Recitation Worksheet Eight
pdf
keyboard_arrow_up
School
University Of Georgia *
*We aren’t endorsed by this school
Course
1110
Subject
Chemistry
Date
Apr 3, 2024
Type
Pages
23
Uploaded by BailiffWillpower14880
Recitation Worksheet Eight (Ch. 6.2 (calorimetry)-6.4) Name: UGA ID:
Instructions: §
Please enter your first and last name as it appears on the eLC roster (do not use a nickname that is not reflected in eLC). §
Your UGA myID is a combination of letters and numbers (example: mine is jmj81738). Do not
enter your 81x number. §
Download this worksheet and print it if you have a printer. Write the answers in the answer boxes and show your work when appropriate. Using the instructions in the Welcome module on eLC, convert your worksheet to a PDF and then upload it to Gradescope. If you have an iPhone or Android device, you can scan and upload directly through the Gradescope app. The pages must be in the correct order
or Gradescope will not be able to read it. §
If you do not have a printer, download the worksheet and type your answers in the answer boxes and upload it to Gradescope. Write your work on separate sheets of paper, convert these pages to a PDF using the instructions in the Welcome module on eLC, then upload them to the dropbox on eLC for this worksheet. §
If you are using an app to annotate the worksheet, make sure the pages are in the correct order and have the same layout as the original
or Gradescope will not be able to read it. §
Answers must be written in the corresponding answer box or no credit will be awarded. §
This worksheet is due no later than 9:00 AM on the Saturday of the recitation week.
§
The instructions for uploading worksheets to Gradescope can be found in the Content area of eLC in the Welcome Module. §
You must show your work to receive credit. §
A periodic table and formula sheet are attached to the end of this worksheet. Please keep these attached to your worksheet in the correct order when submitting to Gradescope.
1. What is false
about a coffee-cup calorimeter? A. It is a form of constant-pressure calorimetry B. Any heat change by the system is equal but opposite to the heat change of the calorimeter C. The heat exchanged measured must have correction made for PV work before the enthalpy can be calculated D. The heat exchanged is equal to the enthalpy change E. More than one of the above is false
2.
A student goes to lab and mixes two solutions together that are both originally at
room temperature causing a reaction to occur. After mixing, the student notes that the
temperature of the solution decreases. Which of the following statements are true
?
Select any that apply.
A. The reaction is absorbing energy
B. The reaction is releasing energy
C. The reaction is exothermic
D. The reaction is endothermic
3. In a coffee-cup calorimeter, 51.0 mL of 0.100 M Ba(NO
3
)
2
and excess H
2
SO
4
are
mixed to yield the following reaction:
Ba
2+
(aq) + SO
4
2-
(aq) → BaSO
4
(s) The two solutions were initially at 23.00 °C, and the final temperature is 23.80 °C. Calculate the heat that accompanies this reaction in kJ/mol of BaSO
4
formed. Assume that the combined solution has a mass of 102.0 g and has a specific heat capacity of 4.18 J/g·°C. A. -67 kJ/mol
B. -340 kJ/mol
C. -5.1 × 10
-3
kJ/mol
D. -0.34 kJ/mol
E. -6.7 × 10
4
kJ/mol F. 67 kJ/mol
4. A student wants to use calorimetry to study the precipitation reaction of sodium carbonate and lead(II) nitrate according to the balanced reaction below: Na
2
CO
3
(aq) + Pb(NO
3
)
2
(aq) → 2 NaNO
3
(aq) + PbCO
3
(s)
They add 100. mL aliquots each of the two salts to a calorimeter with 200. mL of water (for a total final volume of 400. mL) and observe an increase in temperature of 0.999 °C. If the density of the mixture is 1.03 g/mL and the specific heat of the calorimeter is 4.18 J/g·°C, what was the original molarity of the lead(II) nitrate if they know sodium carbonate was in excess? The heat of precipitation in kJ/mol of lead(II) carbonate is -25.2 kJ/mol. Report your answer in standard notation
. M
Your preview ends here
Eager to read complete document? Join bartleby learn and gain access to the full version
- Access to all documents
- Unlimited textbook solutions
- 24/7 expert homework help
5. Under what condition(s) is bomb calorimetry performed? 6. A 7.10 g sample of aniline (C
6
H
5
NH
2
, molar mass 93.13 g/mol) was combusted in a bomb calorimeter with a heat capacity of 13.87 kJ/°C. If the initial temperature was 25.8°C, what is the final temperature of the calorimeter? The heat of combustion for aniline is -3.20 ´
10
3
kJ/mol. Report your answer in standard notation
. °C A. Constant temperature B. Constant volume C. Constant pressure D. Both constant volume and pressure E. None of the above
7. A new biofuel is being tested in a bomb calorimeter. The bomb calorimeter has a heat capacity of 11.2 kJ/K. If 0.9884 g of the biofuel is combusted, causing the temperature of the calorimeter to rise by 2.76 K, what is the heat of combustion of the biofuel in kJ per gram of the biofuel? Report your answer in standard notation
.
