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.reactionobservationsconclusionsThis reaction is always spontanecus, butproceeds faster at temperatures below94. °C.negative 0AAS ispositve 0Al isIick one eThis reaction is faster above - 10. "C thanbelow.AS isIpick one 0AH isk one 0This reaction is spontaneous only below148. °CAS isIrick one回唱

Concept: From the thermodynamic ∆G = ∆H -T∆S A reaction will be spontaneous only when ∆G < 0…

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 AN is This reaction is always spontanecus, but proceeds faster at temperatures below 94. "C. negative 0 A AS is positve AN is Iick one e This reaction is faster above - 10. "C than below. AS is Ipick one 0 AN is k one 0 This reaction is spontaneous only below 148. °C AS is Inick 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 AN is This reaction is always spontanecus, but proceeds faster at temperatures below 94. "C. negative 0 A AS is positve AN is Iick one e This reaction is faster above - 10. "C than below. AS is Ipick one 0 AN is k one 0 This reaction is spontaneous only below 148. °C AS is Inick 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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3. Use the AH° and AS° values below to determine the range of temperatures (in kelvin, K) for which the respective reaction will be favorable AH° = -904 kJ AS° = +0.179 kJ/K AH° = +173 kJ AS° = +0.176 kJ/K AH° = -139 kJ AS° = -0.286 kJ/K AH° = +285 kJ AS° = -0.138 kJ/K
3. - the free energy under the biochemical standard states. Select all that apply. O AG O AG O AG O AG 4. is the free energy of the transition state. O AGt CAG OAG OAG"
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 slower below - 1. °C than above. This reaction is spontaneous only below -3. °C. The reaction is never spontaneous. AH is AS is conclusions AH is As is AH is AS is X ✓ (pick one) î positive negative unknown (pick one) (pick one) (pick one) (pick one) Ś ↑ î
D Try Again Your answer is incorrect. 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 • reaction A: Your answer is incorrect. • reaction C: Your answer is incorrect. B с observations The reverse of this reaction is always spontaneous. This reaction is exothermic and proceeds slower at temperatures below -26. °C. This reaction is always spontaneous, but proceeds faster at temperatures above 139. °C. AH is AS is conclusions AH is As is AH is AS is X unknown negative ŷ negative ↑ unknown î unknown ↑ positive î S
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An spontaneous process ALWAYS has a negative AG has a negative AH has a positiveAH has a positive AG
3.
34. Which of the following reactions has a positive entropy change? 2SO + Oe) 2S0) 2NH,NO, - 2N + 4H,0 + Oe) BF + NH F,BNH) H,O, - H,O CLEAR ALL < PREVIOUS O 27 26 28 O 29 O 30 О 31 32 O 37 36 38 39
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A cvg.cengagenow.com Flipgrid | 50ffc. GRLContent Netflix Favorites My Home 3-Day General.. Netflix Content [Review Topics] [References] 2req Use the References to access important values if needed for this question. 2req The free energy change for the following reaction at 25 °C, when [H*] = 7.21×10³ M and [Hg²*]=1.17 M, is 178 kJ: 2req 2H*(7.21×10-3 M) + Hg(1)→ H,(g) + Hg²*(1.17 M) AG= 178 kJ What is the cell potential for the reaction as written under these conditions? s 2req Answer: V ts 2req Would this reaction be spontaneous in the forward or the reverse direction? ots OM) pts 2reg Submit Answer Retry Entire Group 9 more group attempts remaining pts M) pts
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ab Lock Fn 50 Esc Why is the exothermic reaction below spontaneous at all temperatures? Select the correct answer below: O Because AH is positive and AS is positive. Because AH is negative and AS is positive. O Because AH is negative and AS is negative. O Because AH is positive and AS is negative. 1 ! F1 A N F2 8 2 W S X Alt F3 3 E D F4 C $ TiCl4 (9) + 2H₂O(g) → TiO2 (s) + 4HCI(g) पं F5 R F % 5 V F6 T G < 6 F7 B DELL H F8 7 N F9 *00 M F10 5 2 F11 Alt 3 F12 P PrtScr "R Ctrl { [ ? Ins Pa U