Asked by Jeff
Consider the following reaction at constant P. Use the information here to determine the value of ΔSsurr at 398 K. Predict whether or not this reaction will be spontaneous at this temperature.
4 NH3(g) + 3 O2(g) → 2 N2(g) + 6 H2O(g); ΔH = -1267 kJ
A)ΔSsurr = +3.18 kJ/K, reaction is spontaneous
B)ΔSsurr = -12.67 kJ/K, reaction is spontaneous
C)ΔSsurr = +12.67 kJ/K, reaction is not spontaneous
D)ΔSsurr = +50.4 kJ/K, reaction is not spontaneous
E)ΔSsurr = -3.18 kJ/K, it is not possible to predict the spontaneity of this reaction without more information.
4 NH3(g) + 3 O2(g) → 2 N2(g) + 6 H2O(g); ΔH = -1267 kJ
A)ΔSsurr = +3.18 kJ/K, reaction is spontaneous
B)ΔSsurr = -12.67 kJ/K, reaction is spontaneous
C)ΔSsurr = +12.67 kJ/K, reaction is not spontaneous
D)ΔSsurr = +50.4 kJ/K, reaction is not spontaneous
E)ΔSsurr = -3.18 kJ/K, it is not possible to predict the spontaneity of this reaction without more information.
Answers
Answered by
DrBob222
dHsurr = -dH/T
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