The graph below shows the change in Gibbs free energy for two reactions. Change in Gibbs Free Energy AGsys (kJ/mol) 6.0 5.0- 4.0- 3.0- 2.0- 1.0- 0.0+ A B C 125 D 150 175 Reaction 2- 200 Which statement can be supported by the evidence shown in the graph? Temperature (K) Reaction 1 225 Reaction 1 is spontaneous, but Reaction 2 is only spontaneous at high temperatures. Both reactions are spontaneous. Reaction 2 is spontaneous, but Reaction 1 is only spontaneous at high temperatures. Neither reaction is spontaneous.

The graph below shows the change in Gibbs free energy for two reactions. Change in Gibbs Free Energy AGsys (kJ/mol) 6.0 5.0- 4.0- 3.0- 2.0- 1.0- 0.0+ A B C 125 D 150 175 Reaction 2- 200 Which statement can be supported by the evidence shown in the graph? Temperature (K) Reaction 1 225 Reaction 1 is spontaneous, but Reaction 2 is only spontaneous at high temperatures. Both reactions are spontaneous. Reaction 2 is spontaneous, but Reaction 1 is only spontaneous at high temperatures. Neither reaction is 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...

See similar textbooks

Similar questions

For each of the following reactions indicate whether as written it will be spontaneous at all temperature only at high enough temperatures only at low temperatures not at any temperatures or if the given information is insufficient to draw a conclu
What is the temperature range in which the following reaction is spontaneous? N₂+ 3H2 → 2NH3 S N2(g) 191.5 J/mol K S H2(g) 130.6 J/mol K S NH3(g) 192.5 J/mol K AH, N2(g) 0 kJ/mol AH, H2(g) 0 kJ/mol AH, NH3(g) -46.19 kJ/mol
Chemistry Above what temperature does the following reaction become non-spontaneous? 2 H₂S(g) + 3 O₂(g) → 2 SO₂(g) + 2 H₂O(g) AH = -1036 kJ; AS = -153.2 J/K O 158.7 K This reaction is nonspontaneous at all temperatures. O 298 K This reaction is spontaneous at all temperatures O 6.762 × 103 K
Consider the oxidation of elemental cadmium (II) oxide. 2Cd(s)+O2 (g)--> 2CdO(s) Using the following thermochemical data, calculate the minimu temperature in degrees Celsius at which this reaction is spontaneous. Species delta Hf degrees (kJ/mol) S degrees (J/molxK) Cd(s) 0 51.8 O2 0 205.2 CdO(s) -258.4 54.8 Select the correct answer: a. 2594 degrees Celsius b. 2321 degrees Celsius c. 1.278 degrees Celsius d. -271.9 degrees Celsius e. -270.6 degrees Celsius
For a particular reaction, AH° = -93.8 kJ and AS° = –156.1 J/K. Assuming these values change very little with temperature, at what temperature does the reaction change from nonspontaneous to spontaneous? T = K Is the reaction in the forward direction spontaneous at temperatures greater than or less than the calculated temperature? less than greater than
The value of ∆G0 for forming water from elemental oxygen and hydrogen is -237kJ/mol. 2H2 +O2 --> 2H2O Calculate the standard enthalpy of formation of water using the entropies below.(Hint: Elemental oxygen and hydrogen have the same enthalpy of formation) O2 H2 H2O S0 (J/molK) 205 130 70
From the values of ΔH and ΔS calculate the minimum temperature at which each reaction will become spontaneous. Enter "None" if the reaction is not spontaneous at any temperature. ΔH = -389 kJ/mol, ΔS = 27.8 J/K · mol
∆Gº for the reaction, H2(g)+Br2(g)⇄2HBr(g), is -33.3 kJ. Which statement below is true? To make this reaction go forward, 33.3 kJ must be added. This reaction is non-spontaneous. This reaction is spontaneous. This reaction cannot be at equilibrium.
The vaporization of compound A is described by the following chemical equation. A(1) A(g) AH vap (78.97 °C) = 37.87 kJ/mol Calculate the entropy of vaporization, A.Svap, for A(1) at 25.0 °C given that the boiling point of A is 78.97 °C, and the molar heat capacity of A(1) is 114.29 J/(mol K). Assume that the molar heat capacity of A(g) is 55.9% of that of A(1). ASvap = Calculate the standard enthalpy of vaporization, AHvap, for A(1) at 25.0 °C. AH vap = Calculate tl AG'vap = x10 TOOLS of vaporization, AGvap, at 25.0 °C. Determine the equilibrium constant K for the va 1970ea J. mol-1. K-1 kJ/mol kJ/mol
4
A reaction has a ΔH of -87.36 kJ and a ΔS of -175.3 J/K. At what temperature (in K) does the reaction become spontaneous? 626.4 K This reaction is always spontaneous 498.3 K 434.6 K This reaction is never spontaneous
For a given reaction, ΔH∘∘= +35.5 kJ/mol and ΔS∘∘= +83.6 J/(K∙∙ mol). In what temperature range is the reaction spontaneous? Assume that ΔH∘∘ and ΔS∘∘ do not vary with temperature.