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For a given reaction, ΔH = 35.5 kJ mol–1 and ΔS = 83.6 JK–1 mol–1. The reaction is spontaneous at (Assume that ΔH and ΔS do not vary with temperature):
  • a)
    T > 425 K
  • b)
    All temperature
  • c)
    T > 298 K
  • d)
    T < 425 K
Correct answer is option 'A'. Can you explain this answer?
Most Upvoted Answer
For a given reaction, ΔH = 35.5 kJ mol–1 and ΔS = 83...
Solution:- (A) 
T>425K
The reaction is 
{spontaneousif ΔG<0non-spontaneousif ΔG>0
As we know that,
ΔG=ΔHTΔS
 The reaction is spontaneous.
ΔG<0
ΔHTΔS<0
T>ΔHΔS
Given:-
ΔH=35.5KJ/mol=35500J/mol
ΔS=83.6J/molK
T>3550083.6
T>425K
Hence the reaction will be spontaneous at 
T>425K
.
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For a given reaction, ΔH = 35.5 kJ mol–1 and ΔS = 83.6 JK–1 mol–1. The reaction is spontaneous at (Assume that ΔH and ΔS do not vary with temperature):a)T > 425 Kb)All temperaturec)T > 298 Kd)T < 425 KCorrect answer is option 'A'. Can you explain this answer?
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