The heat of vaporization AH, of heptane (C₂H₁6) is 31.2 kJ/mol. Calculate the change in entropy AS when 26. g of heptane condenses at 98.4 °C. Be sure your answer contains a unit symbol and the correct number of significant digits. 0 ☐ μ x10 ロ・ロ 00

The heat of vaporization AH, of heptane (C₂H₁6) is 31.2 kJ/mol. Calculate the change in entropy AS when 26. g of heptane condenses at 98.4 °C. Be sure your answer contains a unit symbol and the correct number of significant digits. 0 ☐ μ x10 ロ・ロ 00

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

3- 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?
3 If we measure the heat change (q) of everything in a system except the calorimeter, we can use the first law of thermodynamics (∆Euniverse = 0) to calculate the heat change of the calorimeter (qcal). In this reaction, we combine 5.75 g of 67.4 ºC water with 6.67 g of 19 ºC water in a calorimeter. Since some of the heat is absorbed by the calorimeter, the final temperature of the water is 25.4ºC. Since the hot and cold water are combined, the final temp of the water is the final temp for the hot water and the cold water. Calculate the heat change of the calorimeter in J. Remember that all of the heat changes must add up to zero so you can calculate the heat change of the hot water (qhotwater) and the heat change of the cold water (qcoldwater) using for each where Cs = 4.186 J/gºC. The first law of thermodynamics tells us that all of these changes sum up to zero so Enter your answer to one decimal place (tenths)
Phthalates used as plasticizers in rubber and plastic products are believed to act as hormone mimics in humans. The value of ΔHcomb for dimethylphthalate (C10H10O4) is –4685 kJ/mol. Assume 0.910 g of dimethylphthalate is combusted in a calorimeter whose heat capacity (Ccalorimeter) is 7.40 kJ/°C at 22.0 °C. What is the final temperature of the calorimeter? °C
A quantity of 2.00×102 mL of 0.786 M HCl is mixed with 2.00×102 mL of 0.393 M Ba(OH)2 in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of the HCl and Ba(OH)2 solutions is the same at 20.76°C. For the process below, the heat of neutralization is −56.2 kJ/mol. What is the final temperature of the mixed solutions? H+(aq) + OH−(aq)→H2O(l) _____°C
A system does 516516 kJ of work and loses 236236 kJ of heat to the surroundings. What is the change in internal energy, Δ?Δ�, of the system? Note that internal energy is symbolized as Δ?Δ� in some sources.
A bomb calorimeter has a heat capacity of 4.66 kJ/°C. When 1.772 g of glucose, C6H₁2O6(s), is combusted in the bomb calorimeter, the temperature of the calorimeter and its contents increased from 22.32 °C to 28.24 °C. Calculate the change in internal energy, AU, for the combustion of 1.772 g of glucose in the bomb calorimeter. AU = -716.36 kJ
Phthalates used as plasticizers in rubber and plastic products are believed to act as hormone mimics in humans. The value of ΔHcomb for dimethylphthalate (C10H10O4) is –4685 kJ/mol. Assume 1.16 g of dimethylphthalate is combusted in a calorimeter whose heat capacity (Ccalorimeter) is 7.85 kJ/°C at 20.0 °C. What is the final temperature of the calorimeter?
55. Does the standard enthalpy of formation of H2O(g) differ from ΔH° for the reaction 2H2(g)+O2(g)⟶2H2O(g)?
If a system has 5.00×102 kcal5.00×102 kcal of work done to it, and releases 5.00×102 kJ5.00×102 kJ of heat into its surroundings, what is the change in internal energy (Δ? or Δ?)(ΔE or ΔU) of the system?
A 0.588 g sample of liquid C5H12 was combusted using excess oxygen gas inside a bomb calorimeter, with the products being carbon dioxide gas and liquid water. The calorimeter's heat capacity is 4.706 kJ °C-1. If the temperature inside the calorimeter increased from 25.0 °C to 29.9 °C, determine ΔrU for this reaction in kJ mol-1 (with respect to C5H12). Do not worry about how realistic the final answer is. Express answer in 2 significant figures.
what is the value of ΔHrxn if the reaction below is reversed? In other words, PCl5 becomes the reactant. Report your answer in kJ to 1 decimal place. PCl3(g) + Cl2(g) → PCl5(g); ΔHrxn = 618.7 kJ
Phthalates used as plasticizers in rubber and plastic products are believed to act as hormone mimics in humans. The value of ΔHcomb for dimethylphthalate (C10H10O4) is –4685 kJ/mol. Assume 1.01 g of dimethylphthalate is combusted in a calorimeter whose heat capacity (Ccalorimeter) is 6.95 kJ/°C at 20.5 °C. What is the final temperature of the calorimeter?