Physical Chemistry
2nd Edition
ISBN: 9781133958437
Author: Ball, David W. (david Warren), BAER, Tomas
Publisher: Wadsworth Cengage Learning,
expand_more
expand_more
format_list_bulleted
Question
Chapter 6, Problem 6.44E
Interpretation Introduction
Interpretation: The pressure at which a chamber is reduced to distill methanol is to be calculated.
Concept introduction: Vapor pressure is defined as the pressure exerted by a vapor in
The Clausius-Clapeyron equation states the relation between vapor pressure and the absolute temperature.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
In vacuum distillation, the surrounding pressure inside a chamber is lowered so the solvent boils at a lower temperature. This is useful when isolating compounds that are temperature-sensitive. To what pressure must a chamber be reduced to distill methanol (ΔvapH = 38.56 kJ/mol, TBP = 351 K) at 25.0°C?
using a calibrated solution calorimeter measured a temperature decrease of 1.10 K when 1.00 g of KNO3 was added to 74.40 g of deionized water in the calorimeter. The specific heat capacity of the solution calorimeter was found to be 4.15 J/gK. Calculate the experimental value of the molar heat of solution of KNO3, ΔHsoln. Was the dissolution of this salt exothermic or endothermic?
A
2C3H18(1) + 2502(g) =
16CO2(g) + 18H20(1)
B
CO2(g) + 2H20(g) = CO2(g) + 4H2(g)
C
3CO(g) + Fe,03(s) = 3CO2(g) + 2Fe(s)
Which of these processes energetically favors the products
A only
B and C only
А, В and C
A and C only
Chapter 6 Solutions
Physical Chemistry
Ch. 6 - Prob. 6.1ECh. 6 - Prob. 6.2ECh. 6 - Prob. 6.3ECh. 6 - Prob. 6.4ECh. 6 - Prob. 6.5ECh. 6 - Prob. 6.6ECh. 6 - Prob. 6.7ECh. 6 - Prob. 6.8ECh. 6 - 6.9. Identify and explain the sign on in equation...Ch. 6 - 6.10. Use Hess’s law to prove that .
Ch. 6 - 6.11. Calculate the amount of heat necessary to...Ch. 6 - Prob. 6.12ECh. 6 - Assume that the vapH of an evaporating liquid...Ch. 6 - 6.14. As a follow-up to the previous exercise,...Ch. 6 - Prob. 6.15ECh. 6 - 6.16. What is for isothermal conversion of liquid...Ch. 6 -
6.17. Estimate the melting point of nickel, Ni,...Ch. 6 -
6.18. Estimate the boiling point of platinum, Pt,...Ch. 6 - Prob. 6.19ECh. 6 - Prob. 6.20ECh. 6 - 6.21. What assumption is used in the integration...Ch. 6 - Prob. 6.22ECh. 6 - Sulfur, in its cyclic molecular form having the...Ch. 6 - Prob. 6.24ECh. 6 - 6.25. Phosphorus exists as several allotropes that...Ch. 6 - Prob. 6.26ECh. 6 - 6.27. What is higher for a substance: its normal...Ch. 6 - 6.28. Elemental gallium is another substance whose...Ch. 6 - Prob. 6.29ECh. 6 - Consider the sulfur solid-state phase transition...Ch. 6 - 6.31. If it takes mega bars of pressure to change...Ch. 6 - Prob. 6.32ECh. 6 - Four alcohols have the formula C4H9OH: 1-butanol,...Ch. 6 - Prob. 6.34ECh. 6 - At 20.0C, the vapor pressure of ethanol is...Ch. 6 - Prob. 6.36ECh. 6 - Prob. 6.37ECh. 6 - Ethanol has a density of 0.789g/cm3 and a vapor...Ch. 6 - Prob. 6.39ECh. 6 - Prob. 6.40ECh. 6 - Prob. 6.41ECh. 6 - 6.42. At what pressure does the boiling point of...Ch. 6 - Prob. 6.43ECh. 6 - Prob. 6.44ECh. 6 - Prob. 6.45ECh. 6 - Prob. 6.46ECh. 6 - Prob. 6.47ECh. 6 - 6.48. Explain how glaciers, huge masses of solid...Ch. 6 - Prob. 6.49ECh. 6 - Prob. 6.50ECh. 6 - Prob. 6.51ECh. 6 - Prob. 6.52ECh. 6 - Prob. 6.53ECh. 6 - Prob. 6.54ECh. 6 - Prob. 6.55ECh. 6 - Prob. 6.56ECh. 6 - Prob. 6.57ECh. 6 - Use the phase diagram of water in Figure 6.6 and...Ch. 6 - Prob. 6.59ECh. 6 - Prob. 6.60ECh. 6 - At the triple point of a substance, the vapor...Ch. 6 - Prob. 6.62ECh. 6 - Prob. 6.63ECh. 6 - Prob. 6.64ECh. 6 - Prob. 6.65ECh. 6 - Prob. 6.66ECh. 6 - The phase diagram for elemental sulfur is shown in...Ch. 6 - Consider the phase diagram of sulfur in the...Ch. 6 - Prob. 6.69ECh. 6 - Rearrange the Clausius-Clapeyron equation,...