kJ/g 8. A student goes to the lab to perform a bomb calorimetry experiment using 7.00 grams of an organic compound. Upon combustion, they note a temperature increase from 25.50 °C to 33.50 °C in their bomb calorimeter. Based on this information, what was the heat capacity of the calorimeter in kJ/°C? The molar mass of the compound is 342.34 g/mol and its heat of combustion is -1.917 × 10
3
kJ/mol. Report your answer in standard notation
. kJ/°C
9. A 25.0 g sample of gold is heated to 90.00 °C and placed in 155 mL of cyclohexane (d = 0.779 g/cm
3
). After some time, the temperature of both the cyclohexane and gold reaches a final temperature of 24.05 °C. Assuming no heat is lost to the surroundings, what was the original temperature of cyclohexane (in °C)? Report your answer to three significant figures
and standard notation
.
Specific heat of gold = 0.129 J/g·°C Specific heat of cyclohexane = 1.85 J/g·°C °C
Your preview ends here
Eager to read complete document? Join bartleby learn and gain access to the full version
- Access to all documents
- Unlimited textbook solutions
- 24/7 expert homework help
10. What is true of the reaction represented by the following diagram? Select any that
apply.
A. It is endothermic
B. It is exothermic
C. 824.2 kJ of heat are released when 1 mole of Fe
2
O
3
(s) is formed
D. 1648.4 kJ of heat are absorbed when 2 mole of Fe (s) and 3 moles of O
2
(g) react
E. 1648.2 kJ of heat are absorbed when 2 moles of Fe
2
O
3
(s) is formed
11. Consider a hypothetical reaction below...
4 A + 3 B ®
5 C + 9 D D
H
rxn
= 525.0 kJ ...then determine D
H
rxn
of the hypothetical reactions below using this information. Report your answers to four significant figures
and standard notation
. 10 C + 18 D ®
8 A + 6 B D
H
rxn
= kJ A + 3
4
B ®
5
4
C + 9
4
D
D
H
rxn
= kJ
12. Determine D
H
rxn
for the reaction: Fe
2
O
3
(s) + 3 CO (g) ®
2 Fe (s) + 3 CO
2
(g) 2 Fe (s) + 3
2
O
2
(g) ®
Fe
2
O
3
(s) D
H
rxn
= -824.2 kJ CO (g) + 1
2
O
2
(g) ®
CO
2
(g) D
H
rxn
= -282.7 kJ Report your answer to three significant figures
and standard notation
. D
H
rxn
= kJ 13. Determine D
H
rxn
for the reaction: 5 C (s) + 6 H
2
(g) ®
C
5
H
12
(l) C
5
H
12
(l) + 8 O
2
(g) ®
5 CO
2
(g) + 6 H
2
O (g) D
H
rxn
= -3244.8 kJ C (s) + O
2
(g) ®
CO
2
(g) D
H
rxn
= -393.5 kJ 2 H
2
(g) + O
2
(g) ®
2 H
2
O (g) D
H
rxn
= -483.5 kJ Report your answer to four significant figures
and standard notation
. D
H
rxn
= kJ
14. Which of the following statements regarding standard states and standard
enthalpies of formation are false
? Select any that apply.
A. The standard state of a pure gas has a pressure equal to 1 torr
B. The standard state of a solution has a concentration equal to 1 M
C. The ΔH°
f
of a pure compound is the change in enthalpy when 1 or more moles of a
compound forms from its constituent elements regardless of their state (i.e. solid, liquid,
etc.)
D. A pure element in its standard state has a ΔH°
f
equal to 0
E. The ΔH°
f
of solid fluorine, F
2
(s), is equal to that of gaseous fluorine, F
2
(g), because
they have the same chemical composition
15. Which of the following elements below is not
in its standard state? Select any that
apply.
