Fall 2023 CHEM 1113 Exam 2 final version-2
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CHEMISTRY 1113 EXAM 2 October 17, 2023 Drs. Carlon, Pochas, & Wise P
LEASE READ THIS COVER PAGE AND FOLLOW THE INSTRUCTIONS
. D
O NOT OPEN THE EXAM UNTIL YOU ARE TOLD TO DO SO
. On the computer graded answer sheet in the appropriate boxes, enter your: 1.
name
2.
student identification number
3.
recitation section
(In the four columns labeled “Section ID”, using a zero before your recitation section number. Ex., section 110 is written as 0110.) Then fill in the corresponding bubbles
below your name, ID number, and recitation section. Answer all questions on the computer graded answer sheet by filling in the proper bubble with a No. 2 pencil. If you change an answer, erase the undesired mark thoroughly. Mark only the best answer to each question. Cell phones must be turned off; all electronic devices must be placed in a backpack or on the floor and may not be accessed during the exam. Students violating this policy will be asked to leave and will receive a zero for the exam. A Periodic Table is printed on the back of this cover sheet. There are 6 exam pages (double-sided) with 25 questions. Each question is worth 6 points for a total of 150 points. Scratch paper is on the back of the exam. When you are instructed to begin the exam, please check that you have all the pages. When you are finished, give the answer sheet to your teaching assistant. You may take the exam with you. Answers will be posted on the Canvas class webpage at the completion of the exam. Good luck! Useful Information: ∆𝐻
?𝑥?
?
= Σ𝑛
????????
Δ𝐻
?,????????
?
− Σ𝑛
??𝑎??𝑎???
Δ𝐻
?,??𝑎??𝑎???
?
ΔU = q + w
w = –PΔV
Heat capacity = q/ΔT
q = m∙c∙ΔT
Specific heat capacity of water c = 4.184 J/g∙K
Density of water = 1.00 g/mL 1 cal = 4.184 J 1 J = 1 kg∙m
2
/s
2 Avogadro’s number:
6.022 × 10
23
entities/mol 101.325 J = 1 L·atm
Solubility Rules for Ionic Compounds in Water Cn Nh Fl Mc Lv 117 Ts (293) Og
CHEMISTRY 1113 Exam 2 Page 1 of 6 1.
How many moles of water molecules are in a sample of water which contains 2.70 x 10
22
hydrogen atoms? A. 4.48 x 10
-2
mol B. 1.63 x 10
46
mol C. 2.24 x 10
-2
mol D. 8.13 x 10
45
mol 2.
Calculate the mass percent of sulfur
in the compound sulfuric acid, H
2
SO
4
. A. 32.7 % B. 65.3% C. 2.04% D. 38.1% 3.
Which of the following compounds have empirical formulas identical
to their molecular formulas? A. Antifreeze; C
2
H
6
O
2
B. Isopropanol; C
3
H
8
O C. Glucose; C
6
H
12
O
6
D. None of the above compounds have empirical formulas identical to their molecular formulas 4.
Despite its name, theobromine, a molecule found in chocolate, consists only of carbon, hydrogen, oxygen, and nitrogen. A 180. g sample of theobromine contains 84.01 g carbon, 55.98 g nitrogen, 31.97 g oxygen, and the rest is hydrogen. What is the correct empirical formula of theobromine? A. C
4
H
4
N
2
O
B. C
7
H
8
N
4
O
2 C.
C
3
H
4
N
2
O D. C
7
H
8
N
2
O 5.
When the following equation for the combustion of decane (C
10
H
22
) is balanced using the smallest ratio of whole numbers, what is the coefficient for water
? C
10
H
22
(
l
) + O
2
(
g
) → CO
2
(
g
) + H
2
O(
g
) A. 22 B. 11 C. 20 D. 36
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Page 2 of 6 Exam 2 CHEMISTRY 1113 6.
What is the correct classification of the following reaction: 2 Fe(
s
) + 3 O
2
(
g
) → Fe
2
O
3
(
s
) A. Synthesis and neutralization B. Synthesis only C. Synthesis and combustion D. Combustion and double displacement 7.
Which of the following images below best represents what happens when aqueous solutions of MgBr
2
and KCH
3
COO are mixed? A.
B. C. D. 8.
Consider the reaction between aqueous solutions of perchloric acid (HClO
4
) and potassium hydroxide (KOH). Which ions are spectator
ions? A. Hydrogen and hydroxide ions B. Hydroxide and perchlorate ions C. Hydrogen and potassium ions D. Perchlorate and potassium ions 9.
What is the oxidation number of chromium in the polyatomic ion dichromate, Cr
2
O
7
2-
? A. +6 B. -2 C. +3 D. -3 10.
Consider the following balanced
redox reaction: 3 CuO(
s
) + 2 NH
3
(
aq
) → N
2
(
g
) + 3 H
2
O(
l
) + 3 Cu(
s
) [
balanced
] Which of the following statements is true
? A. CuO(
s
) is the reducing agent and CuO(
s
) is oxidized. B. CuO(
s
) is the oxidizing agent and CuO(
s
) is reduced. C. NH
3
(
aq
) is the reducing agent and H
2
O(
l
) is reduced. D. CuO(
s
) is the oxidizing agent and NH
3
(
aq
) is reduced. = Mg
2+ = Br
-
= K
+ = CH
3
COO
-
CHEMISTRY 1113 Exam 2 Page 3 of 6 11.
Consider the following unbalanced equation: Ag
2
O(
s
) + Al(
s
) →
Al
2
O
3
(
s
) + Ag(
s
) [
unbalanced
] How many moles of silver form when 6.0 grams of aluminum react? A. 72 mol B. 0.074 mol C. 480 mol D. 0.67 mol 12.
