a) Formulate the second law of thermodynamics.b) Consider the statements below. Answer them and give brief explanations.a. An explosive (e.g. C7H5N3O6) reacts with oxygen, the result is CO2 (g),H2O (g) and N2 (g). Is there an increase or decrease of Entropy after thereaction occurred?b. Colloquially, people say that during the cold months of the year, the “cold”is creeping into the warmer house. Is this statement true considering the2nd law?

Step 1: Step 2: Step 3: Step 4:

Answered: a) Formulate the second law of…

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...

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State the 3rd law of thermodynamics. How is it interpreted in microscopic thermodynamic sense?
eq M M IS M ots M M M # 3 E D Consider the reaction 2H₂O(l) 2H₂(g) + O₂(g) The standard free energy change for this reaction is 474.2 kJ. The free energy change when 1.88 moles of H₂O(1) react at standard condition is kJ. 20 C What is the maximum amount of useful work that the reaction of 1.88 moles of H₂O(l) is capable of producing in the surroundings under standard conditions? If no work can be done, enter none. kJ Submit Answer $ 4 R F > % 5 T [References] Use the References to access important values if needed for this question. Retry Entire Group 9 more group attempts remaining G Cengage Learning Cengage Technical Support 6 B MacBook Pro Y Topics] H & 7 N U J ▶II * 00 8 M I ( 9 K. O < 96 ) L P V t Previous Email Instructor Save and Exit { + 11 [ Next ? } 1 dele
5. Note: Please don't write on a paper. I can't understand handwrittens.
The heat of vaporization AH, of heptane (C-H₁6) is 31.2 kJ/mol. Calculate the change in entropy AS when 736. g of heptane condenses at 98.4 °C. Be sure your answer contains a unit symbol. Round your answer to 3 significant digits. x10 ロ・ロ X H ■
1. Please consider 0.15 gm of Constantan (a Cu/Ni alloy widely used in thermocouples, c = 390 J/•K-kg) that cooled through exposure to the laboratory atmosphere (T 22 •C) from 620 C to 20 C. a. Please determine the change in entropy of the Constantan (in J/ K- kg). b. Please determine the change in entropy of the laboratory atmosphere (in J/ K-kg). c. Please determine the change in entropy of the universe (in J/ K-kg). %3D
Draw the product of nucleophile substitution , and determine the likely mechanism ( SN1 or SN2
Given the following reaction and its enthalpy change, and the sign of the entropy change that you get using what you know of trends in entropy, S, when is this reaction spontaneous? 2 ClO2 (g) + 2 TiCl4 (l) → 2 TiO2 (s) + 5 Cl2 (g) Delta H = – 343.8 kJ Select one: a. This reaction is spontaneous at lower temperatures, but not at higher temperatures. b. This reaction is spontaneous at higher temperatures, but not at lower temperatures. c. This reaction is never spontaneous. d. none of these e. This reaction is spontaneous at all temperatures.
8. You have discovered a new polymer. A monomer is shown below. To better understand its behavior you calculate its theoretical entropy. With careful measurements you find that it can be in 3 positions around the 1st bond in the chain, 2 around the 2nd bond, 1 around the 3rd bond and 3 around the 4th bond. Further, the ring can be in 4 different positions. What is the entropy in units of KB?
Enthalpy and Gibb's Free Energy Chemical energy is released or absorbed from reactions in various forms. The most easily measurable form of energy comes in the form of heat, or enthalpy. The enthalpy of a reaction can be calculated from the heats of formation of the substances involved in the reaction: AHxn = AH₂ (products) - AH (reactants) Entropy change, AS°, is a measure of the number of energetically equivalent microstates introduced into the system during the reaction. The degree of spontaneity of a reaction is represented by the Gibbs free energy, AGO. The Gibbs free energy depends on both the enthalpy and entropy changes that take place during the reaction: AG=AH° - TAS° where T is standard temperature, 298 K. ▼ Part A Calculate the standard enthalpy change for the reaction where the heats of formation are given in the following table: ΔΗ Substance (kJ/mol) A B C D -241 -407 191 -501 Express your answer in kilojoules. ► View Available Hint(s) {—| ΑΣΦ AHixn= 2A+B=2C+2D ? kJ…

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