CHEMISTRY-MOD.MASTERING (18W)
8th Edition
ISBN: 9780136780922
Author: Robinson
Publisher: PEARSON
expand_more
expand_more
format_list_bulleted
Textbook Question
Chapter 9, Problem 9.138SP
Ethyl alcohol has
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
Calculate ΔH for the following reaction: CH4 (g) + O2 (g) ⇌ CO2 (g) + H2O (l) Compound ΔH CH4 (g) -74.8 kJ/mol H2O (l) -285.8 kJ/mol CO2 (g) -393.5 kJ/mo
A compound melts at -55 ∘C and has a heat of fusion of 21 kJ/mol. Calculate its change in entropy when it melts.
ΔS in (J/mol K)
Please explain if you can
The Δ?vapΔHvap of a certain compound is 42.97 kJ·mol−142.97 kJ·mol−1 and its Δ?vapΔSvap is 76.35 J·mol−1·K−1.76.35 J·mol−1·K−1.
What is the boiling point of this compound?
Chapter 9 Solutions
CHEMISTRY-MOD.MASTERING (18W)
Ch. 9 - Prob. 9.1PCh. 9 - Conceptual APPLY 9.2 How much work is done in...Ch. 9 - PRACTICE 9.3 The reaction between hydrogen and...Ch. 9 - Conceptual APPLY 9.4 The following reaction has E...Ch. 9 - Use the following thermo chemical equation to...Ch. 9 - APPLY 9.6 Approximately, 1.8106 kJ of energy is...Ch. 9 - Classify the following reaction as end o- or ex...Ch. 9 - APPLY 9.8 Instant hot packs and cold packs contain...Ch. 9 - PRACTICE 9.9 What is the specific heat of lead in...Ch. 9 - APPLY 9.10 Calculate the heat capacity (C) of a...
Ch. 9 - PRACTICE 9.11 When 25.0 mL of 1.0 M H2SO4 is added...Ch. 9 - Prob. 9.12ACh. 9 - When 1.00 g of toluene, C7H8, is burned in a bomb...Ch. 9 - Prob. 9.14PCh. 9 - Water gas is the name for the mixture of CO and H2...Ch. 9 - Prob. 9.16ACh. 9 - Prob. 9.17PCh. 9 - Prob. 9.18ACh. 9 - Use the data in Table 9.3 to calculate an...Ch. 9 - Benzene ( C6H6 ) has two resonance structures,...Ch. 9 - Prob. 9.21PCh. 9 - Prob. 9.22ACh. 9 - Prob. 9.23PCh. 9 - Prob. 9.24ACh. 9 - Prob. 9.25PCh. 9 - Prob. 9.26ACh. 9 - Prob. 9.27PCh. 9 - Prob. 9.28PCh. 9 - Prob. 9.29PCh. 9 - Prob. 9.30PCh. 9 - Prob. 9.31PCh. 9 - Prob. 9.32PCh. 9 - PROBLEM 9.33 A 12.0 gallon hold 39.9 kg of...Ch. 9 - A piece of dry ice (solid CO2) is placed inside a...Ch. 9 - Imagine a reaction that results in a change in...Ch. 9 - 9.32 Redraw the following diagram to represent the...Ch. 9 - 9.33 A reaction is carried out in a cylinder...Ch. 9 - Prob. 9.38CPCh. 9 - Prob. 9.39CPCh. 9 - Prob. 9.40CPCh. 9 - Prob. 9.41CPCh. 9 - Prob. 9.42CPCh. 9 - Prob. 9.43CPCh. 9 - What is the difference between heat and...Ch. 9 - What is internal energy?Ch. 9 - Prob. 9.46SPCh. 9 - Prob. 9.47SPCh. 9 - Which of the following are state functions, and...Ch. 9 - Prob. 9.49SPCh. 9 - Calculate the work done in joules by a chemical...Ch. 9 - The addition of H2 to C=C double bonds is an...Ch. 9 - Prob. 9.52SPCh. 9 - Prob. 9.53SPCh. 9 - 9.50 A reaction inside a cylindrical container...Ch. 9 - At a constant pressure of 0.905 atm, a chemical...Ch. 9 - RANWhen a sample of a hydrocarbon fuel is ignited...Ch. 9 - Used in welding metals, the reaction of acetylene...Ch. 9 - What is the difference between the internal energy...Ch. 9 - Prob. 9.59SPCh. 9 - The explosion of 2.00 mol of solid trinitrotoluene...Ch. 9 - The reaction between hydrogen and oxygen to yield...Ch. 9 - The enthalpy change for the reaction of 50.0 mL of...Ch. 9 - Assume that a particular reaction evolves 244 kJ...Ch. 9 - What is the enthalpy change ( H ) for a reaction...Ch. 9 - Prob. 9.65SPCh. 9 - Indicate the direction of heat transfer between...Ch. 9 - Indicate the direction of heat transfer between...Ch. 9 - The familiar "ether" used as an anesthetic agent...Ch. 9 - How much energy in kilojoules is required to...Ch. 9 - Aluminum metal reacts with chlorine with a...Ch. 9 - How much heat in kilojoules is evolved or absorbed...Ch. 9 - How much heat in kilojoules is evolved or absorbed...Ch. 9 - Nitromethane sometimes used as a fuel in drag...Ch. 9 - Prob. 9.74SPCh. 9 - How much heat in kilojoules is evolved or absorbed...Ch. 9 - Prob. 9.76SPCh. 9 - Prob. 9.77SPCh. 9 - Sodium metal is sometimes used as a cooling agent...Ch. 9 - Prob. 9.79SPCh. 9 - Assuming that Coca-Cola has the same specific heat...Ch. 9 - Calculate the amount of heat required to raise the...Ch. 9 - Instant cold packs used to treat athletic injuries...Ch. 9 - Instant hot packs contain a solid and a pouch of...Ch. 9 - When 1.045 g of CaO is added to 50.0 mL of water...Ch. 9 - When a solution containing 8.00 g of NaOH in 50.0...Ch. 9 - When 0.187 g of benzene, C6H6 , is burned in a...Ch. 9 - When 0.500 g of ethanol, C2H6O, is burned in a...Ch. 9 - When 1.50 g of magnesium metal is allowed to react...Ch. 9 - A 110.0 g piece of molybdenum metal is heated to...Ch. 9 - Citric acid has three dissociable hydrogens. When...Ch. 9 - Prob. 9.91SPCh. 9 - Prob. 9.92SPCh. 9 - Prob. 9.93SPCh. 9 - The industrial degreasing solvent methylene...Ch. 9 - Hess's law can be used to calculate reaction...Ch. 9 - Find H in kilojoules for the reaction of nitric...Ch. 9 - Set up a Hess's law cycle, and use the following...Ch. 9 - Prob. 9.98SPCh. 9 - Prob. 9.99SPCh. 9 - What phase of matter is associated with the...Ch. 9 - What is the phase of the standard states of the...Ch. 9 - Write balanced equations for the formation of the...Ch. 9 - Prob. 9.103SPCh. 9 - Prob. 9.104SPCh. 9 - Prob. 9.105SPCh. 9 - The standard enthalpy change for the reaction of...Ch. 9 - Prob. 9.107SPCh. 9 - Styrene ( C8H8 ), the precursor of polystyrene...Ch. 9 - Prob. 9.109SPCh. 9 - Prob. 9.110SPCh. 9 - Prob. 9.111SPCh. 9 - Prob. 9.112SPCh. 9 - Prob. 9.113SPCh. 9 - Prob. 9.114SPCh. 9 - Prob. 9.115SPCh. 9 - Prob. 9.116SPCh. 9 - Isooctane, C8H18, is the component of gasoline...Ch. 9 - Calculate an approximate heat of combustion for...Ch. 9 - Use the data in Table 9.3 to calculate an...Ch. 9 - Use the average bond dissociation energies in...Ch. 9 - Use the bond dissociation energies in Table 9.3 to...Ch. 9 - Prob. 9.122SPCh. 9 - Prob. 9.123SPCh. 9 - Prob. 9.124SPCh. 9 - Prob. 9.125SPCh. 9 - Tell whether the entropy changes for the following...Ch. 9 - Prob. 9.127SPCh. 9 - Prob. 9.128SPCh. 9 - Prob. 9.129SPCh. 9 - Prob. 9.130SPCh. 9 - Prob. 9.131SPCh. 9 - Tell whether reactions with the following values...Ch. 9 - Tell whether reactions with the following values...Ch. 9 - Suppose that a reaction has H=33kJ and S=58J/K. At...Ch. 9 - Suppose that a reaction has H=+41kJ and S=27J/K....Ch. 9 - Which of the reactions (a)-(d) in Problem 9.132...Ch. 9 - Vinyl chloride (H2C=CHCI), the starting material...Ch. 9 - Ethyl alcohol has Hfusion=5.02kJ/mol and melts at...Ch. 9 - Chloroform has Hvaporization=29.2kJ/mol and boils...Ch. 9 - The boiling point of a substance is defined as the...Ch. 9 - What is the melting point of benzene in kelvin if...Ch. 9 - Prob. 9.142SPCh. 9 - Methanol (CH3OH) is made industrially in two steps...Ch. 9 - Ethyl chloride ( C2H5CI ), a substance used as a...Ch. 9 - Prob. 9.145MPCh. 9 - For a process to be spontaneous, the total entropy...Ch. 9 - Prob. 9.147MPCh. 9 - Prob. 9.148MPCh. 9 - Prob. 9.149MPCh. 9 - Prob. 9.150MPCh. 9 - Phosgene, COCI2(g), is a toxic gas used as an...Ch. 9 - Prob. 9.152MPCh. 9 - Write a balanced equation for the reaction of...Ch. 9 - Hydrazine, a component of rocket fuel, undergoes...Ch. 9 - Prob. 9.155MP
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
