Use the observations about each chemical reaction in the table below to decide the sign (positive or negative) of the reaction enthalpy AH and reaction entropyAS.Note: if you have not been given enough information to decide a sign, select the "unknown" option.reactionobservationsconclusionsAThis reaction is always spontaneous, butproceeds faster at temperatures below143. °C.ΔΗ is(pick one)As is(pick one)BThe reverse of this reaction is alwaysspontaneous but proceeds slower attemperatures below -46. °C.ΔΗ is(pick one)As is(pick one)ΔΗ isCThis reaction is endothermic and proceedsslower at temperatures below 135. °C.(pick one)As is(pick one)x

To determine the signs of ΔH (enthalpy change) and ΔS (entropy change) for the reactions, we can use…

Answered: Use the observations about each…

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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Mg(s) + 2HCI(aq) MgCl, (aq) + H2 (g) + 1550kJ For this reaction at 25°C, Change in enthalpy: [ Select ] O because [ Select] • Change in entropy: [ Select ] O because [ Select ] · Change in Gibbs free energy: [ Select] thus • This reaction is [ Select ]
1. A potential chemical reaction at 25.0 °C has a ΔHrxn of 147.5 kJ and a ΔSrxn of -386.9 J/K. What is the ΔGrxn in kJ. (Enter answer to 3 significant figures and include no units in your answer) Also, what is true about the potential reaction in the previous problem? a. spontaneous b. illegal c. combustive d. nonspontaneous
Use the observations about each chemical reaction in the table below to decide the sign (positive or negative) of the reaction enthalpy AH and reaction entropy AS. Note: if you have not been given enough information to decide a sign, select the "unknown" option. reaction A B C observations This reaction is always spontaneous, but proceeds faster at temperatures below 140. °C. The reaction is never spontaneous. This reaction is spontaneous only above 129. °C but proceeds at a slower rate below 192. °C. AH is AS is conclusions AH is AS is AH is AS is X ✓ (pick one) positive negative unknown (pick one) î (pick one) (pick one) C Ś ↑ (pick one) î
For a given reaction, dH = 32 kJ/mol and dS = 117 J/mol. At approximately what temperature would this reaction become spontaneous?
Use the observations about each chemical reaction in the table below to decide the sign (positive or negative) of the reaction enthalpy AH and reaction entropy AS. Note: if you have not been given enough information to decide a sign, select the "unknown" option. reaction A C observations This reaction is slower below 18. °C than above. This reaction is spontaneous only above 97. °C. This reaction is always spontaneous, but proceeds faster at temperatures above 72. °C. AH is AS is conclusions AH is AS is AH is AS is ✓ (pick one) positive negative unknown (pick one) (pick one) (pick one) (pick one)
Use the observations about each chemical reaction in the table below to decide the sign (positive or negative) of the reaction enthalpy AH and reaction entropy AS. Note: if you have not been given enough information to decide a sign, select the "unknown" option. reaction observations conclusions ΔΗ is (pick one) A The reverse of this reaction is always spontaneous. As is (pick one) ΔΗ is (pick one) B This reaction is spontaneous only below 20. °C. As is (pick one) с This reaction is spontaneous except below 85. °C but proceeds at a slower rate below ΔΗ is (pick one) 129. °C. As is (pick one) ×
Use the observations about each chemical reaction in the table below to decide the sign (positive or negative) of the reaction enthalpy AH and reaction entropy AS. Note: if you have not been given enough information to decide a sign, select the "unknown" option. reaction A B с observations Crystallization of a pure compound is spontaneous only below 23. °C. This reaction is spontaneous only above 31. °C but proceeds at a faster rate above 83. °C. The reverse of this reaction is always spontaneous but proceeds faster at temperatures above 108. °C. AH is AS is AH is AS is conclusions ΔΗ is AS is (pick one) (pick one) (pick one) (pick one) (pick one) (pick one) V
Use the observations about each chemical reaction in the table below to decide the sign (positive or negative) of the reaction enthalpy ▴ and reaction entropy as. Note: if you have not been given enough information to decide a sign, select the "unknown" option. reaction A B C observations The reverse of this reaction is always spontaneous. This reaction is spontaneous except above 64. °C. This reaction is always spontaneous, but proceeds faster at temperatures below 77. °C. AH is AS is conclusions AH is AS is AH is AS is x (pick one) (pick one) (pick one) (pick one) (pick one) (pick one)
Use the observations about each chemical reaction in the table below to decide the sign (positive or negative) of the reaction enthalpy AH and reaction entropy AS. Note: if you have not been given enough information to decide a sign, select the "unknown" option. reaction observations conclusions AH is A This reaction is always spontaneous, but proceeds slower at temperatures below 45. °C. AS is ΔΗ is This reaction is spontaneous only above 150. °C but proceeds at a faster rate above 180. °C. AS is ΔΗ is This reaction is exothermic and proceeds slower at temperatures below 67. °C. AS is X C (pick one) (pick one) (pick one) (pick one) ✓ (pick one) (pick one) Ś ?
Which is true for the following reaction: N₂(g) + 3H₂(g) 2NH3(g) + heat for the reverse reaction, AH is negative. For the reverse reaction, AS is negative. Enthalpy favors the reactants. Entropy favors the reactants. O
Consider a reaction that has a negative H and a positive S. Which of the following statements is TRUE? This reaction will be spontaneous only at high temperatures. This reaction will be spontaneous at all temperatures. This reaction will be nonspontaneous at all temperatures. This reaction will be nonspontaneous only at high temperatures. It is not possible to determine without more information.

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