7:32BlackboardXRead Only - Save a copy to edit.Qualitatively predicting reaction entropyreactionFor each chemical reaction listed in the first column of the table below, predict the sign (positive or negative) of the reaction entropyASIxn. 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.N₂(g) + 3H₂(g) → 2NH3(g)4Fe(s) + 30₂(g) → 2Fe₂O3(s)N₂(g) + 3H₂(g)12NH3(g)sign of reaction entropyO ASCalculating dG from dH and dsrxnO not enough information.O ASAS > 0rxnOO ASrxnreaction<0rxn<0> 0O not enough information.AS rxnOASxn> 0< 0O not enough information.Using the general properties of Gibbs free energyThe standard reaction free energy AGO = -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.AGOKJAl₂O3(s) + 2 Fe(s)→2 Al(s) + Fe₂O3(s)Al(s) + — Fe₂O3(s) —— Al₂O3(s)— AL₂O3(s) + — Fe(s)→ =— Al(s) + Fe₂O3(s) kJ.5Gc+ Fe(s)Save a copykJ= 7:32BlackboardXRead Only - Save a copy to edit.Calculating dG from dH and dSA chemical engineer is studying the two reactions shown in the table below.In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 130.0 °C andconstant total pressure. Then, he measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reactionenthalpy AH and reaction free energy AG of the second reaction. The results of his measurements are shown in the table.Al₂O3(s) + 2Fe(s) → 2Al(s) + Fe₂O₂ (s)Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.)Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous,or neither forward nor reverse reaction is spontaneous because the system is at equilibrium.CO₂(g) + 2H₂O(g) CH₂(g) + 20₂(g)AH = 852. kJAS = 2044.AG = || kJ- 0²/2KAS =AGWhich is spontaneous?this reactionthe reverse reactionneitherAH = 803. kJ5GcK=Save a copy-27. kJWhich is spontaneous?this reactionthe reverse reactionneither||

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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. Note for advanced students: Assume the temperature remains constant. Assume all gases and solutions are ideal. rxn' reaction N₂(g) + 3H₂(g) 2NH3(g) 4Fe(s) + 30₂(g) → 2Fe₂O₂ (s) N₂(g) + 3H₂(g) 2NH₂(g) sign of reaction entropy OASxn O AS >0 rxn <0 O not enough information. O AS Srxn <0 O AS > 0 rxn O not enough information. OASxn O AS >0 rxn <0 O not enough information.

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. rxn' reaction N₂(g) + 3H₂(g) 2NH3(g) 4Fe(s) + 30₂(g) → 2Fe₂O₂ (s) N₂(g) + 3H₂(g) 2NH₂(g) sign of reaction entropy OASxn O AS >0 rxn <0 O not enough information. O AS Srxn <0 O AS > 0 rxn O not enough information. OASxn O AS >0 rxn <0 O not enough information.

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 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
For which of the following reactions is there an increase in entropy? I. CO2 (g) → CO2 (s) II. 2 NH3 (g) → N2 (g) + 3 H2 (g) III. 2 NO2 (g) → N2O4 (g)
1. Ammonia can be made from the reaction of nitrogen and hydrogen: N2 (g) + 3 H2 (g) ⟺ 2 NH3 (g) For this reaction, K = 1.6 x 102 and ΔH = -91.8 kcal/mole at 25oC. Is the reaction endothermic or exothermic? Briefly explain. Is there in increase in entropy, a decrease in entropy, or no change in entropy? Briefly explain. At 25oC, is this reaction product favored or reactant favored? Briefly explain. Do you expect this reaction to be spontaneous at all temperatures? Briefly explain.
Which of the following processes shows an increase in entropy of the system? 2NO₂(g) → 2NO(g) + O₂(g) CO(g) + Cl₂(g) → COCI₂(g) CO(g) + 2H₂(g) → CH₂OH(I) Na+ (aq) + CIO3(aq) → NaClO3(s)
For each of the following reactions determine if the change in entropy was positive or negative:A) Water at 40°C → Water at 25°CB) 2NO2(g) → N2O4(g)C) CH3OH (l) → CH3OH (g)D) PbCl2(s) → PbCl2(aq)
By examining the following graphs, predict which element- copper or gold-has the higher absolute entropy at a tem- perature of 200 K. 0.3 0.2 Au Cu 0.1 100 200 300 Temperature (K) 7U mol-! K-2)
< 8:41 1 4 7 +/- Question 1 of 17 When heated, CaCO3 decomposes into CaO and CO₂ according to the following equation: CaCO3(s) CaO(s) + CO₂(g) This is an endothermic reaction in which AH° = 178.3 kJ/mol and in which entropy increases, AS° = 159 J/mol K. To what temperature (in °C) must CaCO3 be heated in a closed container in order to produce CO₂ at an equilibrium pressure of 0.250 atm? (Assume AH° and AS° do not change appreciably with temperature). 2 5 8 °C 3 60 9 O Submit Tap here or pull up for additional resources XU x 100
For the following reactions, indicate whether the entropy of the system increases, decreases, or remains nearly the same. a. Al3+(aq) + 3 OH-(aq) → Al(OH)3(s)b. CaCO3(s) → CaO(s) + CO2(g)c. Mg(s) + Cu2+(aq) → Mg2+(aq) + Cu(s)
Does the entropy increase or decrease in these reactions? Why? a) 4 Al + 3 O2 → 2 Al2O3 b) C + 2 Cl2 → CCl4 c) H2O (l) → H2O (g) d) CCl4 → C + 2 Cl2
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 &
O ENTROPY AND FREE ENERGY Using reaction free energy to predict equilibrium composition D 3/5 Consider the following equilibrium: 2NOC1 (g) - 2NO (g)+ Cl, (g) AG" =41. kJ Now suppose a reaction vessel is filled with 2.68 atm of nitrosyl chloride (NOCI) and 3.74 atm of chlorine (Cl,) at 227. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of Cl, tend to rise or fall? fall Is it possible to reverse this tendency by adding NO? In other words, if you said the pressure of Cl, will tend to rise, can that yes be changed to a tendency to fall by adding NO? Similarly, if you said the no pressure of Cl, will tend to fall, can that be changed to a tendency to rise by adding NO? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO needed to reverse it. | atm Round your answer to 2 significant digits. II
Which one of the following choices of gaseous molecules is rank ordered correctly from lowest standard molar entropy (left hand side) to highest standard molar entropy (right hand side)? He, Ne, CO, SiH4 SiH4 , CO, Ne, He SiH4 , Ne, CO, He CO, SiH4 , Ne, He