Consider a reaction for which ΔH = 6.03 kJ/mol; ΔS = 22.1 J/K-mol. Which of the following statements is true?
a. The reaction becomes spontaneous at high temperatures above 273 K
b. The reaction becomes spontaneous at low temperatures below 273 K
c. The reaction is spontaneous at all temperatures
d. The reaction is never spontaneous
Reaction becomes spontaneous when
In our case change in entropy is already > 0. Now for Change in Gibb's free energy to be less than zero,
Substitute values,
6.03 * 1000 < T*22.1
Therefore T > 273 K. For temperatures greater than 273 K, reaction becomes spontaneous.
Answer would be (a)
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