Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Related questions
Question
Transcribed Image Text:Ammonium dichromate is sometimes known as
Vesuvian Fire, because of its use in demonstrations
of tabletop "volcanoes". Using the given data,
calculate the heat of reaction for the following
reaction:
(NH4)2Cr207(s) → Cr2O3(s) + N2(g) +4H2O(g)
AH,°
(kJ
mol")
s°
U mol-
K-')
(k)
mol')
Species
Nitrogen
N;(g)
N(g)
NH,(g)
191.5
472.704
153.19
455.579
-46.11
192.3
-16.5
NH,(aq)
NH,*(aq)
-80.29
111.3
-26.50
-132.51
113.4
-79.31
N,H(€)
50.63
121.2
149.2
(NH,);AsO,(aq)
NH,Br(s)
-1268
-270.83
113
-175.2
NH,C(s)
NH,Cl(aq)
NH,HCO,(s)
-314.4
94.6
-201.5
- 300.2
-847
12.1
-666
- 201.4
NH,I(s)
NH,NO,(s)
117
-113
- 365.6
151.1
-184.0
(NH,);SO,(s)
-1180.85
220.1
-901.67
NF,(g)
-125
260.6
-83.3
210.7
86.57
NO(g)
NO:(g)
90.25
33.2
240.0
51.30
N,O(g)
82.05
219.7
104.2
83.72
321.28
139.46
(3)'O°N
304.2
N,O,(g)
9.16
97.82
N;O;(g)
N,O;(s)
11
356
115
-43.1
178
114
Transcribed Image Text:NO(g)
NO;(g)
90.25
210.7
86.57
33.2
240.0
51.30
N,O(g)
N;O,(g)
82.05
219.7
104.2
83.72
321.28
139.46
(S)*O°N_
(3)*O°N
9.16
304.2
97.82
11
356
115
N,O;(s)
-43.1
178
114
NOCI(g)
HNO,(€)
HNO,(g)
52.59
264
66,36
-174.1
155.6
-80.79
-135.1
266.2
-74.77
HNO, (aq)
-206.6
146
-110.5
Hydrogen
H(g)
218.0
114.6
203.3
H;(g)
130.6
H,O(€)
-285.8
69.91
-237.2
H,O(g)
-241.8
188.7
-228.6
H;O;()
-187.8
109.6
-120.4
Cbromium
Cr(s)
23.8
Cr,O;(s)
Cr,Cl;(s)
-1139.7
81.2
- 1058.1
-556.5
123.0
-486.1
(NH,) ¿Cr,O;(s)
-1807
A
-299.9 kJ/mol
В
3,913.9 kJ/mol
299.9 kJ/mol
D
-3,913.9 kJ/mol
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by stepSolved in 2 steps with 2 images
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- In the recovery of iron from iron ore, the reduction of the ore is actually accomplished by reactions involving carbon monoxide. Use the following thermochemical equations, Fe,O3(s) + 3CO(g)→ 2Fe(s) + 3CO,(g) AH° = -28 kJ 3Fe,O3() + CO(g) 2Fe3O4() + Co,(g) AH = -59 kJ FezO,(s) + CO(g)→ 3FCO(s) + CO,(g) AH° = +38 kJ The AH° for the reaction FeO() + CO(g) Fe(s) + CO2(g) is -16.8 kJ. Use this data and the data in the following table to calculate the value of AH° for FeO. Standard Enthalpies of Formation of Typical Substances AH; (KI mol-1) AH; (kl mol-1) 90.37 Substance Substance AH (KI mol-1) Substance AH; (KI mol-1) Substance Ag(s) AgBr() H,O,(/) -187.6 CH.(g) -84.667 NO(g) - 100.4 - 127.0 HBr(g) -36 CH,OH(/) -277.63 NO,(g) 33.8 AgCI(s) HCIg) -92.30 Ca) 81.57 Al() HI(g) 26.6 CaBr,() -682.8 9.67 Al,0,) -1669.8 HNO,() -173.2 CaCO() - 1207 11 CG) (graphite) H,SO,() -811.32 CaCl,() -795.0 Na(s) CO(g) HC,H,0,) NaHCO,) Na,CO,() -110.5 -487.0 CaO() -635.5 -947.7 CO.(g) -393.5 Hg(/) Ca(OH),()…arrow_forwardThe oxidation of glucose, C6H12O6(s), is described by the following thermochemical equation:C6H12O6(s) + 6 O2(g) → 6 CO2(g) + 6 H2O(l) ΔH = -2772 kJHow much heat, in kilojoules, can be produced by the oxidation of 3.56 g of fuel C6H12O6?Molar mass of C6H12O6 = 180.156 g/molarrow_forwardWhen 0.560g of NaF(s) reacts with excess F2(g) to form NaF(s), 13.8kJ of heat is evolved at standard-state conditions. What is the standard enthalpy of foundation (H*f) of NaF(s)?arrow_forward
- Glucose, C6H12O6(s), (ΔHr° = -1275.2kJ/mol ) is converted to ethyl alcohol, C2H5OH(l), and carbon dioxide in the fermentation of grape juice. What quantity of heat is liberated when 750.0 mL of wine containing 12.0% ethyl alcohol by volume (d = 0.789g/cm3 ) are produced by the fermentation of grapejuice?arrow_forwardCalculate the standard enthalpy of formation for C3H6O (l) from its combustion using the following data: Enthalpy of this combustion is -1793 kJ ( you must write a balanced reaction first).arrow_forward2 N2(g) + O2(g) 2 N2O(g) G° = 203.1 kJ and S° = -148.5 J/K at 262 K and 1 atm. This reaction is (reactant, product) fill in the blank 1 favored under standard conditions at 262 K. The standard enthalpy change for the reaction of 2.07 moles of N2(g) at this temperature would be kJ.arrow_forward
- In the following reaction, how many moles of CH3OH are required to give off 3791 kJ of heat? 2 CH,OH (I) + 3 02 (g) → 2 CO, (g) + 4 H,0(g) AH° = -1280. kJarrow_forward(b) The standard enthalpy change for the following reaction is -697 kJ at 298 K.2 Zn(s) + O2(g)2 ZnO(s)What is the standard heat of formation of ZnO(s)arrow_forwardA food product containing 82% moisture content is being frozen. Predict the specific heat of the product at -8 ° C when 82% of the air is frozen. The specific heat of the dry product is 2.5 kJ / (kg ° C). It is assumed that the specific heat of water at -10 ° C is the same as that of water at 0 ° C, and that the specific heat of ice follows the function Cp ice = 0.0062 T frozen + 2.0649. Cp of frozen product = answer J / kg ° C.arrow_forward
- A cylinder contains a mixture of gases under constant atmospheric pressure. The gases undergo a chemical reaction. Upon reacting, the gases absorb 835 J835 J of heat from the surroundings and the surroundings do 0.497 kJ0.497 kJ of ??PV work on the gases. What is the value of Δ?ΔH in joules for this process?arrow_forward8. The oxidation of the sugar glucose, C6H1206 is described by the following equation: C6 H12 06 (s) + 602 (g) → 6CO2 (g) + 6H2 O(1) AH=-2816 kJ The metabolism of glucose gives the same products, although the glucose reacts with oxygen in a series of steps in the body. (a) How much heat in kilojoules can be produced by the metabolism of 1.0 g of glucose? (b) How many Calories can be produced by the metabolism of 1.0 g of glucose? Dags 1 of 514 words 170arrow_forward
arrow_back_ios
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
ChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill Education
Principles 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 Education
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Elementary 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