Consider the unbalanced
reaction shown below. If 10 moles of A
2
and 4 moles of B
2
react, which reactant is limiting and how much of the excess reactant remains? A
2 + B
2
→ A
2
B [
unbalanced
] A. A
2
is limiting, 1 moles B
2
leftover B. A
2
is limiting, 2 mole B
2
leftover C. B
2
is limiting, 5 moles A
2
leftover D. B
2
is limiting, 2 moles A
2
leftover 13.
How many grams of solid PbCl
2
form when 15.3 g of NaCl(
aq
) reacts with 60.8 g of Pb(NO
3
)
2
(
aq
) according to the balanced
chemical equation shown below? 2 NaCl(
aq
) + Pb(NO
3
)
2
(
aq
) → 2 NaNO
3
(
aq
) + PbCl
2
(
s
) [
balanced
] Molar Mass
: NaCl –
58.44 g/mol Pb(NO
3
)
2
–
331.21 g/mol PbCl
2
–
278.11 g/mol A. 36.4 g PbCl
2
B. 43.8 g PbCl
2 C. 51.1 g PbCl
2
D. 87.5 PbCl
2 14.
What is the actual yield for a reaction that, in theory, should produce 21.2 g of product with a 91.6% yield? A. 23.1 g B. 19.4 g C. 252 g D. 91.6 g 15.
The maximum concentration of a poisonous solute in drinking water is 2.00 x 10
-3
mg/L. What is the molarity of the solution if the molar mass of the solute is 62.49 g/mol? A. 3.20 x 10
-5
M
B. 1.25 x 10
-4
M
C. 3.20 x 10
-8
M
D. 1.25 x 10
-1
M
Page 4 of 6 Exam 2 CHEMISTRY 1113 16.
Shown below is a 100. mL sample of an aqueous stock solution. If 300. mL of water is added to 100. mL of the stock solution, which of the following depicts 100. mL of the new solution? A. B. C. D. 17.
What volume of 0.800 M
HCl is necessary to dissolve a CaCO
3
pearl which weighs 4.00 grams? 2 HCl(
aq
) + CaCO
3
(
s
) →
CaCl
2
(
aq
) + H
2
O(
l
) + CO
2
(
g
) [
balanced
] A. 25.0 mL B. 36.5 mL C. 50.0 mL D. 100. mL 18.
A system gains 575 J of heat and does 425 J of work on the surroundings. Calculate the change in internal energy, Δ
U
, of the system. A. -150 J B. 150 J C. -1000 J D. 1000 J 19.
Consider a system consisting of a metal cylinder that contains a gas which is sealed on the top by a movable piston. An external heat source is used to increase the temperature of the cylinder and the gas. The gas then expands and pushes the piston upwards. What are the signs of q and w of the system in this scenario? A. q < 0, w < 0 B. q > 0, w > 0 C. q < 0, w > 0 D. q > 0, w < 0
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CHEMISTRY 1113 Exam 2 Page 5 of 6 20.
Three metal blocks (X, Y, and Z), each weighing 25.0 g absorb equal amounts of heat. If the specific heat of Y is greater than Z, but less than X, arrange the final temperatures of the metal blocks in increasing order. Assume they all started with the same initial temperature. A. Z < Y < X B. Y < Z < X C. X < Y < Z D. X < Z < Y 21.
Consider water which has a heat capacity of 4.18 J/g·°C. How much heat energy is transferred if you heat your bathtub water from room temperature (25 °C) to 38°C. Assume your bathtub holds 70. gallons of water and the density of the water is 1.00 g/mL. (1 gallon = 3,785 mL). A. 5.4 x 10
1
J B. 4.8 x 10
3
J C. 8.2 x 10
5
J D. 1.4 x 10
7
J 22.
When 50.0 mL of 0.100 M
AgNO
3
is combined with 50.0 mL of 0.100 M
HCl in a coffee-
cup calorimeter, the temperature of the surrounding changes from 23.400°C to 24.210°C. Assuming a density of 1.00 g/mL of the solution and a heat capacity of 4.184 J/g·°C, calculate ΔH
rxn
. A. 3.50 J B. 339 J C. - 339 J D. -3.50 J 23.
At constant pressure, how much heat is released from the combustion of 100.0 g of hydrogen, according to the balanced
thermochemical equation below? 2 H
2
(
g
) + O
2
(
g
) →
2 H
2
O(
l
) Δ
H
rxn
= -571.6 kJ A. 1.415 x 10
4
kJ B. 1.155 x 10
5
kJ C. 2.829 x 10
4
kJ D. 5.773 x 10
4
kJ
Page 6 of 6 Exam 2 CHEMISTRY 1113 24.
Calculate ΔH°
rxn
for the oxidation of CO to CO
2 given the thermochemical reactions below: 2 CO(
g
) + O
2
(
g
) → 2 CO
2
(
g
) ΔH°
rxn = ? C(s) + O
2
(g) → CO
2
(
g
) ΔH°
rxn = -393.5 kJ 2C(s) + O
2
(g) → 2 CO(
g
) ΔH°
rxn = -221.0 kJ A. -173 kJ B. - 566 kJ C. -615 kJ D. -1008 kJ 25.
Consider the following balanced
reaction for the synthesis of tricarbon dioxide: 2 CO(
g
) + C(
s
) →
C
3
O
2
(
g
) [
balanced
] Calculate the reaction enthalpy (
ΔH°
rxn
) using the given standard enthalpies of formation. A. -314.6 kJ B. 16.9 kJ C. 127.4 kJ D. Δ
H
°
f of C(
s
) is needed for this calculation. Compound Δ
H
°
f (kJ/mol) CO(g) -110.5 C
3
O
2
(g) -93.6
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