Knowledge Booster
Similar questions
- The salt calcium chloride is soluble in water. When 1.55 g CaCl₂ is dissolved in 116.00 g water, the temperature of the solution increases from 25.00 °C to 27.47 °C. Based on this observation, calculate the dissolution enthalpy, AdissH, of CaCl₂. Assume that the specific heat capacity of the solution is 4.184 J g¹ °C-1 and that the energy transfer to the calorimeter is negligible.arrow_forwardFor the oxidation of iron to form iron(III) oxide: 4Fe(s) + 3O2(g) ⟷⟷ 2Fe2O3(s) ΔSo = –549.73 J∙K–1 at 298 K. The enthalpy of formation of Fe2O3(s) is –824.2 kJ∙mol–1. What is the standard change in Gibbs free energy for this reaction at 298 K? A)-660 kJ B)-1,485 kJ C)-988 kJ D)-1,812 kJarrow_forward200 cm3 of 1.0M HCL and 200 cm3 of 1.0M NaOH at 33.1oC were mixed in a simple calorimeter. The temperature of the calorimeter assembly increased to 39.3oC. Calculate the enthalpy of neutralization in kJ/mol. The heat capacity of the calorimeter is 101.8 J/K. Assume the specific heat of the solution to be 4.186 J/g.K and density of solution to be 1.0 g/cm3.arrow_forward
- 50.0 g of NH4Cl(s) (53.49 g mol–1) is dissolved in 200.0 mL of H2O in a constant–pressure calorimeter. The initial temperatures of both materials are the same at 20.0°C. The final temperature is 7.13°C. The density of water is 1.00 g cm–3. The specific heat of the solution is 4.184 J g–1 °C–1. What is the heat of the dissolution reaction? What is the energy change of the solution?arrow_forward50.0 g of NH4Cl(s) (53.49 g mol–1) is dissolved in 200.0 mL of H2O in a constant–pressure calorimeter. The initial temperatures of both materials are the same at 20.0°C. The final temperature is 7.13°C. The density of water is 1.00 g cm–3. The specific heat of the solution is 4.184 J g–1 °C–1. What is the energy change of the solution? –13.5 kJ –14.4 kJ +26.0 kJ What is the heat of the dissolution reaction? +13.5 kJ mol–1 –13.5 kJ mol–1 +14.4 kJ mol–1arrow_forwardAt 25 °C, the equilibrium partial pressures for the reaction 3 A(g) + 2 B(g) = C(g) + 2 D(g) were found to be PA = 4.25 atm, Pg = 5.05 atm, Pc = 4.13 atm, and Pp 4.94 atm. %3D What is the standard change in Gibbs free energy of this reaction at 25 °C? kJ molarrow_forward
- Enter a balanced equation for the complete combustion of liquid C3 H60. Express your answer as a chemical equation. Identify all of the phases in your answer. ΑΣΦ ? C, H, O(1) + O, (g)→CO, (g)+H, O(g) A chemical reaction does not occur for this question.arrow_forward4.00 g NaOH(s) (39.996 g mol–1) dissolves in 100.0 g of water in a constant–pressure calorimeter. The initial temperatures of both materials are the same at 20.0°C. The density of the solution is 1.00 g cm–3. The heat of dissolution is –44.51 kJ mol–1. The specific heat of the solution is 4.184 J g–1 °C–1. The specific heat of the calorimeter is 100 J °C–1. What is the final temperature of the solution? 30.23°C 25.94°C 28.32°C What is the energy lost to the calorimeter? 579 J 832 J 721 Jarrow_forwardA student using a calibrated solution calorimeter measured a temperature decrease of 1.10 K when 1.00 g of KNO3 was added to 74.40 g of deionized water in the calorimeter. The specific heat capacity of the solution calorimeter was found to be 4.15 J/gK. Calculate the experimental value of the molar heat of solution of KNO3, ΔH soln. Was the dissolution of this salt exothermic or endothermic?arrow_forward
- A 0.100-L solution is made by dissolving 0.441 g of CaCl21s2 in water. The enthalpy of solution for CaCl2 is ∆H = -81.3 kJ>mol. If the final temperature of the solution is 27 °C, what was its initial temperature? (Assume that the density of the solution is 1.00 g>mL, that its specific heat is 4.18 J>g@K, and that the solution loses no heat to its surroundings.)arrow_forwardDissolving 3.0 g of CaCl2(s) in 150.0 g of water in a calorimeter at 22.4 °C causes the temperature to rise to 25.8 °C. What is the change in enthalpy for the dissolution of CaCl2 in kJ/mol? Assume the specific heat of the solution is 4.184 J g1 °C. a. Calculate the heat of the solution from gsoln = msoln Cs.soln ATsoln. (Hint: Pay attention to the mass in the equation: It is the mass of the solution.)arrow_forwardPotassium nitrate, KNO3, has a molar mass of 101.1 g/mol. In a constant-pressure calorimeter, 23.4 g of KNO3 is dissolved in 259 g of water at 23.00 °C. H₂O KNO3(s) →→→ K+ (aq) + NO3(aq) The temperature of the resulting solution decreases to 21.20 °C. Assume that the resulting solution has the same specific heat as water, 4.184 J/(g. °C), and that there is negligible heat loss to the surroundings. How much heat was released by the solution? 9soln = kJ What is the enthalpy of the reaction? AHrxn= kJ/molarrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning