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First up, we have **temperature**. Temperature is a big one. Generally, as temperature increases, the reaction rate increases. This is because higher temperatures provide reactant molecules with more kinetic energy, making them more likely to collide with enough energy to overcome the activation energy barrier. The relationship between temperature and reaction rate is described by the Arrhenius equation. This equation shows that the rate constant (k) increases exponentially with temperature. Therefore, the **reaction order** itself isn't directly affected by temperature, but the rate constant and the rate of the reaction are. So, changes in temperature can affect the *speed* of the reaction, but the reaction order (how the rate changes with concentration) generally stays the same.