16. Which of the following is a standard formation reaction? Select any that apply.
A. O
2
(g) + 2 F
2
(g) ®
2 OF
2
(g)
B. Xe (l) + 2 F
2
(g) ®
XeF
4
(g)
C. Fe (s) + 3
2
Cl
2
(g) ®
FeCl
3
(s) D. Hg (s) + 1
8
S
8
(s) ®
HgS (s) E. 2 Br
2
(l) + C (graphite) ®
CBr
4
(s)
A. Na (s)
D. Hg (g)
B. Cl
2
(s)
E. S
8
(s)
C. Ne (l)
F. Ti (s)
Your preview ends here
Eager to read complete document? Join bartleby learn and gain access to the full version
- Access to all documents
- Unlimited textbook solutions
- 24/7 expert homework help
17. Which of the following correctly illustrates the ΔH°
f
of lithium sulfate? A. Li
2
SO
4
(s) ®
2 Li (s) + 1
8
S
8
(s) + 2 O
2
(g) B. Li
2
SO
4
(s) ®
2 Li
+
(aq) + SO
4
2-
(aq) C. Li
2
SO
4
(s) ®
2 Li (s) + 8 S (s) + 2 O
2
(g) D. 2 Li
+
(aq) + SO
4
2-
(aq) ®
Li
2
SO
4
(s) E. 2 Li (s) + 1
8
S
8
(s) + 2 O
2
(g) ®
Li
2
SO
4
(s) F. 2 Li (s) + 8 S (s) + 2 O
2
(g) ®
Li
2
SO
4
(s) 18. Determine ΔH°
rxn
for the reaction below using the given ΔH°
f
values in the table. SO
2
Cl
2
(g) + 2 H
2
O (l) ®
2 HCl (g) + H
2
SO
4
(l) Substance ΔH°
f
(kJ/mol) SO
2
Cl
2
(g) -364 H
2
O (l) -286 HCl (g) -92 H
2
SO
4
(l) -814 Report your answer to two significant figures
and standard notation
. kJ
19. Determine ΔH°
rxn
for the reaction below using the given ΔH°
f
values in the table.
CH
4
(g) + 4 Cl
2
(g) ®
CCl
4
(g) + 4 HCl (g) Substance ΔH°
f
(kJ/mol) CH
4
(g) -75
Cl
2
(aq) -23
Cl
2
(g) 0 CCl
4
(g) -96
HCl (g) -92
Report your answer to three significant figures
and standard notation
. kJ 20. What is ΔH°
f
for SO
3
(g) if the ΔH°
rxn
for the reaction below is -198 kJ?
2 SO
2
(g) + O
2
(g) ®
2 SO
3
(g) Substance ΔH°
f
(kJ/mol) SO
2
(g) -297
Report your answer to three significant figures
and standard notation
. kJ
Extra Practice Questions: these questions will not be graded. 1. A 5.45 g sample of calcium oxide is dissolved in a 101.50 g of water in a coffee cup calorimeter. Afterward, the temperature of the solution is observed to increase from 23.4 °C to 41.2 °C. If the specific heat of the solution is 4.18 J/g·°C, what is the enthalpy change for the reaction of CaO with water (shown below) in kJ/mol? Report your answer in standard notation
. CaO (s) + H
2
O (l) → Ca(OH)
2
(aq) Hint: the mass of the solution is the sum of both calcium oxide and water. kJ/mol
Your preview ends here
Eager to read complete document? Join bartleby learn and gain access to the full version
- Access to all documents
- Unlimited textbook solutions
- 24/7 expert homework help
2. The heat capacity of a bomb calorimeter can be determined by burning 7.59 g of methane, which has an energy of combustion of -802 kJ/mol CH
4
. The temperature of the calorimeter was initially measured at 23.2 °C and rose to 31.2 °C. What is the heat capacity (kJ/°C) of the bomb calorimeter? Report your answer in standard notation
. kJ/°C 3. When 3.12 g of glucose, C
6
H
12
O
6
, is burned in a bomb calorimeter, the temperature of the calorimeter increases from 23.8 ºC to 35.6 ºC. The student running the experiment forgot to calibrate the calorimeter, but they know the calorimeter contains 775 g of water and the bomb instrument itself has a heat capacity of 893 J/ºC. Estimate the heat of combustion (kJ/mol) of the glucose sample. Report your answer in standard notation
.
