es)Qualitatively predicting reaction entropyFor each chemical reaction listed in the first column of the table below, predict the sign (positive or negative) of the reaction entropyAS If it's not possible to decide with the information given, check the "not enough information" button in the last column.Note for advanced students: Assume the temperature remains constant. Assume all gases and solutions are ideal.reactionN₂(g) + 3H₂(g) →2NH, (e)4Fe()+30.)- 2Fe₂O, (s)N. (3), (g) 2NH, (g)sign of reaction entropy04ronreaction<<050not enough information.45x250<<0not enough information.45050not enough information.Using the general properties of Gibbs free energyThe standard reaction free energy AG" --835. kJ for this reaction:2 Al(s) + Fe₂O3(s)-Al₂O3(s) + 2 Fe(s)Use this information to complete the table below. Round each of your answers to the nearest kJ.BALAKEN F04AGOFocus

Entropy ir the measure of randomness or disorderness in the system. Among the physical states…

For each chemical reaction listed in the first column of the table below, predict the sign (positive or negative) of the reaction entropy AS If it's not possible to decide with the information given, check the "not enough information" button in the last column. Note for advanced students: Assume the temperature remains constant. Assume all gases and solutions are ideal. reaction N. (z)-3H₂(g) → 2NH, (g) 4Fe()+30.(g) 2Fe₂O, (1) N₂ (s) 3₂ (s) 2NH, (g) sign of reaction entropy 45 * 0 0 on rxn <<0 50 not enough information. 45 <0 450 n not enough information, 450 0 not enough information. Using the general properties of Gibbs free energy The standard reaction free energy AG --835. kJ for this reaction: 2Al(s) + Fe₂O3(s)-Al₂O3(s) + 2 Fe(s) Use this information to complete the table hols

For each chemical reaction listed in the first column of the table below, predict the sign (positive or negative) of the reaction entropy AS If it's not possible to decide with the information given, check the "not enough information" button in the last column. Note for advanced students: Assume the temperature remains constant. Assume all gases and solutions are ideal. reaction N. (z)-3H₂(g) → 2NH, (g) 4Fe()+30.(g) 2Fe₂O, (1) N₂ (s) 3₂ (s) 2NH, (g) sign of reaction entropy 45 * 0 0 on rxn <<0 50 not enough information. 45 <0 450 n not enough information, 450 0 not enough information. Using the general properties of Gibbs free energy The standard reaction free energy AG --835. kJ for this reaction: 2Al(s) + Fe₂O3(s)-Al₂O3(s) + 2 Fe(s) Use this information to complete the table hols