- Cl(g) ΔH°f, = +121.3 kJ mol–1 Cl–(aq) ΔH°f, = –167.2 kJ mol–1 HCl(g) ΔH°f, = –92.3 kJ mol–1 HCl(aq) ΔH°f, = –167.2 kJ mol–1 Cl2(g) ΔH°f, = 0 kJ mol–1 H2O(l) ΔH°f, = –286 kJ mol–1 ClO2(g) ΔH°f, = +102.5 kJ mol–1 Cl2O(g) ΔH°f, = +80.3 kJ mol–1 O(g) ΔH°f, =+249.0 kJ mol–1 H(g) ΔH°f, =+218.2 kJ mol–1 Which material is most 'stable' at 298 K? Question 1 options: Cl2(g) Cl–(aq) Cl(g)arrow_forwardThe enthalpy of fusion (∆Hfusion) for the melting of water is 6.02 kJ/mol. This phase change from solid to liquid water is an example of a process that can be treated as if it were reversible. Ice melts at 0°C. What is the entropy change (in J/K) associated with the melting of one mole of ice? (One decimal place)arrow_forwardFrom the following information, determine ΔH°f of malonic acid, CH2(COOH)2(s).CH2(COOH)2(s) + 2O2(g) → 3CO2(g) + 2H2O(l); ΔH° = –861.0 kJSubstance ΔH°f (kJ/mol)CO2(g) –393.5H2O(l) –285.8a. 2613 kJb. 891.1 kJc. −1540.3 kJd. −2613.1 kJe. −891.1 kJarrow_forward
- What is the ΔH°vap of a liquid that has a vapor pressure of 624 torr at 85.2°C and a boiling point of 93.2°C at 1 atm?arrow_forwardFrom the following enthalpies of reaction: H2 (g) +F2 (g) → 2HF (g) ∆H = −537 kJ C (s) + 2F2 (g) →CF4 (g) ∆H = −680 kJ 2C (s) + 2H2 (g) → C2H4 (g) ∆H = +52.3 kJ calculate ∆H for the reaction of ethylene with F2: C2H4 (g) + 6F2 (g) → 2CF4 (g) + 4HF (g)arrow_forward3- Diethyl ether (CH3CH2OCH2CH3) was one of the first chemicals used as an anesthetic. At 34.6°C, diethyl ether has a vapor pressure of 760. torr, and at 17.9°C, it has a vapor pressure of 400 torr. What is the ΔH of vaporization for diethyl ether?arrow_forward
- Toluene has a normal boiling point of 101.4 ℃ and its ΔHvap is 33.8 kJ/mol. Calculate the molar entropy of vaporization, ΔSvap, in J/mol⋅K. Report your answer to THREE significant figures.arrow_forwardPlease use the following reactions and ∆H values to calculate the theoretical ∆Hsoln for NaCl. NaCl(s) à Na+(g) + Cl–(g) ∆H = + 787.9 kJ/mol Na+(g) à Na+(aq) ∆H = – 453.0 kJ/mol Cl– (g) à Cl– (aq) ∆H = – 331.0 kJ/molarrow_forwardCalculate ΔrH° for the combustion of methane gas, CH4 : CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g) using standard molar enthalpies of formation: molecule ΔfH° (kJ/mol) CH4(g) -74.6 CO2(g) -393.5 H2O( g) -241.8 a) -802.5 kJ b) -495.2 kJ c) +802.5 kJ d) -1460.3 kJ e) -1828.5 kJ Group of answer choicesarrow_forward
- Which value corresponds to a larger Keq: ΔGo = −8 kJ/mol or ΔGo = 20kJ/mol?arrow_forwardUsing the equations N₂ (g) + 3 H₂ (g) → 2 NH₃ (g) ∆H° = -91.8 kJ/mol C(s) + 2 H₂ (g) → CH₄ (g) ∆H° = -74.9 kJ/mol H₂ (g) + 2 C(s) + N₂ (g) → 2 HCN (g) ∆H° = 270.3 kJ/mol Determine the enthalpy for the reaction CH₄ (g) + NH₃ (g) → HCN (g) + 3 H₂ (g).arrow_forwardFor a particular reaction at 148.1 °C, Δ?=−1428.51 kJ, and Δ?=393.69 J/K . Calculate Δ? for this reaction at −62.8 °C. Δ?=Δ?−?Δ? thus, Δ?=Δ?+?Δ? Assume that enthalpy and entropy will not change between the two temperatures. Use these values with the new temperature to determine the new free energy value using the first equation.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry for Today: General, Organic, and Bioche...ChemistryISBN:9781305960060Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. HansenPublisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Chemistry for Today: General, Organic, and Bioche...
Chemistry
ISBN:9781305960060
Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. Hansen
Publisher:Cengage Learning
The Laws of Thermodynamics, Entropy, and Gibbs Free Energy; Author: Professor Dave Explains;https://www.youtube.com/watch?v=8N1BxHgsoOw;License: Standard YouTube License, CC-BY