Question

question 2
is this reaction mostly likely endothermic or exothermic? why?

Explanation:

To determine if a reaction is endothermic or exothermic, we analyze the energy change. In an endothermic reaction, the products have more energy than the reactants (energy is absorbed). In an exothermic reaction, products have less energy (energy is released). The graph (likely a heating/cooling or energy - reaction progress graph) here shows that as the reaction progresses, the energy (y - axis, assuming temperature or energy) increases. This indicates the system is absorbing energy, so it's endothermic. The key is comparing reactant and product energy: if product energy > reactant energy, endothermic (energy absorbed from surroundings).

Answer:

This reaction is mostly likely endothermic. Because in an endothermic reaction, energy is absorbed, and the graph (showing the change in a property like temperature or energy over the reaction process) indicates that the energy of the system increases (e.g., if it's a temperature - time or energy - reaction progress graph, the final state has higher energy than the initial state), meaning the reaction absorbs energy from the surroundings.