For each chemical reaction listed in the first column of the table below, predict the sign (positive or negative) of the reaction entropy ASyn: If it's not possible to rxn' decide with the information given, check the "not enough information" button in the last column. Note for advanced students: Assume the temperature remains constant. Assume all gases and solutions are ideal. reaction sign of reaction entropy AS < 0 rxn AgCI(s) Ag (ag) + CI (aq) O AS vo > 0 rxn O not enough information. O AS < 0 rxn MgCl, (s) + H,O(1) MgO (s) + 2HC1(g) O AS > 0 rxn O not enough information. AS < 0 rxn Ba (OH), 8H,0(s) + 2N - Васl, (ag) + 2Nн, (аq) + 1он,о() O AS v. > 0 rxn not enough information.

For each chemical reaction listed in the first column of the table below, predict the sign (positive or negative) of the reaction entropy ASyn: If it's not possible to rxn' decide with the information given, check the "not enough information" button in the last column. Note for advanced students: Assume the temperature remains constant. Assume all gases and solutions are ideal. reaction sign of reaction entropy AS < 0 rxn AgCI(s) Ag (ag) + CI (aq) O AS vo > 0 rxn O not enough information. O AS < 0 rxn MgCl, (s) + H,O(1) MgO (s) + 2HC1(g) O AS > 0 rxn O not enough information. AS < 0 rxn Ba (OH), 8H,0(s) + 2N - Васl, (ag) + 2Nн, (аq) + 1он,о() O AS v. > 0 rxn not enough information.

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 chemical reaction listed in the first column of the table below, predict the sign (positive or negative) of the reaction entropy A.Sxn If it's not possible to decide with the information given, check the "not enough information" button in the last column. Note for advanced students: Assume the temperature remains constant. Assume all gases and solutions are ideal. reaction H₂O(/) + AL₂ S₂ (s) → H₂S (g) + Al₂O₂ (s) 2C₂H, (g) + 70₂(g) → 4CO₂(g) + 6H₂O(g) BaCl₂ (aq) + K₂SO4 (aq) BaSO₂ (s) + 2K Cl(aq) sign of reaction entropy AS rxn AS rxn not enough information. AS 0 X 0 rxn not enough information. 3
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 25.0 °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. 2NO(g) N₂(g) + O₂(g) - - N₂H (9) + H₂(g) → 2NH₂(g) ΔΗ = = 181. ΚΙ AS-568. AG = KJ Which is spontaneous? Othis reaction O the reverse reaction Oneither AH-188. kJ J K AS = D² K AG=…
es) Qualitatively predicting reaction entropy For each chemical reaction listed in the first column of the table below, predict the sign (positive or negative) of the reaction entropy AS If it's not possible to decide with the information given, check the "not enough information" button in the last column. Note for advanced students: Assume the temperature remains constant. Assume all gases and solutions are ideal. reaction N₂(g) + 3H₂(g) → 2NH, (e) 4Fe()+30.)- 2Fe₂O, (s) N. (3), (g) 2NH, (g) sign of reaction entropy 04 ron reaction <<0 50 not enough information. 45x 250 <<0 not enough information. 450 50 not enough information. Using the general properties of Gibbs free energy The standard reaction free energy AG" --835. kJ for this reaction: 2 Al(s) + Fe₂O3(s)-Al₂O3(s) + 2 Fe(s) Use this information to complete the table below. Round each of your answers to the nearest kJ. BALAKEN F04 AGO Focus
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 69.0 °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. HCH, CO₂(1)→ CH₂OH(g) + CO(g) Al₂O₂ (s) + 2Fe(s) -> 2A1(s) + Fe₂O₂ (s) AH = 172. kJ AS = 543. AG = Which is spontaneous? O this reaction O the reverse reaction Oneither ΔΗ = 852. kJ…
For each chemical reaction listed in the first column of the table below, predict the sign (positive or negative) of the reaction entropy AS, to decide with the information given, check the "not enough information" button in the last column. I rxn Note for advanced students: Assume the temperature remains constant. Assume all gases and solutions are ideal. reaction CaCl₂ (aq) + Na₂CO3(aq) → CaCO3 (s) + 2NaCl(aq) CaO(s) + CO,(g) CaCO3(s) HCI(g) + NH₂(g) NH₂Cl(s) sign of reaction entropy AS rxn AS > 0 rxn not enough information. AS 0 rxn not enough information. AS 0 rxn not enough information. X If it's not possible
rxn For each chemical reaction listed in the first column of the table below, predict the sign (positive or negative) of the reaction entropy AS. If it's not possible to decide with the information given, check the "not enough information" button in the last column. Note for advanced students: Assume the temperature remains constant. Assume all gases and solutions are ideal. reaction H₂O (1) + Al₂S₂ (s) → H₂S (g) + Al₂O₂ (s) CO(g) + 2H₂(g) CH₂OH (g) CaO(s) + CO,(g) CaCO3(s) sign of reaction entropy AS 0 rxn not enough information. AS 0 rxn not enough information. AS 0 rxn not enough information. X S
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 24.0 °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. AH = 188. kJ AS = X Ś ? N₂H₂(g) + H₂(g) → 2NH₂(g) AG = 4 2 P₂(g) + 6Cl₂ (g) 4PC1₂ (g) 688. kJ Which is spontaneous? this reaction the reverse reaction neither AH = - 1207. kJ J AS =…
#3 Calculate the standard entropy, AS in, of the reaction at 25.0 C using the table of thermodynamic properties. C₂H₂(g) + H₂O(1)→ C₂H₂OH(1) ASixn = Calculate the standard Gibbs free energy of the reaction, AGixn. The standard enthalpy of the reaction, AHxn, is -44.2 kJ.mol-¹. AGixn= TOOLS x10 Determine in which direction the reaction is spontaneous as written at 25.0 °C and standard pressure. $ 4 % 5 Okay MacBook Pro & N You 8 ( BABAE 9 J-K-¹-mol-1 A kJ-mol-1 O delet-
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