Editing Reaction rate (section)

==Influencing factors==
Factors that influence the reaction rate are the nature of the reaction, concentration, [[pressure]], [[Order (chemistry)|reaction order]], [[temperature]], [[solvent]], [[electromagnetic radiation]], catalyst, [[isotope]]s, surface area, [[Mixing (process engineering)|stirring]], and [[diffusion limit]]. Some reactions are naturally faster than others. The number of reacting species, their [[Phase (matter)|physical state]] (the particles that form solids move much more slowly than those of gases or those in [[Solution (chemistry)|solution]]), the complexity of the reaction and other factors can greatly influence the rate of a reaction.

Reaction rate increases with concentration, as described by the [[rate law]] and explained by [[collision theory]]. As reactant concentration increases, the [[frequency]] of [[collision]] increases. The rate of gaseous reactions increases with pressure, which is, in fact, equivalent to an increase in the concentration of the gas. The reaction rate increases in the direction where there are fewer moles of gas and decreases in the reverse direction. For condensed-phase reactions, the pressure dependence is weak.

The order of the reaction controls how the reactant concentration (or pressure) affects the reaction rate.

Usually conducting a reaction at a higher temperature delivers more energy into the system and increases the reaction rate by causing more collisions between particles, as explained by collision theory. However, the main reason that temperature increases the rate of reaction is that more of the colliding particles will have the necessary activation energy resulting in more successful collisions (when bonds are formed between reactants). The influence of temperature is described by the [[Arrhenius equation]]. For example, coal burns in a fireplace in the presence of oxygen, but it does not when it is stored at [[room temperature]]. The reaction is spontaneous at low and high temperatures but at room temperature, its rate is so slow that it is negligible. The increase in temperature, as created by a match, allows the reaction to start and then it heats itself because it is [[exothermic]]. That is valid for many other fuels, such as [[methane]], [[butane]], and [[hydrogen]].

Reaction rates can be independent of temperature (''non-Arrhenius'') or decrease with increasing temperature (''anti-Arrhenius''). Reactions without an activation barrier (for example, some [[radical (chemistry)|radical]] reactions), tend to have anti-Arrhenius temperature dependence: the rate constant decreases with increasing temperature.

Many reactions take place in solution and the properties of the solvent affect the reaction rate. The [[ionic strength]] also has an effect on the reaction rate.

Electromagnetic radiation is a form of energy. As such, it may speed up the rate or even make a reaction spontaneous as it provides the particles of the reactants with more energy.{{citation needed|date=January 2019}} This energy is in one way or another stored in the reacting particles (it may break bonds, and promote molecules to electronically or vibrationally excited states...) creating intermediate species that react easily. As the intensity of light increases, the particles absorb more energy and hence the rate of reaction increases. For example, when methane reacts with [[chlorine]] in the dark, the reaction rate is slow. It can be sped up when the [[mixture]] is put under diffused light. In bright sunlight, the reaction is explosive.

The presence of a catalyst increases the reaction rate (in both the forward and reverse reactions) by providing an alternative pathway with a lower activation energy. For example, [[platinum]] catalyzes the combustion of hydrogen with oxygen at room temperature.

The [[kinetic isotope effect]] consists of a different reaction rate for the same molecule if it has different isotopes, usually hydrogen isotopes, because of the relative mass difference between hydrogen and [[deuterium]].
In [[reactions on surfaces]], which take place, for example, during [[heterogeneous catalysis]], the rate of reaction increases as the surface area does. That is because more particles of the solid are exposed and can be hit by reactant molecules.

Stirring can have a strong effect on the rate of reaction for [[Homogeneous and heterogeneous reactions|heterogeneous reactions]].

Some reactions are limited by diffusion. All the factors that affect a reaction rate, except for concentration and reaction order, are taken into account in the reaction [[rate coefficient]] (the coefficient in the rate equation of the reaction).