Final answer:
Increasing temperature will decrease the reaction time by making collisions between reactants more frequent and energetic, allowing them to overcome the activation energy barrier more easily.
Step-by-step explanation:
Increasing temperature will decrease the time of a reaction. Raising the temperature of a chemical reaction significantly affects the reaction rate. Particles of reactants move more rapidly when heated, leading to an increased frequency of collisions. Moreover, the collisions become more forceful, surmounting the activation energy barrier more effectively and forming products at a higher rate.
According to LibreTexts™, a 10 °C increase in temperature generally doubles the rate of a chemical reaction, meaning reactions occur faster at higher temperatures. For enzyme-catalyzed reactions, there is an optimum temperature around body temperature, beyond which the rate can start to decline. In thermodynamic terms, an increase in temperature can shift chemical equilibria, changing the concentrations of reactants and products as the system adjusts to minimize the free energy change, according to Le Châtelier's Principle.
Overall, increasing temperature generally accelerates reactions by increasing effective collisions between reacting particles, thus reducing the reaction time.