Deposits of elemental sulfur are often seen near active volcanoes. Their presence may be due to the following reaction of SO2 with H2S:so, (8) + 2H,S (g) →Sg(s)+2H,0(g)1st attempti See Periodic TableAssuming the values of A Hixn and ASfxn do not change appreciably with temperature, at what temperature does the reaction becomespontaneous?K

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Deposits of elemental sulfur are often seen near active volcanoes. Their presence may be due to the following reaction of SO, with H2S: so, (8) + 2H,S(8) () + 2H1,0(3) > 1st attempt See Periodic Table Assuming the values of A Hxn and ASixn do not change appreciably with temperature, at what temperature does the reaction become spontaneous? K

Deposits of elemental sulfur are often seen near active volcanoes. Their presence may be due to the following reaction of SO, with H2S: so, (8) + 2H,S(8) () + 2H1,0(3) > 1st attempt See Periodic Table Assuming the values of A Hxn and ASixn do not change appreciably with temperature, at what temperature does the reaction become spontaneous? K

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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at el Solve the following problems. ende 1. From the following AH and AS values, predict whether the reaction would be spontaneous. If not, at what temperature might the reaction become spontaneous? AH = -126 kJ 0)ont e) (lo\ AS = 84 J/K 6.6 ges 2.8 olgmoxa dard x ndiions, Gre free emergy change is caled
Spontaneous or non-spontaneous
For a chemical reaction to be spontaneous at all temperatures, which of the following conditions must be met? O Itis not possible for a reaction to be spontaneous at all temperatures. O AS° > 0, AH > 0 O AS° > 0, AH 0
At 1200 oC, the reduction of iron (III) oxide (Fe2O3) to elemental iron is not spontaneous: 2Fe2O3(s) → 4Fe(s) + 3O2(g) rG° = +840 kJ At the same temperature solid carbon spontaneously reacts with oxygen, to form CO2 gas. It is found that by mixing carbon with Fe2O3 at this temperature the reduction can be made to proceed, providing at least 3 moles of carbon are present for every 2 moles of Fe2O3. (a)write a balanced equation for the total reaction (b) Use the reaction stoichiometry to determine an upper limit for rG, i.e. the least negative value possible, for the reaction of carbon with oxygen at this temperature. (+840 is the only delta G value given in the question)
6. For each reaction below, determine the sign of AH and AS. Also state under what conditions the reaction is spontaneous (in the forward direction): (a) never spontaneous, (b) always spontaneous, (c) spontaneous at low temperatures, or (d) spontaneous at high temperatures. 1) C2 (g) → 2 Cl (g) (ii) 2 C2H6 (g) + 7 O2 (g) → 4 CO2 (g) + 6 H2O (g)
Calculate the AS°rxn of the following reaction at 223°C and standard pressure. 1st attempt O See Hint C,H,(8) + 30,(g) . 200,(g) + 2H,0(g) AH°f, kJ/mol S°, J/mol K AG°F, kJ/mol C2H4(g) 52.3 219.5 68.1 O2(g) 205.0 CO2(g) -393.5 213.6 -394.4 H20(g) -241.8 188.7 -228.6 J/mol K
For a nonspontaneous reaction , AS° = 189 J/K, and AH° = 76.3 KJ. At what temperature this reaction becomes spontaneous ? 520 K 302 K 298 K 404 K
For the reaction delta H° = 98.8 kJ/mol and delta S° =141.5 J/(mol*K). 3H2 (g) +Fe2O2(s) →2Fe(s) +3H2O(g) (19) Over what temperature range (if any) is the reaction spontaneous?
Determine the AHrxn • AH° N2(g) = 0 kJ/mol • AH°+ H2(g) = 0 kJ/mol • AH˚ NH3(g) = -46.19 kJ/mol о
Which one of the following processes would you expect to be spontaneous only at high temperatures? options: H2O (1) - --> H2O (g) 3 02 (g )-- --> 2 03 (g) Mg (s) + Cl2 (g) - --> MgCl2 (s) CO2 (g) ) 2 H2 (g) + O2 (g) --> 2 H2O (g) - CO2 (s
5:49 Question 9 of 15 A) It is exothermic Which of the following is true for a process where AS (universe) < 0 at 298 K? B) It is nonspontaneous. C) It is product-favored. D) It is spontaneous. E) It is endothermic. ..ll 5GW Tap here or pull up for additional resources Submit