Review I CoPart AMISSED THIS? Read Section 19.6(Papes 863 - 867): Watch KCV 19.6. IWE 19.4.AH =-98 kJ, AS-145 J/K, T = 297 KCalculate the change in Gibbs free energy for eachof the following seots of AH, ASn, and T.(Assume that all reactants and products are in theirstandard states.)Express your answer as an integer.AG =kJSubmitRequest AnswerPart BAHan =-98 kJ, ASan =-145 J/K, T = 850 KExpress your answer as an integer.AGkJ Part CMISSED THIS? Read Section 19.6(Pages 863-867): Watch KCV 19.6, IWE 19.4.AH = 98 kJ, AS=-145 J/K, T = 297 KExpress your answer as an integer.Calculate the change in Gibbs free energy for eachof the following sets of AHn ASan, and T.(Assume that all reactants and products are in theirstandard states.)?AGn =kJSubmitRequest AnswerPart DAHan = -98 kJ, ASi = 145 J/K, T = 408 KExpress your answer as an integer.AGan =kJSubmitRequest AnswerPart E Complete previous part(s)

Answered: Image /qna-images/answer/d55f2c4c-ec4f-42c1-ab6a-57ac3203d9ba.jpg

Part A THIS? Read Section 19.6 53-867): Watch KCV 19.6. IWE 19.4 AH--98 kJ, ASi-145 J/K, T- 207 K Express your answer as an integer. the change in Gibbs free energy for each owing sets of A H ASa, and T. that all reactants and products are in their states.) AG i- kJ Submit Request Answer Part B AHan =-98 kJ, AS -145 J/K, T= 850K Express your answer as an integer.

Part A THIS? Read Section 19.6 53-867): Watch KCV 19.6. IWE 19.4 AH--98 kJ, ASi-145 J/K, T- 207 K Express your answer as an integer. the change in Gibbs free energy for each owing sets of A H ASa, and T. that all reactants and products are in their states.) AG i- kJ Submit Request Answer Part B AHan =-98 kJ, AS -145 J/K, T= 850K Express your answer as an integer.

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 the reaction N₂ (g) + 2O2(g) → 2NO2(g) - 122 J/K AH° = 66.4 kJ and AS = The equilibrium constant for this reaction at 343.0 K is Assume that AH° and AS are independent of temperature.
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Table 2. Gibbs Free Energies of formation (kJ), ∆G°f, for Ions in 1M Solution and Ionic Solids Cations Cl--131.228 I--51.57 NO3--108.74 SO4-2-744.53 Ca2+-553.58 -748.1 -528.9 -743.07 -1797.28 W2 ∆G°f of water = -237.129 kJ/mol Calculated values of ∆G°rxn and the ∆Grxn of each box, Predicted results (ppt or no ppt).Observations (Rxn or No Rxn). S or support and R for Refute Cations Cl- I- NO3- SO4-2 Ca+2 help
Chp 19 #19
Discuss the spontaneity of each process in the following scenarios, based on the use of the Gibbs free energy equation: 1. N₂(g) + 3H₂(g) + 2NH3(g), AH = -46.11 kJ/mol 2. An exothermic reaction with an increase in entropy 3. A block of solid carbon dioxide subliming to gaseous carbon dioxide
E The Carnot cycle, which is a particular example of a thermodynamic cycle, allows determining the efficiency of a "heat-to-work" engine. Clausius used this to find the macroscopic definition of entropy as the heat change of the system at a particular temperature. Th and T are the high and low qh and q for the heats transferred at these temperatures. When plotted in a T-S temperatures and representation, entropy only changes in the processes (steps) where heat is added or removed. However, when plotting the Carnot cycle in the P-V representation it is clear that work is done (on or by) the system in each of the 4 processes of the cycle. a) Give the names of the 2 processes of the Carnot cycle (an engine) in which the surroundings do work on the system. Indicate the condition(s) of the walls for these processes. b) Consider the microscopic, i.e., Boltzmann's, definition of entropy for an ideal gas. Briefly discuss what needs to be satisfied so that there is no change of entropy during a…
Mark the correct statements. (Select all that apply.) O [The reaction 2H20(g) → 2H2(g) + O2(g) is expected to have a positive value of ASº.] O [If a sample of pure ozone changed to oxygen at constant T and P, the entropy of the sample would decrease.] O [For the process H20(1) → H20(s) occurring at 0°C and 1 atm, the sign of AS is negative.] O [The value of AS for the process CHC13(1) – CHC13(g) is negative.] O [The reaction CH4(g) + 202(g) → CO2(g) + 2H2O(g) has a negative value of ASsurr-]
A chem.. ngineer 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 52.0 °C and constant total pressure. Then, he measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of his measurements are shown in the table. 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. AH = 181. kJ J AS = 557. K N, (g) + 0, (g) → 2NO (g) AG = N, (g) + 0,(8) kJ Which is spontaneous? this reaction the reverse reaction neither ΔΗ - - 1353. kJ J AS = K 2CH,OH (g) + 30,(g)…
For the reaction NH4NO3(aq) 1 N₂O(g) + 2 H₂0 (1) AG° -179.4 kJ and AH = -149.6 kJ at 298 K and 1 atm. This reaction is (reactant, product) favored under standard conditions at 298 K. The entropy change for the reaction of 1.51 moles of NH4NO3(aq) at this temperature would be J/K.
1 3. Determine AS (in J K-¹ to the nearest whole number) for a system composed of 85.0 g of water that evaporates from a liquid to a gas at the normal boiling point of water. Additionally, what is AS if you evaporated twice this amount of water? (AHcondensation (H₂O) = −40.7 kJ mol−¹ ) A: 515; 1030 2-0 Ł p X-90.7) 5
Try Again Your answer is wrong. • Second reaction: Your answer for A Sis incorrect. A 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 88.0 °C and constant total pressure. Then, he measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of his measurements are shown in the table. 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. 2Fe₂O3(s) 4Fe(s) + 30₂ (g) ΔΗ = 1648. kJ AS = 4631. AG = J K -24 kJ Which is spontaneous? this…
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