Part A Learning Goal: To use molecular-level diagrams to predict the signs of thermodynamic properties. The equations The image (Eigure 1) represents a spontaneous, gaseous reaction. Predict whether AH, AS, and AG for this reaction are positive, negative, or zero. AG = -RTINK and Drag each item to the appropriate bin. > View Available Hint(s) AG = AH - TAS relate entropy change, AS, enthalpy change, AH, free energy change, AG, and the equilibrium constant, K, for a given reaction at a given temperature. Reset Help AGAH AS Positive Zero Negative Submit • Part B For the gaseous reaction shown here, the bins below represent three different possibilities for the equilibrium mixture. Classify each mixture by what it indicates about AG, K, and InK for the reaction at standard conditions. Drag each item to the appropriate bin. > View Available Hint(s) Reset Help AG° = 0] AG° >0 AG° <0 AG <0 K= 1K>1 K<1 In K=0 In K>0 In K<0 Mixture 1 Mixture 2 Mixture3 Figure 1 of 1 Submit Provide Feedback Next > ceso

Part A Learning Goal: To use molecular-level diagrams to predict the signs of thermodynamic properties. The equations The image (Eigure 1) represents a spontaneous, gaseous reaction. Predict whether AH, AS, and AG for this reaction are positive, negative, or zero. AG = -RTINK and Drag each item to the appropriate bin. > View Available Hint(s) AG = AH - TAS relate entropy change, AS, enthalpy change, AH, free energy change, AG, and the equilibrium constant, K, for a given reaction at a given temperature. Reset Help AGAH AS Positive Zero Negative Submit • Part B For the gaseous reaction shown here, the bins below represent three different possibilities for the equilibrium mixture. Classify each mixture by what it indicates about AG, K, and InK for the reaction at standard conditions. Drag each item to the appropriate bin. > View Available Hint(s) Reset Help AG° = 0] AG° >0 AG° <0 AG <0 K= 1K>1 K<1 In K=0 In K>0 In K<0 Mixture 1 Mixture 2 Mixture3 Figure 1 of 1 Submit Provide Feedback Next > ceso

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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Using enthalpies of formation, calculate ΔΗ° for the following reaction at 25°C. Also calculate AS for this reaction from standard entropies at 25°C. Use these values to calculate AGO for the reaction at this temperature. Species AH (kJ/mol) S (J/mol.K) COC12 (9) H₂O(1) CO₂(g) HCl(g) ΔΗ° = AS° AGⓇ -220.1 -285.8 -393.5 -92.31 KJ J/K 283.9 kJ 69.95 COC12(g) + H₂O(1) → CO₂ (g) + 2HCl(g) 213.7 186.8
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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 (pick one) The reverse of this reaction is always spontaneous but proceeds faster at A temperatures above 25. °C. AS is (pick one) v This reaction is spontaneous except below AH is (pick one) 63. °C but proceeds at a faster rate above 117. °C. AS is (pick one) v AH iS This reaction is always spontaneous, but proceeds faster at temperatures above (pick one) v C 115. °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 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
Predict the sign of the entropy change, A,S°, for each of the reaction displayed. Drag the appropriate items to their respective bins. • View Available Hint(s) Reset Help A : Ba?- (ag) + SO4²- (ag)→BASO( : Ca(OH)2(s)→C2O(s) + H2O(g) C: 2N20(9)→2N2(9) + O2(9) D: 2Na(s) + Cl2(9)→2NaCl(s) E : C3H3 (9) + 502(9)→3CO2(9) +4 F: 12(s)¬I2(9) Positive Negative
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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ll Verizon ? 5:55 AM 9 100% webassign.net Among other things, an ideal fuel for the control thrusters of a space vehicle should decompose in a spontaneous exothermic reaction when exposed to an appropriate catalyst. Evaluate the following substances under standard state conditions as suitable candidates for fuels. (Provide AG° and AH° in kJ/mol reactant.) (a) nitrous oxide: N,0(g) → N2(9) + 1/2 0,(9) AG° = kJ/mol AH° = kJ/mol Spontaneity O spontaneous O nonspontaneous Thermicity O endothermic O exothermic Suitability O suitable O not suitable (b) diborane: B,H,(9) - 2 B(s) + 3 H,(9) AG° = kJ/mol AH° = kJ/mol Spontaneity O spontaneous O nonspontaneous Thermicity O endothermic exothermic Suitability O suitable O not suitable (c) dinitrogen trioxide: N,0,(9) – N,(9) + 3/2 0,(9) AG° = KJ/mol AH° - kJ/mol Spontaneity O spontaneous O nonspontaneous Thermicity O endothermic O exothermic Suitability O suitable O not suitable (d) aluminum hydride: AIH, (s) – Al(s) + 3/2 H,(9) AG° = kJ/mol ΔΗ' -…
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on Item 3 Review Constants Periodic Table Part C Complete previous part(s) Part D Calculate the standard-state entropy for the following reaction: 1 CHĄ(g) +2 O2(g) → 1 CO2(g) + 2 H2O(1) (If applicable, coefficients of one have been included for clarity.) The standard entropy values are given in the table. S° Formula J/(K-mol) CO2(g) 214 H2O(1) 189 CH4(g) 186 O2(g) 205 Express your answer with the appropriate units. • View Available Hint(s)
Calculate ∆G° for the reaction of iron(III) oxide with carbon monoxide to give elemental iron and carbon dioxide.Use data in the table below:
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 This reaction is spontaneous only above ΔΗ is (pick one) A 144. °C but proceeds at a faster rate above 181. °C. AS is |(pick one) ΔΗ is |(pick one) В This reaction is exothermic. AS is |(pick one) ♥ ΔΗ is |(pick one) This reaction is always spontaneous, but proceeds slower at temperatures below -37. °C. C AS is |(pick one) ?