5. a. Calculate the standard entropy change for the following reaction: 2 SO3 (9) → 2 SO2 (g) + O2 (g) Calculate the entropy change which occurs when 36.0 g of H₂O vapor at 110 °C is cooled, condensed to a liquid at 100 °C, the liquid is converted to a solid at 0 °C, and the solid is then cooled to -10 °C. For water: b. Cp (vapor) Cp (liquid) Cp (solid) AHfusion AHvaporization 33.6 J/mol K 75.2 J/mol-K 37.6 J/mol K 6.019 kJ/mol 40.7 kJ/mol (6)

5. a. Calculate the standard entropy change for the following reaction: 2 SO3 (9) → 2 SO2 (g) + O2 (g) Calculate the entropy change which occurs when 36.0 g of H₂O vapor at 110 °C is cooled, condensed to a liquid at 100 °C, the liquid is converted to a solid at 0 °C, and the solid is then cooled to -10 °C. For water: b. Cp (vapor) Cp (liquid) Cp (solid) AHfusion AHvaporization 33.6 J/mol K 75.2 J/mol-K 37.6 J/mol K 6.019 kJ/mol 40.7 kJ/mol (6)

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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Calculate AG° (in kJ) for the reaction below at 36°C. 2 SO2(g) + O2(g) 2 SO3(g) Enter your result as a number without units. You may use standard or exponential notation. A quantity 543.1 kJ would be entered as 5.431E2. Substance ΔΗ S° (kJ/mol) (J/mol-K) SO2 (g) -288 241.7 02(g) 198 SO3(g) -389 262.2
Standard molar entropies, S°, in J/K•mol, are given below each reactant and product in the reaction shown below. The standard entropy of reaction, AS°, for this reaction is J. CH4(g) + 2 O2(g) CO2(g) + 2 H2O() 213.6 186.2 _205.0 69.9 Express your answer using four significant figures.
2H2O(g) ----> 2H2(g) + O2(g) The reaction above is only spontaneous at temperatures above 2000K. Is the reaction endothermic (+ΔH) or exothermic (-ΔH)?
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
What is A-G° in unit of kJ at 298 K for the following reaction? Zn(s) + H20(g) ZnO(s) + H2(g) Substance AH (kJ/mol-rxn) at 298 K S (J/K mol-rxn) at 298 K Zn(s) 46 H20(g) -241.8 188.7 ZnO(s) H2g) -337.1 42.6 130.6 Please keep your answer to one decimal place.
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.
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
Use the data shown below, to calculate AH°rxn and AS°rxn at 25°C for the following reaction: 3 H₂(g) + Fe₂O₂(s) → 2 Fe(s) + 3 H₂O(g) What is the value of AGᵒrxn at 25°C? Substance: H₂(g) AHof (kJ.mol-¹) 0 So (J.K-¹.mol-¹) 130.7 Fe₂O3(s) -824.2 87.40 Fe(s) 0 27.28 H₂O(g) -241.8 188.8
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…