Use the standard free energy data to determine the free energy change for the following reactions, which is run under standard state conditions and 25 °C. Identify it as spontaneous or nonspontaneous at this condition. CASO 2H:0(s)→CASO($)+ 2H;O(g) AG (CaSO s)--132.0kJmol AG (HO g)--228.59 klimol AG (Caso-H;0s)=-1797.45 klimol 0 18.3kJ/mol, nonspontaneous 0-18.3kJ/mol, spontaneous 0 15.6 kl/mol, nonspontaneous

Use the standard free energy data to determine the free energy change for the following reactions, which is run under standard state conditions and 25 °C. Identify it as spontaneous or nonspontaneous at this condition. CASO 2H:0(s)→CASO($)+ 2H;O(g) AG (CaSO s)--132.0kJmol AG (HO g)--228.59 klimol AG (Caso-H;0s)=-1797.45 klimol 0 18.3kJ/mol, nonspontaneous 0-18.3kJ/mol, spontaneous 0 15.6 kl/mol, nonspontaneous

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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a) b)
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For a chemical reaction that is spontaneous at standard conditions, which of the following holds? ΔGorxn > 0; Eocell < 0; K < 1 ΔGorxn > 0; Eocell > 0; K < 1 ΔGorxn < 0; Eocell > 0; K > 1 ΔGorxn < 0; Eocell < 0; K > 1
8e. Consider the following reaction: Caco3 (s) → Cao (s) + CO2 (g) Data: A,H = +177.5 kJ mol1 A,S = +160.7 J mol1K1 At which temperature will the reaction become spontaneous?
The standard reaction free energy AG=-1482. kJ for this reaction: 4 Fe(s) + 30₂(g) 2 Fe₂O3(s) Use this information to complete the table below. Round each of your answers to the nearest kJ. reaction 2Fe₂O₂ (s) 4Fe(s) + 30, (g) - Fe(s) + O₂(g) → Fe₂03 (s) Fe₂O₂ (s) → Fe(s) + 0₂ (8) AG kJ kJ X 5
6
For the reaction CO(g) + 3H2(g)- →CH4(g) + H,O(g) AH° = -206.1 kJ and AS° = -214.7 J/K The equilibrium constant for this reaction at 290.0 K is Assume that AH° and AS° are independent of temperature.
Consider the following reaction at constant pressure. Use the information here to determine the value of AS surr at 298 K. Predict whether or not this reaction will be spontaneous at this temperature. N₂(g) +202(g) → 2NO₂(g) AHrxn = +88.4 kJ mol-1 ASsurr = +88.4J K-1 mol-1, reaction is spontaneous Assurr = -88.4J K-1 mol-1, reaction is spontaneous ASsurr = -88.4J K-1 mol-1, reaction is not spontaneous ASsurr = +297 J K-1 mol-1, reaction is spontaneous ⒸASsurr = -297J K-1 mol-1, reaction is not spontaneous
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For the reaction Fe3O4 (s) + 4H2(g) → 3Fe(s) + 4H₂O(g) AH° = 151 kJ and AS° = 169 J/K The equilibrium constant for this reaction at 342.0 K is Assume that AH° and AS are independent of temperature.