8. Thermochemistry
Endothermic & Exothermic Reactions
8. Thermochemistry Endothermic & Exothermic Reactions
31PRACTICE PROBLEM
Sulfur dioxide gas can be produced by heating up solid sodium sulfite.
Na2SO3(s) → Na2O(s) + SO2(g) ΔH = −697 kJ/mol
When heated, Na2SO3 decomposes spontaneously. Is the reverse reaction, the formation of Na2SO3 from Na2O and SO2, spontaneous under normal conditions? Please explain.
Sulfur dioxide gas can be produced by heating up solid sodium sulfite.
Na2SO3(s) → Na2O(s) + SO2(g) ΔH = −697 kJ/mol
When heated, Na2SO3 decomposes spontaneously. Is the reverse reaction, the formation of Na2SO3 from Na2O and SO2, spontaneous under normal conditions? Please explain.