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 67.0 °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. 2NH₂(g) → N₂H₂(g) + H₂(g) 4FeC1₂ (s) + 30₂ (g) - 6C₁₂(g) + 2Fe₂O₂ (s) AH = 188. kJ AS = 553. J K AG = 1 kJ Which is spontaneous? O this reaction O the reverse reaction neither AH = -50. kJ AS = AG = 11. kJ Which is spontaneous? Othis reaction O the reverse reaction O neither 00

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 67.0 °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. 2NH₂(g) → N₂H₂(g) + H₂(g) 4FeC1₂ (s) + 30₂ (g) - 6C₁₂(g) + 2Fe₂O₂ (s) AH = 188. kJ AS = 553. J K AG = 1 kJ Which is spontaneous? O this reaction O the reverse reaction neither AH = -50. kJ AS = AG = 11. kJ Which is spontaneous? Othis reaction O the reverse reaction O neither 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...

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For a certain chemical reaction, the standard Gibbs free energy of reaction at 15.0 °C is 142. kJ . Calculate the equilibrium constant K for this reaction.Round your answer to 2 significant digits.
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 15.0 °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 = -1207. kJ J AS = -4236. K P,(g) + 6CL, (3) 4PCI, (g) AG = kJ Which is spontaneous? O this reaction O the reverse reaction O neither AH = -76. kJ AS = 2NO(g) + CL, (3) → 2NOC1(g)…
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 130.0 °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. Al₂O3(s) + 2Fe(s) → 2Al(s) + Fe₂O3(s) CO₂(g) + 2H₂O(g) → CH₂(g) + 20₂(g) AH = 852. kJ AS = 2044. AG = | KJ Which is spontaneous? this reaction the reverse reaction neither = 803. kJ…
Match equivalent statements. Standard Gibbs free energy of reaction 0 no preference for reactants or products at equilibrium Standard Gibbs free energy of reaction = 0 products dominate at equilibrium
AH = 439. kJ J AS = 1285. K 4H, PO, (s) - P,010 (s) + 6H,0(1) AG = kJ Which is spontaneous? this reaction the reverse reaction neither AH = 852. kJ J AS = || K Al, 0, (s) + 2Fe(s) -→ 2A1(s) + Fe,0,(s) AG = 0. kJ Which is spontaneous? this reaction the reverse reaction neither O O O
dont round and take your time please
A chemical engineer is studying the two reactions shown in the table below. In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 33.0 °C and constant total pressure. Then, she 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 her measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and A.S 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. N₂(g) + 3H₂(g) → 2NH₂(g) 2NO(g) N₂(g) + O₂(g) AH = -92. kJ AS = -214. AG = kJ Which is spontaneous? Othis reaction O the reverse reaction O neither AH = -181. kJ AS = J K J K AG =…
A chemical engineer is studying the two reactions shown in the table below. In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 96.0 °C and constant total pressure. Then, she 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 her 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- - 2220. kJ J AS = -6102. K C,H, (g) + 50,(g) → 3C0,(8) + 4H,0() AG = ||| kJ Which is spontaneous? this reaction the reverse reaction neither
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 54.0 °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.
A chemical engineer is studying the two reactions shown in the table below. In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 123.0 °C and constant total pressure. Then, she 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 her 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. alo Ar AH = 1353. kJ J AS = 3371. K 2co, (g) + 4H,0(g) → 2CH,он (g) + зо, (з) AG = ||| kJ Which is spontaneous? this reaction the reverse reaction neither
Classify each of the reactions according to one of the four reaction types summarized in the table below. Reaction Spontaneous Process? Турe ΔΗ' (system) AS" (system) (Standard Conditions) 1 Exothermic, 0 Spontaneous at all temperatures. AS (universe) > 0. Exothermic, 0 Positive, > 0 Depends on relative magnitudes of AH and AS°. Spontaneous at higher temperatures. 3 4 Endothermic, > 0 Negative, < 0 Not spontaneous at any temperature. AS" (universe) <0. C,H12 O6 (s) + 6 O2(g) → 6 CO2 (g) + 6 H2O(L) a. A,H° = -673 kJ/mol-rxn A,S° = 60.4 J/K · mol-rxn O Spontaneous at all temperatures. O Spontaneous at lower temperatures. Spontaneous at higher temperatures. ONot spontaneous at any temperature. b. FeO(s) + C(graphite) → Fe(s) + CO(g) A,H° = 153.2 kJ/mol-rxn A,S' = 160.4 J/K · mol-rxn O Spontaneous at all temperatures. O Spontaneous at lower temperatures. Spontaneous at higher temperatures. ONot spontaneous at any temperature.
Classify each of the reactions according to one of the four reaction types summarized in the table below. Reaction Spontaneous Process? Туре ΔΗ' (system) AS (system) (Standard Conditions) 1 Exothermic, 0 Spontaneous at all temperatures. AS (universe) > 0. Exothermic, 0 Positive, > 0 Depends on relative magnitudes of AH and AS". Spontaneous at higher temperatures. 3 Endothermic, > 0 Negative, < o Not spontaneous at any temperature. AS° (universe) < 0. 4 C6 H12O6 (s) + 6 02 (g) → 6 CO2 (g) + 6 H2O(l) a. A,H° = -673 kJ/mol-rxn A,S° = 60.4 J/K · mol-rxn O Spontaneous at all temperatures. O Spontaneous at lower temperatures. O Spontaneous at higher temperatures. ONot spontaneous at any temperature. b. ВаО(s) + C(graphite) — Ba(s) + СО(g) A,H° = 437.6 kJ/mol-rxn A,S° = 184.9 J/K· mol-rxn OSpontaneous at all temperatures. O Spontaneous at lower temperatures. O Spontaneous at higher temperatures. ONot spontaneous at any temperature.