The reaction starts spontaneously at 411 K.
As the temperature rises, ΔG° value decreases. The value switches from being positive to being negative. The reaction's spontaneity shifts from non spontaneous to spontaneous.
The formula ΔG°, as shown below, can be used to determine the temperature at which the reaction becomes spontaneous.
Here ΔG° turns into zero.
ΔG°=ΔH°-TΔS°
0= 90.7 kJ/mol-T(220.7J/mol.K)(1kJ/1000J)
T=90.7/0.2207K
T=411 K
As a result, the reaction starts spontaneously at 411 K.
Learn more about ΔG° here:
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