Consider the reaction shown to answer the following question. BaO (s) + CO2 (g) → BaCO3 (s) AH = - and AS° Which statement below is true? This reaction is spontaneous at all temperatures. There is not enough information to make an assessment. O This reaction is non-spontaneous at all temperatures. O This reaction is spontaneous at relatively lower temperatures and non-spontaneous at higher temperatures. O This reaction is spontaneous at relatively higher temperatures and non-spontaneous at lower temperatures.

Consider the reaction shown to answer the following question. BaO (s) + CO2 (g) → BaCO3 (s) AH = - and AS° Which statement below is true? This reaction is spontaneous at all temperatures. There is not enough information to make an assessment. O This reaction is non-spontaneous at all temperatures. O This reaction is spontaneous at relatively lower temperatures and non-spontaneous at higher temperatures. O This reaction is spontaneous at relatively higher temperatures and non-spontaneous at lower 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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Is the following reaction spontaneous (a) only at low temperatures; (b) only at high temperatures; (c) at all temperatures? (d) a reaction can also be never spontaneous (Hint: Find formation values for each species in your book and calculate reaction, you can determine if is positive or negative by looking at the equation.) 2 NO (g) + O2 (g) → 2 NO2 (g)
For a specific reaction, AH = -25.8 kJ/mol and AS = +45.6 J/K-mol. Which of these statements is true? O The reaction is never spontaneous. O The reaction is only spontaneous at high temperatures. OThe reaction is spontaneous at all temperatures. The reaction is only spontaneous at low temperatures.
Calculate AG for a reaction at 85 °C if AH is -34.6 kJ and AS is -114 J/K. Is the reaction spontaneous? Calculate AG for a reaction at -12 °C if AH is -34.6 kJ and AS is -114 J/K. Is the reaction spontaneous? 9. Considering the two questions above, at what temperature does this reaction become spontaneous? ANSWER QUESTION 9
Use the standard free energy of formation data to determine the free energy change for each of the following reactions, which are run under standard state conditions and 25 °C. Identify each as either spontaneous or nonspontaneous at these conditions. a. MnO₂ (s) → Mn (s) + O₂ (g) b. H₂(g) + Br2 (1)→ 2HBr (g) c. Cu (s) + S (g) → CuS (s) d. 2LiOH (s) + CO₂ (g) → Li₂CO3 (s) + H₂O (g)
Consider the following reaction
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
The reaction, Fe203(s) + 3C(s) → 2Fe(s) + 3CO(g) AH° = +490.7 kJ, AS° = +541 J-K-1 %3D This reaction is spontaneous only below a certain temperature always spontaneous never spontaneous spontaneous only above a certain temperature
33. Use the standard free energy of formation data in Appendix G to determine the free energy change for each of the following reactions, which are run under standard state conditions and 25 °C. Identify each as either spontaneous or nonspontaneous at these conditions. MnO2 (s) ⟶ Mn(s) + O2 (g) H2 (g) + Br2 (l) ⟶ 2HBr(g) Cu(s) + S(g) ⟶ CuS(s) 2LiOH(s) + CO2 (g) ⟶ Li2CO3 (s) + H2O(g) CH4 (g) + O2 (g) ⟶ C(s, graphite) + 2H2O(g) CS2 (g) + 3Cl2 (g) ⟶ CCl4(g) + S2Cl2 (g)
1.) Complete A and B to move on. a.) Write the complete, balanced chemical equation for the following reaction on a separate sheet of paper. Provide products where they are not given. Assume that the reaction is spontaneous. Propane (C3H8) + oxygen → carbon dioxide + water Type the sum of the coefficients in the equation into the answer blank. If there is no coefficient, count it as one. Include ( g, s, l, or aq) b.) Write the complete, balanced chemical equation for the following reaction on a separate sheet of paper. Provide products where they are not given. Assume that the reaction is spontaneous. Diphosphorus pentoxide + water → Type in the coefficient and formula for the product in the equation that contains phosphorus. Include ( g, s, l, or aq)
The following reaction is endothermic. 2NH3(g) → N2(g) + 3H2(g) This means the reaction A. will be spontaneous at high temperatures. B. will be spontaneous at low temperatures. C. is not spontaneous at any temperature. D. is spontaneous at all temperatures.
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