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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12. Consider the oxidation of iron metal 4Fe +302g → 2FE2O3() , by determining the sign of Astotal, Show that the reaction of spontaneous Material Fe Fe2O3 87.4 O2 S° J/K.mol ΔΗ, K/mol 27.3 205.0 -824.2
(a) Using Gibb's free energy equation, predict whether at 28.0 °C, the following reaction is spontaneous or not: 4 NH3 (g) + 5 O2 (g) 4 NO (g) + 6 H2O (g) (Given: AU = + 9.08 kJ.mol¬' and AS = + 35.7 JK-' mol-') Hint: Use AU and above equation to calculate AH first. (b) Calculate the Change in Gibb’s Free energy for the following reaction and predict whether the reaction is spontaneous under standard conditions or not? 4 KCIO3 (9) — ЗКСІО4 (9) + КCІ () Given: Molecules дн? (кJ/mol) S°(J/mol.K) KCIO3 (s) -397.7 143.1 KCIO4 (s) -432.8 151.0 KCI (s) -436.7 82.6
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.
At what point the reaction is spontaneous at? 2CH4(g) + 3O2(g) -> 2H2O(l) + 2CO2(g) A. At low T B. At high T C. It depends on the temperature D. All temperature ranges E. The reaction is not spontaneous at T
Solve the following problem. Use GRESA Calculate in change in Enthalpy and Entropy of the Chemical reaction. Get the Gibb's free energy in both different temperatures. Indicate if the reaction is spontaneous or non-spontaneous NH.C(s) –> NH3 (g) + HCI (g) Find the AG° at 25 °C and AG at 500 °C.
When AH is negative and AS is positive, the reaction is: ONever spontaneous Spontaneous at low temperatures O Always spontaneous O Spontaneous at high temperatures
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The reaction 2 C4H10(g) + 13O2(g) - has AG° = -5407 kJ. Determine the value of AG°, for C4H10(8). 8 CO2lg) + 10 H20(g) Standard Free Energies of Formation of Typical Substances at 298.15 K TABLE 18.2 Substance Substance Substance AG? (kJ mol ') AG? (kJ mol-") AG? (kJ mol ) Agt) CaO6) -604.2 K,SO,G) -1316.4 AgC6) -109.7 Ca(OH),() -896.76 N,() Al() 0.00 CaSO) NH,(g) NH.CI() -1320.3 -16.7 ALĻO,6) C) (graphite) COO Co,( -1576.4 CaSO, H,OG) -1435.2 - 203.9 CaSO,2H,0G) -1795.7 NO(g) + 86.69 NO,(g) N,O) N,0, -137.3 +51.84 -394.4 Fe() +103.6 CH( -50.79 Fe,O,6) -741.0 +98.28 CH,A(g) -58.6 Na() CH,OH() -166.2 H,0(g) -228.6 Na,CO,() -1048 CO(NH)l) -197.2 -237.2 NaHCO,6) -851.9 CO(NH)(ag) C,H,(g -203.8 HCI -95.27 NaC) -384.0 +209 HNO,) -79.91 NaOH) -382 +68.12 H,SO() -689.9 Na,SO.) -1266.8 HC,H,0,(/) Hg(/) Hg(g) -32.9 -392.5 C,H,OH() -174.8 PbO) -189.3 +17.3 +31.8 Ca(o) K() SO;(g) -300.4 Ca00,() -1128.8 KCI) -408.3 -370.4 CaC,6) -750.2 i kJ e Textbook and Media Choose the value of K, for the…
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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?
H.W/ Which the substance in each following pairs would have the greater entropy? Explain. (a) At 75°C and 1 bar: 1mol H,O (1) or 1 mol H20 (g) (b) At 5°C and 1 bar: 50g Clor 0.8 mol Cl, (g) (c) 1 mol Br2 (1, 1 bar, 8°C) or 1 mol Br, (s, 1 bar, -8°C) (d) 0.312 mol SO2 (g, 0.110 bar, 32.5 °C) or 0.284 mol (g, 15 bar, 22.3°C).
Calculate ∆G° for the reaction of iron(III) oxide with carbon monoxide to give elemental iron and carbon dioxide.Use data in the table below: