Consider the reaction below at 25°C: 2 N205 (g) = 4NO2 (g) + O2 (g) AG° rxn =+1.65 kJ What is AG when [N205] = 0.0019 M, [NO2] = 0.065 M and [02] = 5.2 M? O a. -1.01 b. +2.63 kJ C. -1.65 kJ d. +9.70 kJ e. +9.3 kJ For the reaction C2H6 (g) C2H4 (g) + H2 (g) -> AH° is +137 kJ/mol and AS° is +120 J/K. mol. Which statement is true? O a. spontaneous only at low temperature b. nonspontaneous at all temperatures C. spontaneous only at high temperature O d. spontaneous at all temperatures

Consider the reaction below at 25°C: 2 N205 (g) = 4NO2 (g) + O2 (g) AG° rxn =+1.65 kJ What is AG when [N205] = 0.0019 M, [NO2] = 0.065 M and [02] = 5.2 M? O a. -1.01 b. +2.63 kJ C. -1.65 kJ d. +9.70 kJ e. +9.3 kJ For the reaction C2H6 (g) C2H4 (g) + H2 (g) -> AH° is +137 kJ/mol and AS° is +120 J/K. mol. Which statement is true? O a. spontaneous only at low temperature b. nonspontaneous at all temperatures C. spontaneous only at high temperature O d. spontaneous at all temperatures

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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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
Under which one of the following conditions will the following reaction be spontaneous as written? 2CO(g) + O2(g) → 2 CO2(g) AH-565.97 kJ/molrxn, AS-173.0 J/molrxnk Select one: a. spontaneous at all temperatures O b. spontaneous at low temperatures O c. spontaneous at high temperatures O d. not spontaneous at any temperature
Which of the following combinations of values for AH and AS for a given process, indicate that the process is spontaneous at all temperatures? A. O Both AH and AS are positive. B. O Both AH and AS are negative. C. O AH is positive and AS is negative. D. O AH is negative and AS is positive.
For a given reaction, ΔH = +35.5 kJ/mol and ΔS = +83.6 J/mol·K. Which of the following is TRUE? a. The reaction is spontaneous at standard conditions. b. The reaction is spontaneous at T > 425 K. c. The reaction is spontaneous at all temperatures. d. The reaction is spontaneous at T < 425 K.
1. Find DHrxn, DSrxn, and DGrxn, using the tables at the end of your textbook for the phase change of water from liquid to gas at 25.0°C. H2O (l) <---> H2O (g) 2. Is this phase change spontaneous at 25.0°C? Give the reason for your answer. 3. Find the temperature at which this phase change becomes spontaneous. Give in both K and ℃. 4. Is this what you expect, and why? (Is the answer to question #3 what you expect)
39. provide the answer ASap
The following reaction takes place at 120°C: H20( I) → H20( g) AH 44.0 kJ/ mol AS = 0.119 kJ/mol K Which of the following must be true? O a. The reaction is not spontaneous. b. The reaction is spontaneous. O c. AG = 0 O d. AG <0 O e. Two of these.
If the process is exothermic and not spontaneous, then what must be TRUE? O a. AS0 O c. AH=0 O d. AS> 0
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