Multiple Choice1. This overall reaction is best described as being:a. exothermicb. endothermicc. endergonicd. exergonice. spontaneous in the forward directiona. -35800 kJ/molb. 173.4 kJ/molc. 35800 kJ/mold. 101.7 kJ/mole. -274.2 kJ/mola. +0.46 Vb. +0.617 Vc. +1.39 Vd. -0.46 Ve.+1.21 VGa. 147 g Alb. 0.606 g Alc. 4.55 × 10-3 g AlReactants2. At 298 K, AH° for the following reaction is -137.5 kJ/mol, and AS° is +120.5 J/K.Calculate the value of AG° for this reaction at 298 K.C2H4 (g) + H2 (g) C2H6 (g)d. 16.4 g Ale. 49.1 g AlXReactants2Fe2+ (aq) + Sn4+ (aq)Products3. Use the Table to calculate the standard cell potential (Eºcell) for the voltaic cell basedon the reaction below.Sn2+(aq) + 2Fe3+, (aq)Reaction progressProductsHalf-reactionCr³+ (aq) + 3e-Fe2+ (aq) + 2e-Fe3+ (aq) + e- →Sn4+(aq) + 2e- →→Cr (s)Fe (s)Fe2+ (s)Sn²+ (aq)4. How many grams of aluminum metal are produced in the electrolysis of molten AIC13for 3.25 br with an electrical current of 15.0 A.Al³+ + 3e- Al(s)E° (V)-0,74-0.440+0.771+0.154

Answered: Image /qna-images/answer/f6074dda-1833-416e-886d-172522e50467.jpg

Multiple Choice 1. This overall reaction is best described as being: a. exothermic b. endothermic c. endergonic d. exergonic e. spontaneous in the forward direction a. -35800 kJ/mol b. 173.4 kJ/mol c. 35800 kJ/mol d. -101.7 kJ/mol e. -274.2 kJ/mol G Reactants a. +0.46 V b. +0.617 V c. +1.39 V d. -0.46 V e. +1.21 V Reactants 2. At 298 K, AH° for the following reaction is -137.5 kJ/mol, and AS° is +120.5 J/K. Calculate the value of AG for this reaction at 298 K. C2H4 (g) + H2 (g) C2H6 (g) Products Reaction progress Products 3. Use the Table to calculate the standard cell potential (Eºcell) for the voltaic cell based on the reaction below. Sn²+ (aq) + 2Fe3+ (aq) → 2Fe²+ (aq) + Sn4+ (aq) Half-reaction Cr³+ (aq) + 3e → Cr (s) Fe2+ (aq) + 2e →→ → Fe (s) Fe2+ (s) Fe³+ (aq) + e- → Sn4+ (aq) + 2e- Sn²+ (aq) E° (V) -0.74 -0.440 +0.771 +0.154

Multiple Choice 1. This overall reaction is best described as being: a. exothermic b. endothermic c. endergonic d. exergonic e. spontaneous in the forward direction a. -35800 kJ/mol b. 173.4 kJ/mol c. 35800 kJ/mol d. -101.7 kJ/mol e. -274.2 kJ/mol G Reactants a. +0.46 V b. +0.617 V c. +1.39 V d. -0.46 V e. +1.21 V Reactants 2. At 298 K, AH° for the following reaction is -137.5 kJ/mol, and AS° is +120.5 J/K. Calculate the value of AG for this reaction at 298 K. C2H4 (g) + H2 (g) C2H6 (g) Products Reaction progress Products 3. Use the Table to calculate the standard cell potential (Eºcell) for the voltaic cell based on the reaction below. Sn²+ (aq) + 2Fe3+ (aq) → 2Fe²+ (aq) + Sn4+ (aq) Half-reaction Cr³+ (aq) + 3e → Cr (s) Fe2+ (aq) + 2e →→ → Fe (s) Fe2+ (s) Fe³+ (aq) + e- → Sn4+ (aq) + 2e- Sn²+ (aq) E° (V) -0.74 -0.440 +0.771 +0.154

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter16: Thermodynamics

Section: Chapter Questions

Problem 2E: What is a nonspontaneous reaction?

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