To determine the nature of the reaction given the enthalpy change [tex]\( \Delta H \)[/tex], we should examine the sign and magnitude of [tex]\( \Delta H \)[/tex].
The enthalpy change ([tex]\( \Delta H \)[/tex]) for a reaction tells us whether the reaction absorbs or releases heat:
1. Positive [tex]\(\Delta H\)[/tex]: If the enthalpy change is positive, the reaction absorbs heat from its surroundings, indicating that it is an endothermic reaction.
2. Negative [tex]\(\Delta H\)[/tex]: If the enthalpy change is negative, the reaction releases heat to its surroundings, indicating that it is an exothermic reaction.
In this problem, the enthalpy change ([tex]\( \Delta H \)[/tex]) is given as 16.71. Since this value is positive, it means that the reaction absorbs heat. Therefore, this reaction is an endothermic reaction.
Now, let's analyze the options:
- A. The reaction is exothermic.
- This is incorrect because an exothermic reaction would have a negative [tex]\( \Delta H \)[/tex].
- B. The reaction produces heat.
- This is also incorrect because producing heat would mean the reaction releases heat, which would correspond to an exothermic reaction with a negative [tex]\( \Delta H \)[/tex].
- C. The reaction is endothermic.
- This is correct because a positive [tex]\( \Delta H \)[/tex] indicates that the reaction absorbs heat and is endothermic.
- D. The reaction cannot happen.
- This is incorrect because the possibility of the reaction occurring is not determined solely by [tex]\( \Delta H \)[/tex]. Moreover, [tex]\( \Delta H \)[/tex] being positive simply indicates that the reaction requires heat, not that it cannot occur.
Therefore, the correct answer is:
C. The reaction is endothermic.