Hint: the heat produced by the reaction is absorbed by the water and the bomb. kJ/mol
4. A 30.0 g sample of water at 280. K is mixed with 50.0 g water at 330. K. Calculate the final temperature (K) of the mixture assuming no heat loss to the surroundings. The specific heat capacity of water is 4.184 J/g·K. Report your answer in standard notation
. K
5. The combination of coke and steam produces a mixture called coal gas, which can be used as a fuel or as a starting material for other reactions. The equation for the production of coal gas is: 2 C(s) + 2 H
2
O (g) → CH
4
(g) + CO
2
(g) Determine the standard enthalpy change for this reaction based on the standard enthalpies of reaction below. Report your answer to three significant figures
and standard notation
. C (s) + H
2
O (g) → CO (g) + H
2
(g) D
H
rxn
= 131.3 kJ CO (g) + H
2
O (g) → CO
2
(g) + H
2
(g) D
H
rxn
= - 41.2 kJ CH
4
(g) + H
2
O (g) → 3 H
2
(g) + CO (g) D
H
rxn
= 206.1 kJ kJ
Your preview ends here
Eager to read complete document? Join bartleby learn and gain access to the full version
- Access to all documents
- Unlimited textbook solutions
- 24/7 expert homework help
6. Chlorine monofluoride can react with fluorine to form chlorine trifluoride: ClF (g) + F
2
(g) → ClF
3
(g) ∆
r
Hº = ??? Use the reactions below to determine ∆
r
Hº for the above reaction. 2 OF (g) → O
2
(g) + 2 F
2
(g) ∆
r
Hº = -49.4 kJ 2 ClF (g) + O
2
(g) → Cl
2
O (g) + OF
2
(g) ∆
r
Hº = +214.0 kJ ClF
3
(g) + O
2
(g) → 1/2 Cl
2
O (g) + 3/2 OF
2
(g) ∆
r
Hº = +236.2 kJ A. -104.5 kJ B. +2.5 kJ C. -153.9 kJ D. +367.9 kJ
7. Determine D
H
rxn
for the reaction: Zn (s) + 1
8
S
8
(s) + 2 O
2
(g) ®
ZnSO
4
(s) Zn (s) + 1
8
S
8
(s) ®
ZnS (s) D
H
rxn
= -183.92 kJ 2 ZnS (s) + 3 O
2
(g) ®
2 ZnO (s) + 2 SO
2
(g) D
H
rxn
= -927.54 kJ 2 SO
2
(g) + O
2
(g) ®
2 SO
3
(g) D
H
rxn
= -196.04 kJ ZnO (s) + SO
3
(g) ®
ZnSO
4
(s) D
H
rxn
= -230.32 kJ Report your answer to five significant figures
and standard notation
. D
H
rxn
= kJ
8.
Which of the following is not
a standard formation reaction at room temperature? You
may assume the states of matter of the products
are written in their standard state.
Select any that apply.
A. C (diamond) + O
2
(g) ®
CO
2
(g)
B. Cu (s) + 1
2
O
2
(g) ®
CuO (s) C. 2 Na (l) + Cl
2
(g) ®
2 NaCl (s)
D. As (s) + 1 1
2
H
2
(l) ®
AsH
3
(s) E. Ca (s) + C (graphite) + 3
2
O
2
(g) ®
CaCO
3
(s) 9.
Which of the following is a standard formation reaction at room temperature? You
may assume the states of matter of the products
are written in their standard state.
Select any that apply.
