Answer:
Option D. 1191.49 K
Explanation:
The following data were obtained from the question:
Change in enthalphy (ΔH) = 280 kJ/mol
Change in entropy (ΔS) = +235 J/Kmol
Temperature (T) =...?
Next, we shall express the enthalphy in joule (J). This is illustrated below:
1 KJ/mol = 1000 J/mol
Therefore, 280 kJ/mol = 280 x 1000 = 280000 J/mol
Therefore, 280 KJ/mol is equivalent to 280000 J/mol
Now, we can obtain the temperature at which the reaction was feasible as follow:
ΔS = ΔH/T
235 = 280000/ T
Cross multiply
235 x T = 280000
Divide both side by 235
T = 280000/235
T = 1191.49 K
Therefore, the temperature at which the reaction was feasible is 1191.49 K
