Use the observations about each chemical reaction in the table below to decide the sign (positive or negative) of the reaction enthalpy ΔH and reaction entropy ΔS.Note: if you have not been given enough information to decide a sign, select the "unknown" option.| reaction | observations | conclusions ||----------|----------------------------------------------------------------------------------------------|----------------------|| A | This reaction is always spontaneous, but proceeds faster at temperatures below 121°C. | ΔH is (pick one) || | | ΔS is (pick one) || B | Crystallization of a pure compound is spontaneous only below 109°C. | ΔH is (pick one) || | | ΔS is (pick one) || C | This reaction is exothermic and proceeds faster at temperatures above 34°C. | ΔH is (pick one) || | | ΔS is (pick one) |**Explanation:**- The table provides observations and requires conclusions about the signs of ΔH (enthalpy change) and ΔS (entropy change) based on given temperature information and spontaneity of reactions.- For each reaction, an explanation is not given, and the appropriate choice must be selected from an unspecified list.

Criteria of spontaneous reaction △G (change in gibbs free energy) < 0 △G = △H - T△S △H-…

reaction A B C observations This reaction is always spontaneous, but proceeds faster at temperatures below 121. °C. Crystallization of a pure compound is spontaneous only below 109. °C. This reaction is exothermic and proceeds faster at temperatures above 34. °C. conclusions AH is AS is AH is AS is AH is AS is (pick one) (pick one) (pick one) (pick one) (pick one) (pick one)

reaction A B C observations This reaction is always spontaneous, but proceeds faster at temperatures below 121. °C. Crystallization of a pure compound is spontaneous only below 109. °C. This reaction is exothermic and proceeds faster at temperatures above 34. °C. conclusions AH is AS is AH is AS is AH is AS is (pick one) (pick one) (pick one) (pick one) (pick one) (pick one)

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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Would conditions of +ΔH and -ΔS favor a spontaneous or non-spontaneous reaction? Why? a. Non-spontaneous because energy is absorbed and contained. b. Spontaneous only at low temperatures because energy is released but it is also somewhat concentrated. c. Spontaneous definitely because energy is released and dispersed. d. Spontaneous only at high temperatures because energy is absorbed but it is also dispersed.
A Moving to another question will save this response. Question 11 A reaction has an equilibrium constant (K) of 58.2. If the entropy of this reaction is-36.7 J/mol"K at a temperature of 317 K, what is the enthalpy of this reaction in kJ/mol? Report your answer to one decimal place. If your answer is negative, make sure to input a negative sign (-). Moving to another question wvill save this response. lyp 144 &
A spontaneous reaction always has: A. a positive enthalpy change and a negative entropy change. B. a positive Gibbs free energy change. C. a negative Gibbs free energy change. D. a standard enthalpy of formation equal to zero for one of the reactants. E. a standard free energy of formation equal to zero for one of the reactants.
Would conditions of +ΔH and -ΔS favor a spontaneous or non-spontaneous reaction? Why? Select one: a.Non-spontaneous because energy is absorbed and contained. b.Spontaneous only at low temperatures because energy is released but it is also somewhat concentrated. c.Spontaneous definitely because energy is released and dispersed. d.Spontaneous only at high temperatures because energy is absorbed but it is also dispersed.
A certain reaction has negative values for both AH and AS. Therefore, the reaction cannot be spontaneous at any temperature. must be spontaneous at all temperatures. can be spontaneous if the temperature is high enough. Ohas a positive free energy at any temperature. can be spontaneous if the temperature is low enough.
At 25 ?C the reaction from Part A has a composition as shown in the table below. Substance Pressure (atm) 3.75 C2H2(g) H2(g) C2H6(g) 5.25x10?2 What is the free energy change, ?G, in kilojoules for the reaction under these conditions? 4.75
49.For the decomposition of hydrogen peroxide to water and oxygen, H2O2(g) ⟶⟶ H2O(g) + O2(g) ΔΔH° = -106 kJ, and ΔΔS° = +0.0580 kJ/K. In what temperature range is the reaction spontaneous (ΔΔG° < 0)? A. The temperature must be greater than 1.83××103 K B. The temperature must be less than 1.83 ××103 K. C. The temperature must be between 225 K and 1.83 ××103 K. D. ΔΔG° is always less than zero. E. ΔΔG° is never less than zero.
chapter 12: 8) Calculate the free-energy change of the following reaction at 448°C and standard pressure. Values in the table are at standard pressure and 25°C. C2H4(g)+3O2(g)--->2CO2(g)+2H2O(g) ΔHºf,(kJ/mol) Sºf, J/mol•K ΔGºf, kJ/mol C2H4(g) 52.3 219.5 68.1 O2(g) 0 205.0 0 CO2(g) –393.5 213.6 –394.4 H2O(g) –241.8