The effect of temperature on the reaction rate and safety of the exothermic reaction between sodium hydroxide NaOH and hydrochloric acid HCl can be explained through the collision theory and the concept of activation energy.1. Reaction rate: As the temperature increases, the kinetic energy of the reacting particles NaOH and HCl also increases. This leads to more frequent collisions between the particles, and the collisions are more energetic. As a result, the reaction rate increases with an increase in temperature. This can be described by the Arrhenius equation, which relates the reaction rate constant k to the temperature T and activation energy Ea .2. Safety: The reaction between NaOH and HCl is exothermic, meaning it releases heat. As the temperature increases, the reaction rate increases, and more heat is released in a shorter amount of time. This can lead to a rapid increase in temperature, which may cause the reaction mixture to become too hot to handle safely. Additionally, if the reaction is carried out in a closed system, the rapid release of heat can cause a buildup of pressure, potentially leading to an explosion or rupture of the container.In summary, increasing the temperature of the reaction between sodium hydroxide and hydrochloric acid will increase the reaction rate but can also decrease the safety of the reaction due to the rapid release of heat and potential pressure buildup. It is essential to control the temperature and carry out the reaction in a well-ventilated area with appropriate safety measures in place.