Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Transcribed Image Text:Decomposition of CaCO3 has a AH° = 178.3 kJ/mol and AS° = 159 J/molK. At what
temperature does this become spontaneous?
1121°C
121°C
395°C
848°C
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- Given the particulate models here that depict Cu in solid form, Br2 in liquid form, and He in gaseous form, answer the following questions regarding the changes in entropy. Calculate the change in entropy if Br2(l) is converted into gaseous Br atoms. S° for Br2(l) = 152.2 J/(mol•K)S° for Br2(g) = 245.5 J/(mol•K)S° for Br(g) = 175.0 J/(mol•K)arrow_forwardConsider the following reaction: SO((g) + CaO(s) = CasO4(s). If AGº is -345 kJ/mol for this reaction at 298K, what is the Keg at this temperature? Recall that R is 8.314 J mol-1 K-1. A) 3.1 x 1040 B) 3.50 x 1050 c) 2.96 x 1060 D 2.23 x 1070arrow_forwardPart 1 and part 2 go together For part 2, Then use the data below to calculate ∆G rxn using free energies of formation.arrow_forward
- Given the particulate models here that depict Cu in solid form, Br2 in liquid form, and He in gaseous form, answer the following questions regarding the changes in entropy. Calculate the change in entropy if Br2(l) is converted to Br2(g).S° for Br2(l) = 152.2 J/(mol•K)S° for Br2(g) = 245.5 J/(mol•K)S° for Br(g) = 175.0 J/(mol•K)arrow_forwardDissolution of ionic compounds generally involves an increase in entropy (+ΔS°), but for a few specific metal ions, dissolution of the ionic compound can lead to a decrease in entropy. For example, the dissolution of magnesium chloride (MgCl2) has a ΔS° = -115 J K-1 mol-1. Explain this decrease in entropyarrow_forward50.Calculate ΔΔS° for the following reaction, 2SO2(g) + O2(g) ⟶⟶ 2SO3(g) given S°[SO2(g)] = 248.2 J/mol×K, S°[O2(g)] = 205.1 J/mol×K, and S°[SO3(g)] = 256.8 J/mol×K. a. –196.5 J/K b. –94.0 J/K c. –187.9 J/K d. +187.9 J/K e. +196.5 J/Karrow_forward
- HI has a normal boiling point of –35.4°C, and its DHvapis 21.16 kJ/mol. Calculate the molar entropy of vaporization (DSvap). Be sure to include the correct units with your answer.arrow_forwardUse the AH°f and AHO rxn information provided to calculate AH°f for IF: kJ IF7(g) IF5(g) AHᵒf (kJ/mol) -900. -850. IF7(g) + 12(g) →→ IF5(g) + 2 IF(g) AH rxn = -87arrow_forwardA reaction has a ΔH of -87.36 kJ and a ΔS of -175.3 J/K. At what temperature (in K) does the reaction become spontaneous? 626.4 K This reaction is always spontaneous 498.3 K 434.6 K This reaction is never spontaneousarrow_forward
- (multiple choice question) Using ΔΗΟ and ΔSO for the following reaction: HBr(g) + Cl2(g) ---> HCl(g) + Br2(l) a. Is this is a spontaneous reaction at all temperatures? b. Spontaneous only at low temperatures? or c. Spontaneous only at high temperatures? Explain:arrow_forwardchapter 12: 8) Calculate the free-energy change of the following reaction at 448°C and standard pressure. Values in the table are at standard pressure and 25°C. C2H4(g)+3O2(g)--->2CO2(g)+2H2O(g) ΔHºf,(kJ/mol) Sºf, J/mol•K ΔGºf, kJ/mol C2H4(g) 52.3 219.5 68.1 O2(g) 0 205.0 0 CO2(g) –393.5 213.6 –394.4 H2O(g) –241.8arrow_forward
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