Determine the S'universe at 298 K for the reaction:31.342 J/mol K2NO(g) + 20z(g) → 2NO2(g)For the reaction,4KCIO3(s) → 3KCIO«(s) + KCI(s)Calculate AGʻsys for the process at 298 K if AH'sys =144.3 kJ and AS'sys = -36.8J/K.133.33 kJA key step in the production of sulphuric acid is the oxidation ofSO2(g) + Oz(g) → 2SO3(g)At 98K, AGʻsys = - 500.51kJ; AH’sys = - 494.61. kJ; and AS'sys = -60.16 J/Ka) Use the data to decide if this reaction is spontaneous at 25°, and predicthow AG° will change with increasing TReaction is spontaneous at lower temperature and vice versab) Assuming AH´sys and AS'sys are constant with increasing T, is the reactionspontaneous at 900°C?Spontaneous

Given: 4KClO3(s)→3KClO4(s)+KCl(s)∆Hsyso=144.3kJ∆Ssyso=-36.8J/K

a) Use the data to decide if this reaction is spontaneous at 25°, and predict how AG° will change with increasing T Reaction is spontaneous at lower temperature and vice versa b) Assuming AH'sys and AS'sys are constant with increasing T, is the reaction spontaneous at 900°C? Spontaneous

a) Use the data to decide if this reaction is spontaneous at 25°, and predict how AG° will change with increasing T Reaction is spontaneous at lower temperature and vice versa b) Assuming AH'sys and AS'sys are constant with increasing T, is the reaction spontaneous at 900°C? Spontaneous

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 ΔSvap for hydrogen sulfide from the following data: normal boiling point of H2S: -60.7oC ΔHvap of H2S: 18.7 kJ/mol Place ΔSvap in units of J/(mol K) and your answer should have 3 significant figures.
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For the reaction: 20PCI3(g) 2PCI3(1) + 02(g) AH° = 508 kJ-mol-1 and AS° = 178 J-mol-1.K-1 at 298 K. Which of the following statements is true? Periodic Table and Datasheet O The reaction is spontaneous at all temperatures. O The reaction is spontaneous at high temperatures. O The reaction is spontaneous at low temperatures. O The reaction is not spontaneous at any temperature.
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19 Thermodynamic Quantities for Selected Substances at 298.15 K (25°C) AHf AGf AS° AHf (kJ/mol) AGf (kJ/mol) AS° Substance (kJ/mol) (kJ/mol) (J/mol-K) Substance (J/mol-K) Aluminum Chlorine CI (g) C (аq) Cl2 (g) HCI (aq) HCI (g) Chromium Al (s) AIC13 (s) 28.32 121.7 105,7 - 131,2 165.2 - 705.6 - 630.0 109.3 - 167.2 56.5 Al203 (s) - 1669.8 1576.5 51.00 222,96 - 131.2 -95.27 - 167.2 56.5 186,69 Barium - - Ba(s) BaCO3(s) BaO(s) Beryllium Be(s) 63.2 -92.30 - 1216,3 - 553.5 - 1137.6 112.1 Cr (g) Cr (s) Cr203 (s) Cobalt Со (g) Copper Cu (s) CuCl2 (s) CuO (s) - 525.1 70.42 397.5 352.6 174.2 23.6 9.44 - 1139.7 - 1058.1 81.2 BeO(s) Be(ОН)2(8) 13.77 50.21 - 608.4 -579,1 - 817.9 - 905.8 439 393 179 Bromine 111.8 - 120.9 Br(g) Br-(aq) Br2(g) Br2(1) HBr(g) Calcium Ca(g) Ca(s) CaCO3 (s, calcite) CaCl2(s) CaF2(s) CaO(s) Ca(OH)2(s) CaSO4(s) 82.38 174.9 33.30 108.1 - 102.8 - 167,7 - 128,3 - 147.9 80.71 - 205.9 30,71 3.14 245.3 - 156,1 42,59 - Cu20 (s) Fluorine F (g) F- (aq) F2 (g) HF (g) Hydrogen 152.3…
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?
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