Consider the following reaction at constant pressure. Use the information here to determine thevalue of AS surr at 298 K. Predict whether or not this reaction will be spontaneous at thistemperature.N₂(g) +202(g) → 2NO₂(g) AHrxn = +88.4 kJ mol-1ASsurr = +88.4J K-1 mol-1, reaction is spontaneousAssurr = -88.4J K-1 mol-1, reaction is spontaneousASsurr = -88.4J K-1 mol-1, reaction is not spontaneousASsurr = +297 J K-1 mol-1, reaction is spontaneousⒸASsurr = -297J K-1 mol-1, reaction is not spontaneous

∆Hsurr = - ∆Hrxn ∆S = ∆H/T T = temperature For a spontaneous process: ∆Stotal >0 For a…

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-1¹, 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 O ASsurr = -297 J K-¹ mol-1, reaction is not spontaneous

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-1¹, 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 O ASsurr = -297 J K-¹ mol-1, reaction is not spontaneous

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...

See similar textbooks

Similar questions

Endothermic reactions are more likely to be spontaneous. O True O False
10) Use the Standard Free Energy of Formation values below to calculate Standard Free Energy for the balanced equation: PbCl₂(s) + 2NOF(g) →→→ PbF₂(s) + 2NOCl(g) Substance AGran (kJ/mol) PbCl₂(s) -314.2 NOF(g) -50.29 PbF₂(s) -630.9 NOCI(g) 66.07 Scanned with CamScanner
For a given reaction, dH = 32 kJ/mol and dS = 117 J/mol. At approximately what temperature would this reaction become spontaneous?
For each reaction with ΔH = + 245 kJ/mol and ΔS = + 48 J/molK ,at what temperature at which the reaction will be spontaneous.
For the reaction Fe3O4 (s) + 4H2(g) → 3Fe(s) + 4H₂O(g) AH° = 151 kJ and AS° = 169 J/K The equilibrium constant for this reaction at 342.0 K is Assume that AH° and AS are independent of temperature.
A reaction has values ΔS = 72.3 J K mol-1 and ΔH = 47.0 kJ mol-1. At what temperature (in °C) will this reaction become spontaneous?
39. provide the answer ASap
The law of thermodynamics states that every spontaneous process moves towards greater ontropy. second first O third O fourth
1. On the basis of your experience, predict which of the following reactions are spontaneous. 1) NaCl(s)→→ NaCl(/) at 25 °C 2) 2 NaCl(s)→→ 2 Na(s) + Cl₂(g) 3) CO2(g) → CO2(s) at 25 °C 4) CO2(g) → C(s) + O2(g) 5) H₂O(s)→ H₂O() at 25 °C a) 1, 2, and 3 b) 1, 2, and 4 c) 3 and 5 d) 3 e) 5
Use the standard free energy data to determine the free energy change for the following reactions, which is run under standard state conditions and 25 °C. Identify it as spontaneous or nonspontaneous at this condition. CASO2H;0(s) → CaSOds) + 2H¿O(g) AG (CaSO s)= -1322.0 kJ'mol 40 (HOg)--228.59 kl'mol AG(CasO-H;0,s) =.]797,45 kJ/mol 0 18.3kJ/mol, nonspontaneous 0-18.3kJ/mol, spontaneous 0 156kl/mol, nonspontaneous
Consider the reaction CaCO3(s)- →CaO(s) + CO₂(g) The standard free energy change for this reaction is 130.4 kJ. The free energy change when 1.87 moles of CaCO3(s) react at standard condition is 243.8 kJ. What is the maximum amount of useful work that the reaction of 1.87 moles of CaCO3(s) is capable of producing in surroundings under standard con ions? If no work can be done, enter none. kJ
A 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 spontaneous