A. ½ H
2
(g) + ½ Cl
2
(g) → HCl (g)
B. 2 Na (s) + H
2
(g) + 2 C (s, graphite) + 3 O
2
(g) → 2 NaHCO
3
(s)
C. 3 Zn (s) + 2 P (g) → Zn
3
P
2
(s)
D. Sr (s) + Br
2
(g) → SrBr
2
(s)
E. Fe (s) + 1/8 S
8
(s) + 2 O
2
(g) → FeSO
4
(s)
Your preview ends here
Eager to read complete document? Join bartleby learn and gain access to the full version
- Access to all documents
- Unlimited textbook solutions
- 24/7 expert homework help
10. What is ΔH°
f
for IF (g) if the ΔH°
rxn
for the reaction below is -89 kJ? IF
7
(g) + I
2
(s) ®
IF
5
(g) + 2 IF (g) Substance ΔH°
f
(kJ/mol) IF
7
(g) -941 IF
5
(g) -840 Report your answer to two significant figures
and standard notation
. kJ/mol 11. Ethanol (C
2
H
5
OH) has been proposed as an alternative fuel. Calculate the standard enthalpy of combustion (kJ/mol) for ethanol. Substance ΔH°
f
(kJ/mol) C
2
H
5
OH (g) -278.0 CO
2
(g) -393.5 H
2
O (l) -286 Report your answer to four significant figures
and standard notation
. kJ/mol
Formula Sheet
Length
1 kilometer = 0.62137 mile 1 inch = 2.54 centimeters (exactly) 1 Å
ngstrom = 1 × 10
−10
meter Energy
1 joule = 1 kg·m
2
/s
2
1 calorie = 4.184 joules 1 Calorie = 1 kilocalorie = 1000 calories 1 L·atm = 101.325 joules Pressure
1 pascal = 1 N/m
3
= 1 kg/m·s
2
1 atmosphere = 101.325 kilopascals = 760 mm Hg = 760 torr = 14.70 lb/in
2
1 bar = 1 × 10
5
Pa (exactly) Temperature
0 K = −273.15°C
K = °C + 273.15
°C = (5/9)(°F − 32)
Mass
1 kg = 2.205 lbs Volume
1 mL = 1 cm
3
= 1 cc Constants
c = 2.998 × 10
8
m/sec h = 6.626 × 10
−34
J·sec R = 0.08206 L·atm/mol·K = 8.314 J/mol·K Specific heat of water = 4.184 J/g∙K
Mass of an electron: 9.109 x 10
−31
kg Mass of a proton: 1.673 x 10
-27
kg RH = 2.18 x 10
−18
J Specific heat of water = 4.184 J/g∙K
STP = 273.15 K and 1 atm Avogadro's number: 6.022 × 10
23
Equations d (density) = m/V P
1
V
1
=P
2
V
2
V
1
/T
1
=V
2
/T
2
P
1
V
1
/n
1
T
1
=P
2
V
2
/n
2
T
2
PV=nRT (P + a(n
2
/V
2
))·(V − nb) = nRT
molar mass (M) = mRT/PV density (d) = MP/RT x
A
= n
A
/n
tot = P
A
/P
tot
= V
A
/V
tot
Your preview ends here
Eager to read complete document? Join bartleby learn and gain access to the full version
- Access to all documents
- Unlimited textbook solutions
- 24/7 expert homework help
P
tot
= P
A
+ P
B
+ …
n
tot
= n
A
+ n
B
+ … 𝜇𝜇
𝑟𝑟𝑟𝑟𝑟𝑟
=
�
3
𝑅𝑅𝑅𝑅
𝑀𝑀
𝑅𝑅𝑅𝑅𝑅𝑅𝑅𝑅
𝑜𝑜𝑜𝑜
𝑅𝑅𝑜𝑜𝑜𝑜𝑒𝑒𝑒𝑒𝑒𝑒𝑜𝑜𝑒𝑒
𝐴𝐴
𝑅𝑅𝑅𝑅𝑅𝑅𝑅𝑅
𝑜𝑜𝑜𝑜
𝑅𝑅𝑜𝑜𝑜𝑜𝑒𝑒𝑒𝑒𝑒𝑒𝑜𝑜𝑒𝑒
𝐵𝐵
=
�
𝑀𝑀𝑀𝑀
𝐵𝐵
𝑀𝑀𝑀𝑀
𝐴𝐴
Q = C × ΔT = c
specific
× m × ΔT
Q = n × ΔH (kJ/mol) = m × ΔH (kJ/g)
w = −PΔV
ΔE = q + w
ΔH° = ΣnΔHf°(products) − ΣnΔHf°(reactants)
ΔH° = ΣnΔH°(bonds broken) − ΣnΔH°(bonds formed)
E=hν
c=λν
λ = h/mv ∆𝐸𝐸
= −
2.18 × 10
−18
𝐽𝐽
(
1
𝑒𝑒
𝑓𝑓
2
−
1
𝑒𝑒
𝑖𝑖
2
)
C
g
= kP
g P
solution
=P
solvent
X
solvent
P
solution
=∑P
j
=∑P
j
X
j
ΔT
b
= K
b
m
i
ΔT
f
= K
f
m
i
π
= MRT
i
Thermodynamic and Electrochemistry S = k
b
× ln(
W
) k
b
= 1.381 × 10
−23
J/K ΔS = q
rev
/T ΔS
surr
= q
surr
/T = −q
rev
/T ΔS
univ
= ΔS
sys
+ ΔS
surr
ΔS°
rxn
= Σ
ν
S°
products
− Σ
ν
S°
reactants
ΔH°
rxn
= Σ
ν
H°
products
− Σ
ν
H°
reactants
ΔG°
rxn
= Σ
ν
G°
products
− Σ
ν
G°
reactants
ΔG = ΔH – TΔS
∆
G = ∆
G° + RT∙lnQ
R=8.314 J/mol.K ∆
G° = −RT∙lnK
∆
G= −nFE
cell
F = 96485 J/(V∙mol e
−
) E°
