For the process: Z₂(g) →2 Z(g), AH° = +478 kJ.What would be predicted for the sign of ASxn and theconditions under which this reaction would be spontaneous?A.B.C.D.ASTXBpositivepositivenegativenegativeSpontaneousat low temperatures onlyat high temperatures onlyat high temperatures onlyat low temperatures only

Given reaction: Z2(g) → 2Z(g), ∆H∘ = +478 kJ We have to find the sign of ∆Srxn and the…

For the process: Z₂(g) →2 Z(g), AH° = +478 kJ. What would be predicted for the sign of ASxn and the conditions under which this reaction would be spontaneous? A. B. C. D. ASrxn positive positive negative negative Spontaneous at low temperatures only at high temperatures only at high temperatures only at low temperatures only

For the process: Z₂(g) →2 Z(g), AH° = +478 kJ. What would be predicted for the sign of ASxn and the conditions under which this reaction would be spontaneous? A. B. C. D. ASrxn positive positive negative negative Spontaneous at low temperatures only at high temperatures only at high temperatures only at low temperatures only

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 a given reaction, ΔH = +35.5 kJ/mol and ΔS = +83.6 J/mol·K. Which of the following is TRUE? a. The reaction is spontaneous at standard conditions. b. The reaction is spontaneous at T > 425 K. c. The reaction is spontaneous at all temperatures. d. The reaction is spontaneous at T < 425 K.
1. Find DHrxn, DSrxn, and DGrxn, using the tables at the end of your textbook for the phase change of water from liquid to gas at 25.0°C. H2O (l) <---> H2O (g) 2. Is this phase change spontaneous at 25.0°C? Give the reason for your answer. 3. Find the temperature at which this phase change becomes spontaneous. Give in both K and ℃. 4. Is this what you expect, and why? (Is the answer to question #3 what you expect)
The following reaction is endothermic. 2NH3(g) → N2(g) + 3H2(g) This means the reaction A. will be spontaneous at high temperatures. B. will be spontaneous at low temperatures. C. is not spontaneous at any temperature. D. is spontaneous at all temperatures.
Use the observations about each chemical reaction in the table below to decide the sign (positive or negative) of the reaction enthalpy AH and reaction entropy AS. Note: if you have not been given enough information to decide a sign, select the "unknown" option. reaction A B с observations Crystallization of a pure compound is spontaneous only below 23. °C. This reaction is spontaneous only above 31. °C but proceeds at a faster rate above 83. °C. The reverse of this reaction is always spontaneous but proceeds faster at temperatures above 108. °C. AH is AS is AH is AS is conclusions ΔΗ is AS is (pick one) (pick one) (pick one) (pick one) (pick one) (pick one) V
The following reaction takes place at 120°C: H20( I) → H20( g) AH 44.0 kJ/ mol AS = 0.119 kJ/mol K Which of the following must be true? O a. The reaction is not spontaneous. b. The reaction is spontaneous. O c. AG = 0 O d. AG <0 O e. Two of these.
If the process is exothermic and not spontaneous, then what must be TRUE? O a. AS0 O c. AH=0 O d. AS> 0
For each reaction, calculate ΔH°rxn, ΔS°rxn, and ΔG°rxn at 25 °C and 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?a. 2 CH4( g)------->C2H6( g) + H2( g)b. 2 NH3( g)------> N2H4( g) + H2( g)c. N2( g) + O2( g)-------->2 NO( g)d. 2 KClO3(s)-------->2 KCl(s) + 3 O2( g)
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At what temperatures will a reaction be spontaneous if AH = +158 kJ and AS = +411 %3D J/K? O The reaction will never be spontaneous. O The reaction will be spontaneous at any temperature. O All temperatures above 384 K O All temperatures below 384 K