Silver oxide decomposes based on the reaction: 2 Ag20 (s) → 4 Ag (s) + 02 (g) The standard molar enthalpy of formation AH°F and the standard molar entropy s°m of the reacting species of this reaction are given below. Note AH°fand s°m are temperature independent. Ag20 (s) Ag (s) 02 (8) AH°F (k/mol) -31.05 s°m U/K-mol) 121.34 42.55 205 Which of the following statements is correct regarding this reaction at different temperatures? O a. At 25 °C, the equilibrium constant of this reaction is Kp >1 (pressure based equilibrium constant). O b. At 25 °C, the entropy change of surroundings AS(surroundings) > 0. O. The equilibrium constant of this reaction increases as temperature is increased. d. The reaction is non-spontaneous at all temperatures. e. None of the above

Silver oxide decomposes based on the reaction: 2 Ag20 (s) → 4 Ag (s) + 02 (g) The standard molar enthalpy of formation AH°F and the standard molar entropy s°m of the reacting species of this reaction are given below. Note AH°fand s°m are temperature independent. Ag20 (s) Ag (s) 02 (8) AH°F (k/mol) -31.05 s°m U/K-mol) 121.34 42.55 205 Which of the following statements is correct regarding this reaction at different temperatures? O a. At 25 °C, the equilibrium constant of this reaction is Kp >1 (pressure based equilibrium constant). O b. At 25 °C, the entropy change of surroundings AS(surroundings) > 0. O. The equilibrium constant of this reaction increases as temperature is increased. d. The reaction is non-spontaneous at all temperatures. e. None of the above

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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All spontaneous processes are characterized by an increase in the total entropy of the universe and a decrease in the enthalpy of the system. Select one: O True O False Adding a catalyst to a reaction will change its rate but not its spontaneity. Select one: O True False If systems A and B each consist of one mole of pure liquid H20 at 1 atm pressure and if the temperature TA > TB, then the internal energy of system A must be greater than that of B. Select one: O True O False In an isobaric process, the enthalpy change is equal to the sum of heat and work. Select one: O True O False
For the reaction CaCO3(s) Ca0(s) + CO2(g) ΔΗ AH° = 178.3 kJ and AS° = 160.6 J/K The equilibrium constant for this reaction at 266.0 K is Assume that AHo and AS° are independent of temperature.
V A chem ngineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 100.0 °C and constant total pressure. Then, he measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. 2NO(g) + Cl₂(g) 4 Explanation 2NOCI(g) 2H₂(g) + O₂(g) → 2H₂O(g) Check AH = -76. kJ AS = -278. AG = kJ Which is spontaneous? O this reaction AS the reverse reaction neither AH = -484. kJ…
= ● ENTROPY AND FREE ENERGY Calculating dG from dH and dS A chemical engineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 52.0 °c and constant total pressure. Then, he measures the reaction enthalpy AH and reaction entropy as of the first reaction, and the reaction enthalpy Aн and reaction free energy AG of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and As for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. 2NO(g) + Cl₂(g) → 2NOCI(g) N₂H₂(g) + H₂(g) → 2NH₂(g) ΔΗ - - 76, kJ AS-234. AG = 24 Which is spontaneous? O this reaction O…
A chemical engineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 58.0 °C and constant total pressure. Then, he measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. AH = 107. kJ J AS = 323. K cCL, (e) - C(s) + 2C1, (g) AG = Which is spontaneous? O this reaction O the reverse reaction O neither AH = -803. kJ AS = CH, (2) + 20,(8) - co,() + 2H,0(3)…
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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
A chemical engineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 133.0 °C and constant total pressure. Then, he measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. 2CH₂OH(g) + 30₂(g) → 2CO₂(g) + 4H₂O(g) 4H₂PO4(s) P4O10 (s) + 6H₂0 (1) AH-1353. kJ AS = -3331. AG = Which is spontaneous? Othis reaction O the reverse reaction Oneither ΔΗ = 439. kJ -…
AG (ky/mol) SUbStance / 1on so (ky/mol) -1206.9 /moi k) 92.9 • CaC03l>) -|128.8 • CaO (s) |- 635. I – 60 3.5 38.2 • CO2(9) - 393.5 - 394.4 213.7 191.5 3 H2(g) 202.7 ZNH3 ) -45.9 -16 193 • Hz (g) 202.7 223.0 -92.31 - 95. 30 186.79
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A chem ngineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 42.0 °C and constant total pressure. Then, he measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. ΔΗ Ξ - 1207. kJ J AS = -3779. K P, (g) + 6Cl, (g) → 4PCI, (g) AG = ||| Which is spontaneous? this reaction the reverse reaction neither ДН —D — 12. kJ J AS = K Sn (s) + 2CO,(g). SnO, (s) +…
given rgetable of standard molar entropy values of each substance in the reaction below, what is the standard change in entropy, delta s, for the following reaction? 2CH3OH(g)+3OH2- 2CO2(g)+4H2O(g) Substance= CH3OH(g) S(J/mol•K) 240 Substance=O2(g) S(J/mol•K) 205 Substance=CO2(g) S(J/mol•K) 214 Substance=H2O(g) S(J/mol•k) 189 a. -352 J/K b. -1302 J/K c. 315 J/K d. 89 J/K E. 1830 J/K