cell
= RT/nF lnK
E°
cell
= (0.0257/n) lnK = (0.0592/n) logK
E
cell
= E°
cell
− (RT/nF) lnQ
E
cell
=E°
cell
− (0.0257/n) lnQ
Electrolysis: Q (total charge) = I × t = n × F
Your preview ends here
Eager to read complete document? Join bartleby learn and gain access to the full version
- Access to all documents
- Unlimited textbook solutions
- 24/7 expert homework help
Integrated Rate Laws & half-life
Equilibrium and Acid / Base K
P
= K
c
× (RT)
Δn
pH = −log[H
3
O
+
] K
w
= 1.0 × 10
−14
at 25 °C
K
w
= [H
3
O
+
] × [OH
−
] K
w
= K
a
× K
b
pK
a
= −log[K
a
] Buffer: pH = pK
a
+ log
ln
𝐾𝐾
2
𝐾𝐾
1
= ∆
𝐻𝐻
𝑟𝑟𝑟𝑟𝑟𝑟
°
𝑅𝑅
(
1
𝑇𝑇
1
−
1
𝑇𝑇
2
)
Your preview ends here
Eager to read complete document? Join bartleby learn and gain access to the full version
- Access to all documents
- Unlimited textbook solutions
- 24/7 expert homework help
Related Documents
Related Questions
True/False
Indicate whether the statement is true or false.
(2 marks)
1. A reaction XY occurs in a closed vessel. When it reaches equilibrium at temperature T, the
number of molecules changing from X to Y is equal to the number of molecules changing from Y
to X. (EQ1.1)
2. In an exothermic reaction, an increase in temperature favors the formation of products. (EQ1.6)
Multiple Choice
Identify the choice that best completes the statement or answers the question.
(10 marks)
1. Under suitable laboratory conditions, the products of many chemical reactions can be made to
directly react to re-form the reactants. Such reactions are described as (EQ1.1)
a. dynamic.
b. stressed.
c. reversible.
d. catalyzed.
2. The state of chemical equlibrium exists when (EQ1.1)
a. one of more of the products is a gas or a solid.
b. products of a reaction recombine to form reactants.
c. concentration of reactants and products are equal.
d. forward and reverse reaction are occurring at the same rate.
3. Which is…
arrow_forward
QUESTION 11
Write the condensed structural formula for the following molecule
H.
H.
C
N-
H.
For the toolbar, press ALT+F10 (PC) or ALT+FN+F10 (Mac).
B
IUS
Paragraph
Arial
10pt
A
Ix
x X,
次 T T
ΩΘ
Click Save and Submit to save and submit. Click Save All Answers to save all answers.
MacBook Pro
!!
!!!
+]
arrow_forward
(6)
H20, H30*
1) ВН3 THF
(7)
2) H2O2, OH
?
(8) (CH3)2C=CH2
(CH3)2CHCH2OH
arrow_forward
Hello, I need help with my chemistry hw. I have been trying to solve this for hours, thank you.
arrow_forward
(7)
KMNO4, NaOH
arrow_forward
If the enthalpy of C12H22O11 combustion is said to be -5.65 x 103 kJ/mol, calculate the mass of C12H22O11 needed to be burned to produce 2.6 kJ of heat. (MM of sucrose: 342.3)
arrow_forward
1.
2.
3.
4. Н
Н Н
С
H
C
Н
Н
Н Н H
H-C C C
Н
H
Н
Н
Н
Н
Н
Н Н
Н
мор
Н
Н
Hydrocarbon Reactions
Н
Н
Н
Н
Н
С10Н22(1) → С2Н6(9) + C7H16(l) + C(s)
C
Н
Н
C-H -
Н
·H + H — Н
Н
C
Н
H
с
Н
CH₂
+
Н Н
с
Н
C
Н
-H + H-
H
С
Н
Н
T
Н
c- c- Н
H
Н
arrow_forward
give the IUPAC name for the diagram
arrow_forward
Lab 10: Enthalpy of Neutralization
(7) Identify the limiting reagent and briefly explain why it is limiting. ds toad sdd sialla ()
Jed ofhioea sh ba Im & SO1 aew ouurbim
answer
wans
(8) Find AHneutzn for the reaction.
