Module 8,Is the change in entropy for the followingchemical reactions positive or negative?(Note: ASº for these species can be foundin Appendix G of the textbook: Link toAppendix G from Chemistry Atoms First e )1. 2 C2H2(g) + 5 O2(g) → 4 CO2(g) + 2H20(g)2. C2H4(g) + 3 O2(g)2 CO2(g) + 2H2O(g)3. 2 C2H6(g) + 7 O2(g) → 4 CO2(g) + 6H2O(g)4. Write out the equilibrium constant for thereaction in Question 15. Write out the equilibrium constant for thereaction in Question 26. Write out the equilibrium constant for thereaction in Question 3

Equilibrium constant is defined as ratio of concentration of product to concentration of reactant.

Module 8, Is the change in entropy for the following chemical reactions positive or negative? (Note: ASº for these species can be found in Appendix G of the textbook: Link to Appendix G from Chemistry Atoms First - ) 1.2 С2H2(g) + 5 02(g) → 4 CO2(g) + 2 H2O(g) 2. C2H4(g) + 3 O2(g) = → 2 CO2(g) + 2 H20(g)

Module 8, Is the change in entropy for the following chemical reactions positive or negative? (Note: ASº for these species can be found in Appendix G of the textbook: Link to Appendix G from Chemistry Atoms First - ) 1.2 С2H2(g) + 5 02(g) → 4 CO2(g) + 2 H2O(g) 2. C2H4(g) + 3 O2(g) = → 2 CO2(g) + 2 H20(g)

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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For each of the following pairs, predict which substancehas the higher entropy per mole at a given temperature:(a) Ar(l) or Ar(g), (b) He(g) at 3 atm pressure or He(g)at 1.5 atm pressure, (c) 1 mol of Ne(g) in 15.0 L or 1 mol ofNe(g) in 1.50 L, (d) CO2(g) or CO2(s).
Ice cubes at 0°C are poured into a glass that initially contains 150 g of liquid water at 20°C. The contents of the glass are gently stirred. After a short time, some of the ice melts, and the liquid cools to 0°C. No appreciable heat exchange occurs between matter inside the glass with matter outside the glass during this process. (a) Calculate the entropy change of the universe during the process. Use only the following data: the constant pressure heat capacity of liquid water is approximately 4.18 J/(g K) over the temper- ature range of interest. You may further presume that the density of water is constant over the temperature range. (b) If the same process were performed reversibly, how much useful work would be obtained from it? Any required heat exchange to achieve the same final state reversibly should be with matter outside the glass, which are at 20°C.
For each of the following reactions determine if the change in entropy was positive or negative:A) Water at 40°C → Water at 25°CB) 2NO2(g) → N2O4(g)C) CH3OH (l) → CH3OH (g)D) PbCl2(s) → PbCl2(aq)
Elemental carbon usually exists in one of two forms: graphite or diamond. It is generally believed that diamonds last forever. The table shows the standard enthalpy of formation (AH) and the standard molar entropy (Sº) values for diamond and graphite. Part A AGrxn= What is the standard Gibbs free energy for the transformation of diamond to graphite at 298 K? Cdiamond →Cgraphite Submit Express your answer to three significant figures and include the appropriate units. ► View Available Hint(s) O Substance Cgraphite Cdiamond μA Value AH (kJ/mol) Units 0 1.897 ? S° (J/mol. K) 5.740 2.38
What is the temperature at which the reaction below becomes spontaneous, if the standard entropies of reactants and products at 25oC are So (C(gr)) = 5.74 J/mol*K, So(H2(g)) = 130.68 J/mol*K, and So (C8H8(g)) = 345.2600J/mol*K and the heat of formation of C8H8(g)) is 147.8500 kJ/mol?C8H8(g) ↔ 8C(gr) + 4H2(g)a)661.88 Kb)707.958 Kc)the reaction is never spontaneousd)the reaction is always spontaneous
Which one of the following processes produces a decrease in the entropy of the system? precipitation of AgCl(s) from Ag*(aq) and Cl (aq) ions in solution dissolution of KCl(s) in water evaporation of Hg(1) to form Hg(g) mixing of two gases into one container O melting ice to form water
Which of the following processes will result in an increase in entropy for the system? (A) 2N2O(g) + O2(g) --> 4NO(g); (B) 2NO(g) + O2(g) --> 2NO2(g); (C) CO(g) + NO2(g) --> CO2(g) + NO(g); (D) SO3(g) + H2O(l) --> H2SO4(aq)
3. What change will increase the entropy of the system? Group of answer choices liquid to solid solid to gas gas to liquid gas to solid 2.ΔSsyst>0 for the following reaction: Group of answer choices A, 2NO (g) + O2(g) → 2NO2(g) B, HCl (g) + NH3(g) → NH4Cl (s) C, C3H8(g) + 5 O2(g) → 3CO2 (g) + 4 H2O (g) D, 2N2 (g) + 3H2(g) → 2NH3(g) E, Pb2+(aq) + 2Cl-(aq) → PbCl2 (s)
Determine the standard entropy of NO(g) given the following information: NO(g)+0,(g) → NO, (g) AS xn = -73.2 J/K Substance S° (J/mol · K) NO2(3) 240.0 O2(g) 205.0 NO(g) ? O -210.7 J/K O +210.7 J/K +108.2 J/K -108.2 J/K O +54.1 J/K