Question

a. calculate \\( \delta t \\) and show your work.
b. is the reaction endothermic or exothermic?

Explanation:

Step1: Calculate ΔT

ΔT is calculated as \( T_{final}-T_{initial}\). From the table, \(T_{initial} = 24.6^{\circ}C\) and \(T_{final}=18.2^{\circ}C\).

$$ \Delta T=18.2 - 24.6=- 6.4^{\circ}C $$

Step2: Determine reaction type

In an endothermic reaction, the system absorbs heat, causing the temperature of the surroundings (in this case, the reaction mixture) to decrease. In an exothermic reaction, the system releases heat, causing the temperature of the surroundings to increase.
Since \(\Delta T=-6.4^{\circ}C\) (temperature decreased), the reaction is endothermic.

Answer:

a. \(\Delta T = - 6.4^{\circ}C\)
b. The reaction is endothermic.