ardt gaieu mite bee momod asminolso ard yd bodioeda 1sod lo inuorms srlt sdaluole )
(A) S nobesuC ni batsluol Instenoo 1odsminol
answer
5wans
badioeds lesdl Intoi ont sisiuoin ()
O8.0 lo.im 0.001 bas HOM M0080 lo Jm 0.001 lo noibesnsdi yd boenslon tead Indot orl: bnit (a)
arrow_forward
Write the type of reaction that is occurring on the line provided then complete the reaction. Only include the
major products and any byproducts (e.g. H2O) but no minor products. Please use either full structural
diagrams or the combination method shown in the lesson. Skeletal/line diagrams will not be accepted.
H3C
1.
2.
3.
OH
Type of Reaction:
NH
Type of Reaction:
ა
C
CH3
Δ
Acid
+ H2O
Catalyst
+ HBr
Type of Reaction:
H3C
4.
Type Reaction:
CH2 + H2O
arrow_forward
What is the IUPAC name of the following compound?
Multiple Choice
bicyclo[2.2.2]octane
bicyclo[3.3.3]octane
bicyclo[2.2.2]hexane
bicyclo[3.3.3]hexane
arrow_forward
(4) Find the AH for the reaction below, given the following reactions and subsequent AH values:
CO₂(g) → C(s) + O₂(g)
H₂O(1)→ H₂(g)+ ½ O₂(g)
C₂H.(g)
2 C(s) + 3H₂(g)
2 CO₂(g) + 3 H₂O(1)→ C₂H(g) + ¹/₂O₂(g)
1
ΔΗ = 643 kJ
ΔΗ = 190,6 kJ
AH=3511.1 kJ
arrow_forward
pls help will rate u thank you!
arrow_forward
2. (20 points) An investor takes the position below on the same stock with a strike price of $100 and the same maturity:
Buy 1 XYZ call at $3.30
Buy 1 XYZ put at $3.20
Draw a graph to show the possible profit and loss. (don’t forget to show break-even points, strike price etc.) ***please draw a graph***
arrow_forward
Use the following two equations
a. ½ N2 (g) + O2 (g) à NO2 (g) dHo = +35 kJ
b. ½ N2 (g) + ½ O2 (g) à NO (g) dHo = +90.4 kJ
to calculate the dHo of
NO (g) + ½ O2 (g) à NO2 (g) dHo =
arrow_forward
5
(cont...)
Given -
- KMn 04 +
1
MASO4 + - CO₂ + -
a) A student
into
b) A student
a
-
- H₂C₂O4 +_ H₂SO4
flask.
mixes
and
mixes
a flask. Determine the
mixes
c) A student
H₂6204
why H₂SO4 cannot
an
->>
1.50 mol of each reactant
Determine the limiting reactant.
1.50g of each reactant into
limiting
reactant.
KMnO4 with 3.00 mol
1.00 mal
H₂0+
K₂SO4
excess
of H₂SO4. Explain
be the limiting reactant.
arrow_forward
1. (6.5 points) The preparation of aspirin is achieved through acetylation of salicylic acid. Provide the full curved-arrow
mechanism for this transformation. All starting materials, reagents, and products should be accounted for.
ཚེཚེས༔-༩ལིན་ཐིག
OH
OH
salicylic acid
H3C
+
H3C
H3PO4 (conc.)
CH3
CH3
50 °C to 0 °C
H3C
OH
OH
acetic anhydride
:O-P-OH
: OH
HO.
acetylsalicylic acid
(aspirin)
눈요
CH3
O-P-OH
: OH
H3C
CH3
H3C
H.
H
H3C-
acetic acid
::
CHEM 238
H3C
H3C
.0:
CH3
HO
H
но.
