At which temperature would a reaction with H -220 kJmol and S -0.05 kJ(molK) be spontaneous?

To determine the temperature at which the reaction becomes spontaneous, we can use the Gibbs free energy equation: ΔG = ΔH - TΔS. A reaction is spontaneous when ΔG is less than 0. Given ΔH = -220 kJ/mol and ΔS = -0.05 kJ/(mol·K), we set up the inequality: -220 kJ/mol - T(-0.05 kJ/(mol·K)) < 0. Solving for T gives T > 4400 K, meaning the reaction will be spontaneous at temperatures above 4400 K.