Consider the reaction :
`2H_(2) (g) + O_(2) (g) hArr2H_(2)O (g)`
When hyudrogen is ignited in the presence of oxygen, a lot of heat is released and water is produced. At room temperature, the `DeltaH_(r xx n)^(@)` is about `-484 k J//mol` and `Delta S_(r xx n)^(@)` is about -87 kJ/mol. Given this data how would you interpet this thermodynamic process ? Select the correct answer:

Options

A. The reaction is exothermic (heat is released) and it is becoming more ordered
B. The reaction is endothermic (heat is absorbed) and it is becoming more disorderde
C. The reaction is exothermic (heat is released) and it is becoming more disordered
D. the reaction is endothermic (heat is absorbed) and it is becoming more ordered.

Answer

A

Explanation

`Delta H^(@) = -484 kJ`/mol indicates exothermic nature of reaction while `Delta S^(@) = - 87 J//K (lt 0)` indicates that the system is becoming more ordered