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Speed of reaction is the speed of change of reactant concentration or product in a chemical reaction per unit time. This is usually stated in the molarity per second divided by S. Speed of reaction can be influenced by various factors, including reactant concentration, temperature, pressure, and the presence of catalysts. Concentration that affects the speed of reaction is the number of moles in 1 liter of solution. The unit of concentration used is the molarity. The larger the molarity of a reactant, the faster the speed of reaction. The higher the molarity means the denser and more molecules contained. The increase in temperature accelerates the speed of reaction because the increase in temperature causes the movement of particles to be faster. This movement causes the kinetic energy of particle-by-particle to increase so that there is a greater possibility of effective growth. Catalysts make it possible for the reaction to go faster or make it possible for the reaction to be at a lower temperature due to the change in its direction towards the reaction. The wider the surface of the center, the reaction set, the easier it is to grow, effectively causing a chemical reaction, thus accelerating the speed of reaction. An increase in pressure or a smaller volume in the reaction involved in the form of a gas reaction will increase the speed of reaction. For example, a crack. The speed of reaction that happens very fast produces a loud noise, light, and heat. This happens because the crack contains mesium powder that is a chemical base. Another example is corrosion or rust. Corrosion in metal occurs due to the interaction between metal and an environment that is corrosive, namely a humid environment that contains water vapor and is induced by the presence of H2O or H2O.