The enthalpy change of formation reaction of the \%N\%\|phenyl\|\%N\%\+′\|(1,2,3\|thiadiazol\|5\|yl)urea has been determined by a microcalorimeter, using 5\|amino\|1,2,3\|thiadiazole and phenylisocyanate as starting ...The enthalpy change of formation reaction of the \%N\%\|phenyl\|\%N\%\+′\|(1,2,3\|thiadiazol\|5\|yl)urea has been determined by a microcalorimeter, using 5\|amino\|1,2,3\|thiadiazole and phenylisocyanate as starting materials in the solvent of THF. The reaction temperature was kept at 25 ℃. On the basis of experimental and calculated results, the enthalpy change is Δ\-r\%H\%\+\{o-\}\-m=(-142.304±0.390) kJ·mol\+\{-1\}; the reaction order is \%n\%=1/2; the rate constant \%k\%=1.357 9×10\+\{-4\} s\+\{-1\} and the activation free\|energy is Δ\%G\%\+\{o-\}\-m=95.098 \{kJ·mol\+\{-1\}\}. The result indicates that the title reaction takes place easily at room temperature.展开更多
文摘The enthalpy change of formation reaction of the \%N\%\|phenyl\|\%N\%\+′\|(1,2,3\|thiadiazol\|5\|yl)urea has been determined by a microcalorimeter, using 5\|amino\|1,2,3\|thiadiazole and phenylisocyanate as starting materials in the solvent of THF. The reaction temperature was kept at 25 ℃. On the basis of experimental and calculated results, the enthalpy change is Δ\-r\%H\%\+\{o-\}\-m=(-142.304±0.390) kJ·mol\+\{-1\}; the reaction order is \%n\%=1/2; the rate constant \%k\%=1.357 9×10\+\{-4\} s\+\{-1\} and the activation free\|energy is Δ\%G\%\+\{o-\}\-m=95.098 \{kJ·mol\+\{-1\}\}. The result indicates that the title reaction takes place easily at room temperature.