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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For each chemical reaction listed in the first column of the table below, predict the sign (positive or negative) of the reaction entropy AS. If it's not possible to decide with the information given, check the "not enough information" button in the last column. rxn Note for advanced students: Assume the temperature remains constant. Assume all gases and solutions are ideal. reaction N₂(g) + 3H₂(g) 2NH₂(g) Ba(OH), 8H₂O(s) + 2NH₂Cl(s) BaCl,(aq) +2NH, (aq) + 10H,O(l) HCl(g) + NH₂(g) NH,C1(s) sign of reaction entropy AS 0 rxn not enough information. AS 0 rxn O not enough information. AS 0 rxn not enough information. S 0
Using the data in the table, calculate the standard entropy changes for the following reactions at 25°C. S(s) + O2(g) → S02(g) Species [J/(mol K)] S(s) 167.83 J/(mol K) O2(g) 205.15 MGCO3(s) → MgO(s) + CO2(g) SO,(g) 248.22 MGCO3(s) 65.7 J/(mol K) MgO(s) 27.0 CO28) 213.78 2 C,H,(g) + 7 O2g)→ 4 CO2(g) + 6 H2O(1) C;Hg) 229.16 J/(mol K) H,0() 69.95
Determine whether the reactions are entropy-favored or disfavored under standard conditions. Predict how a decrease in temperature will affect the value of A,G°. Br2 (g) → 2 Br(g) a Standard entropy for some substance given below. Compound S°, J/K· mol Br2 (g) 245.47 Br(g) 175.022 The reaction is v under standard conditions. With a decrease in temperature, A,G° will b. 2 СО(g) + О:(s) > 2 СО2(g) Standard entropy for some substance given below. Compound S', J/K · mol CO(g) 197.674 CO2(g) 213.74 O2 (g) 205.07 The reaction is v under standard conditions. With a decrease in temperature, A,G° will SiCl, (g) + 2 H20(e) → SiO2 (s) + 4 HCl(g) с. Standard entropy for some substance given below. Compound S°, J/K · mol SİCL, (g) 330.86 H20(e) 69.95 SiO2 (s) 41.46 HCl(g) 186.2 The reaction is V under standard conditions. With a decrease in temperature, A,G° will |
- Chapter 9 and 18 - Thermodynamics Exercise 18.36 Enhanced with Feedback and Hints Without doing any calculations, determine the sign of ASsys for each of the following chemical reactions. Drag the appropriate items to their respective bins. • View Available Hint(s) Reset Help CH4(g) + 202(g)→ CO2(g) + 2H2O(1) 203(g) → 302(g) SO3(g) + H2O(1)→H2SO4(1) Mg(s) + Cl2 (g) → MgCl2 (s) ASsy greater than 0 ASy smaller than 0
Calculate the standard entropy change for the reaction at 25 °C. Standard molar entropy values can be found in this table. HCl(g)+NaOH(s)⟶NaCl(s)+H2O(l) Δ?∘rxn=
For each chemical reaction listed in the first column of the table below, predict the sign (positive or negative) of the reaction entropy A.Sxn If it's not possible to decide with the information given, check the "not enough information" button in the last column. Note for advanced students: Assume the temperature remains constant. Assume all gases and solutions are ideal. reaction H₂O(/) + AL₂ S₂ (s) → H₂S (g) + Al₂O₂ (s) 2C₂H, (g) + 70₂(g) → 4CO₂(g) + 6H₂O(g) BaCl₂ (aq) + K₂SO4 (aq) BaSO₂ (s) + 2K Cl(aq) sign of reaction entropy AS rxn AS rxn not enough information. AS 0 X 0 rxn not enough information. 3
The reaction in (C --> B + A) is favorable at low temperatures only and the reaction in (B + 2C --> D) is favorable at all temperatures. What does this imply for the sign of the entropy change of each reaction? Suggest one possible phase of matter for each of the species (A, B, C, and D) consistent with both of these entropy changes C --> B + A ΔH= -730kJ/mol B + 2C --> D ΔH= -185 kJ/mol
Which of the following results in a decrease in the entropy of the system?A) O2(g), 300 K → O2(g), 400 KB) H2O(s), 0°C → H2O(l), 0°CC) N2(g), 25°C → N2(aq), 25°CD) NH3(l), −34.5°C → NH3(g), −34.5°CE) 2H2O2(g) → 2H2O(g) + O2(g)
Consider the following reaction at constant pressure. Use the information here to determine the value of AS surr at 298 K. Predict whether or not this reaction will be spontaneous at this temperature. N₂(g) +202(g) → 2NO₂(g) AHrxn = +88.4 kJ mol-1 ASsurr = +88.4J K-1 mol-1, reaction is spontaneous Assurr = -88.4J K-1 mol-1, reaction is spontaneous ASsurr = -88.4J K-1 mol-1, reaction is not spontaneous ASsurr = +297 J K-1 mol-1, reaction is spontaneous ⒸASsurr = -297J K-1 mol-1, reaction is not spontaneous
Which reaction is accompanied by an increase in entropy? Ba(OH)2(s) + 2 HCl(g) BaCl₂x2H₂O(s) C12H20()+17 O₂(g) NH4Cl(s) NH3(g) + HCI(g) (CH3)2CO(l) +4Ozg) ® 3CO2g) + 3H2O()) 2 C₂H2(g) + 5O2(g) 4CO2(g) + 2 H₂O(s) 12 CO₂(g) + 10 H₂O()
Which reaction produces a decrease in the entropy of the system? A) 4 NH3(g) + 5 O2 (g) → 4 NO (g) + 6 H2O (g) B) Na (s) + 1/2 Cl2 (g) → NaCl (s) C) 2 HgO (s) → 2 Hg (l) + O2 (g) D) UF6 (s) → U (s) + 3F2 (g) E) H2O (s) → H2O (g)
7.Draw the Lewis structure first, then predict the molecular shape and electron group geometry for each of the following: CS2 H3O+ PBr3 SiCl4