CH3
H-00
HO
Ή
OH
: OH
CH3
HO
CH3
CH3
но
HO-P―O:
I
HO:
H-O
Н
H3C-
H3C
: OH
1
arrow_forward
Please answer as soon as possibly and I will leave a like.
arrow_forward
Please correct answer and don't used hand raiting
arrow_forward
Using the thermodynamic information in the ALEKS Data tab, calculate the standard reaction free energy of the following chemical reaction:
4Fe (s)+30, (g)→ 2Fe,0, (s)
Round your answer to zero decimal places.
kJ
x10
Continue
O2021 McGraw Hill LLC. All Rights Reserved. Terms
arrow_forward
SEE MORE QUESTIONS
Recommended textbooks for you
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY
Related Questions
- True/False Indicate whether the statement is true or false. (2 marks) 1. A reaction XY occurs in a closed vessel. When it reaches equilibrium at temperature T, the number of molecules changing from X to Y is equal to the number of molecules changing from Y to X. (EQ1.1) 2. In an exothermic reaction, an increase in temperature favors the formation of products. (EQ1.6) Multiple Choice Identify the choice that best completes the statement or answers the question. (10 marks) 1. Under suitable laboratory conditions, the products of many chemical reactions can be made to directly react to re-form the reactants. Such reactions are described as (EQ1.1) a. dynamic. b. stressed. c. reversible. d. catalyzed. 2. The state of chemical equlibrium exists when (EQ1.1) a. one of more of the products is a gas or a solid. b. products of a reaction recombine to form reactants. c. concentration of reactants and products are equal. d. forward and reverse reaction are occurring at the same rate. 3. Which is…arrow_forwardQUESTION 11 Write the condensed structural formula for the following molecule H. H. C N- H. For the toolbar, press ALT+F10 (PC) or ALT+FN+F10 (Mac). B IUS Paragraph Arial 10pt A Ix x X, 次 T T ΩΘ Click Save and Submit to save and submit. Click Save All Answers to save all answers. MacBook Pro !! !!! +]arrow_forward(6) H20, H30* 1) ВН3 THF (7) 2) H2O2, OH ? (8) (CH3)2C=CH2 (CH3)2CHCH2OHarrow_forward
- Hello, I need help with my chemistry hw. I have been trying to solve this for hours, thank you.arrow_forward(7) KMNO4, NaOHarrow_forwardIf the enthalpy of C12H22O11 combustion is said to be -5.65 x 103 kJ/mol, calculate the mass of C12H22O11 needed to be burned to produce 2.6 kJ of heat. (MM of sucrose: 342.3)arrow_forward
- 1. 2. 3. 4. Н Н Н С H C Н Н Н Н H H-C C C Н H Н Н Н Н Н Н Н Н мор Н Н Hydrocarbon Reactions Н Н Н Н Н С10Н22(1) → С2Н6(9) + C7H16(l) + C(s) C Н Н C-H - Н ·H + H — Н Н C Н H с Н CH₂ + Н Н с Н C Н -H + H- H С Н Н T Н c- c- Н H Нarrow_forwardgive the IUPAC name for the diagramarrow_forwardLab 10: Enthalpy of Neutralization (7) Identify the limiting reagent and briefly explain why it is limiting. ds toad sdd sialla () Jed ofhioea sh ba Im & SO1 aew ouurbim answer wans (8) Find AHneutzn for the reaction. ardt gaieu mite bee momod asminolso ard yd bodioeda 1sod lo inuorms srlt sdaluole ) (A) S nobesuC ni batsluol Instenoo 1odsminol answer 5wans badioeds lesdl Intoi ont sisiuoin () O8.0 lo.im 0.001 bas HOM M0080 lo Jm 0.001 lo noibesnsdi yd boenslon tead Indot orl: bnit (a)arrow_forward
- Write the type of reaction that is occurring on the line provided then complete the reaction. Only include the major products and any byproducts (e.g. H2O) but no minor products. Please use either full structural diagrams or the combination method shown in the lesson. Skeletal/line diagrams will not be accepted. H3C 1. 2. 3. OH Type of Reaction: NH Type of Reaction: ა C CH3 Δ Acid + H2O Catalyst + HBr Type of Reaction: H3C 4. Type Reaction: CH2 + H2Oarrow_forwardWhat is the IUPAC name of the following compound? Multiple Choice bicyclo[2.2.2]octane bicyclo[3.3.3]octane bicyclo[2.2.2]hexane bicyclo[3.3.3]hexanearrow_forward(4) Find the AH for the reaction below, given the following reactions and subsequent AH values: CO₂(g) → C(s) + O₂(g) H₂O(1)→ H₂(g)+ ½ O₂(g) C₂H.(g) 2 C(s) + 3H₂(g) 2 CO₂(g) + 3 H₂O(1)→ C₂H(g) + ¹/₂O₂(g) 1 ΔΗ = 643 kJ ΔΗ = 190,6 kJ AH=3511.1 kJarrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY