga.
. 3. Summarize at least three patterns you discovered during this lesson.
4. Predict the electron arrangement of tin, Sn. Draw a shell model of it.
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SPECTRA FOR HOMEWORK 11, CHE 230 002
This page is not to be submitted to Gradescope. Use these spectra as you answer questions on the Homework 11 document.
Spectra for Problem 1
100
%T
80
60
40
20
Relative Intensity
4000
100-
80
8
60-
40-
20-
0
20
2H 2H
3000
m/z
50.0
75.0
76.0
155.0
157.0
183.0
185.0
212.0
214.0
100.0
97.5
11.8
11.7
1686 cm
40 60 80
2000
rel, intensity
11.9
16.9
17.6
28.8
27.8
Wavenumber[cm-1]
100
120
m/z
1500
7.90 7.85 7.80 7.75 7.70 7.65 7.60 7.55
1588 cm²
20 20 ₂
مسلسل..............للمسلسل
ppm
140 160 180 200 220
2H
1000
3.12
3.00 2.95 2.90
3H
500 400
A. Propose a
molecular
formula
for this
compound
B. Propuse.
a structure
selected
1.25 1.20 1.15
201
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