Consider the reaction below at constant pressure.Use the information provided to determine the value of ASsurr at 398 K, and predict whether or not thisreaction will be spontaneous at this temperature.4NH3(g) + 302(g) → 2N2(g) + 6H20(g)AH°rxn = -1267 kJ%3DASsurr = +12.67 kJ/K, reaction is spontaneousASsurr = +3.18 kJ/K, reaction is spontaneousASsurr = -12.67 kJ/K, reaction is spontaneousASsurr = +3.18 kJ/K, it is not possible to predict the spontaneity of this reaction without more information.

If delta S surrounding is positive then reaction will be spontaneous.

Consider the reaction below at constant pressure. Use the information provided to determine the value of ASsurr at 398 K, and predict whether or not this reaction will be spontaneous at this temperature. 4NH3(g) + 302(g) → 2N2(g) + 6H20(g) AH°rxn = -1267 kJ ASsurr = +12.67 kJ/K, reaction is spontaneous ASsurr = +3.18 kJ/K, reaction is spontaneous ASsurr = -12.67 kJ/K, reaction is spontaneous O ASsurr = +3.18 kJ/K, it is not possible to predict the spontaneity of this reaction without more information.

Consider the reaction below at constant pressure. Use the information provided to determine the value of ASsurr at 398 K, and predict whether or not this reaction will be spontaneous at this temperature. 4NH3(g) + 302(g) → 2N2(g) + 6H20(g) AH°rxn = -1267 kJ ASsurr = +12.67 kJ/K, reaction is spontaneous ASsurr = +3.18 kJ/K, reaction is spontaneous ASsurr = -12.67 kJ/K, reaction is spontaneous O ASsurr = +3.18 kJ/K, it is not possible to predict the spontaneity of this reaction without more 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...

See similar textbooks

Similar questions

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
For a particular reaction, AH° = -93.8 kJ and AS° = –156.1 J/K. Assuming these values change very little with temperature, at what temperature does the reaction change from nonspontaneous to spontaneous? T = K Is the reaction in the forward direction spontaneous at temperatures greater than or less than the calculated temperature? less than greater than
A reaction has values ΔS = 60.3 J K-1 mol-1 and ΔH = 49.6 kJ mol-1. At what temperature (in °C) will 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.
A reaction has values ΔS = 60.3 J K-1 mol-1 and ΔH = 44.7 kJ mol-1. At what temperature (in °C) will this reaction become spontaneous?
Given the values of AH, ASn, and T, determine ASuniy and predict whether or not each reaction is spontaneous. (Assume that all reactants and products are in their standard states.) a. AH = -95 kJ; AS;n = -157 J/K; T = 298 K b. AH = -95 kJ; AS"n = -157 J/K; T = 855 K Calculate the Gibbs free energy for the above sets (a) and (b)
For each of the following reactions, calculate ΔH∘rxn, ΔS∘rxn, and ΔG∘rxn at 25 ∘C. State whether or not the reaction is spontaneous. If the reaction is not spontaneous, would a change in temperature make it spontaneous? If so, should the temperature be raised or lowered from 25 ∘C?2CH4(g)→C2H6(g)+H2(g), Calculate ΔS∘rxn at 25 ∘C. 2NH3(g)→N2H4(g)+H2(g) Calculate ΔS∘rxn at 25 ∘C. N2(g)+O2(g)→2NO(g) Calculate ΔS∘rxn at 25 ∘C. 2KClO3(s)→2KCl(s)+3O2(g) Calculate ΔS∘rxn at 25 ∘C.
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?
For a particular chemical reaction H = 6.8 kJ and S = –29 J/K. Under what temperature condition is the reaction spontaneous?
Consider the reaction below for the decomposition of carbon tetrachloride gas: CCl4(g) ------> C(s) + 2Cl2 (g) ΔH = + 95.7 kJ; ΔS = + 142.2 J/K If the reaction above is not spontaneous at 25 oC, determine at what temperature (if any) the reaction becomes spontaneous.
The vaporization of compound A is described by the following chemical equation. A(1) A(g) AH vap (78.97 °C) = 37.87 kJ/mol Calculate the entropy of vaporization, A.Svap, for A(1) at 25.0 °C given that the boiling point of A is 78.97 °C, and the molar heat capacity of A(1) is 114.29 J/(mol K). Assume that the molar heat capacity of A(g) is 55.9% of that of A(1). ASvap = Calculate the standard enthalpy of vaporization, AHvap, for A(1) at 25.0 °C. AH vap = Calculate tl AG'vap = x10 TOOLS of vaporization, AGvap, at 25.0 °C. Determine the equilibrium constant K for the va 1970ea J. mol-1. K-1 kJ/mol kJ/mol
A reaction has AH°= 100 kJ/mol and AS°= 250 J/mol.K. Is the reaction spontaneous at room temperature? If not, under what temperature conditions will it become spontaneous?