Consider the following reaction; use the information here to determine the value of #\DeltaS_(surr)# at 398 K ... Will this reaction be spontaneous at this temperature?
"Predict whether or not this reaction will be spontaneous at this temperature"
#4NH_3# (g) + #3O_2# (g) #rarr2N_2# (g) + #6H_2O# (g)
#\DeltaH=-1267# kJ
A) #\DeltaS_(surr)# =+12.67 kJ/K, rxn not spontaneous
B) #\DeltaS_(surr)# = -12.67 kJ/K, rxn spontaneous
C) #\DeltaS_(surr)# = +50.4 kJ/K, rxn not spontaneous
D) #\DeltaS_(surr)# = +3.18 KJ/K, rxn spontanous
E) #\DeltaS_(surr)# -3.18 kJ/K, it is not possible to predict the spontaneity of this rxn without more information
"Predict whether or not this reaction will be spontaneous at this temperature"
A)
B)
C)
D)
E)
2 Answers
C)
Explanation:
This is what I got based off of class notes...
as
The correct answer is D)
Explanation:
For a reaction to be spontaneous, we must have
The sign of
Thus, the sign of