The reaction is spontaneous at a temperature of 7281.4 K
As the value of temperature rises, it is decreasing in accordance with the value of ΔG°, according to the value ofΔG° calculated. The value shifts from being more positive to being less positive. It ΔG°at a certain temperature.
It would appear that the value of would be negative, causing the reaction to occur on its own.
The calculation shown below can be used to determine the temperature at which the reaction starts spontaneously.
ΔG°= ΔH°-TΔS°
ΔG° now equals zero.
0 = 180.58 - T 24.8(1/1000)
T= 180.58/0.0248 K
T=7281.4 K
therefore, the reaction is spontaneous at a temperature of 7281.4 K
Learn more about ΔG° here:
brainly.com/question/17214066
#SPJ4
