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The rate of reaction increases with temperature due to the Arrhenius equation.

The rate of a chemical reaction is the speed at which reactants are converted into products. Temperature affects the rate of reaction because it influences the kinetic energy of the particles involved. As temperature increases, the kinetic energy of the particles also increases, leading to more frequent and energetic collisions between reactant molecules. This results in a higher rate of reaction.

The Arrhenius equation is a mathematical formula that describes the relationship between temperature and the rate constant of a chemical reaction. The equation states that the rate constant (k) is proportional to the activation energy (Ea) and the temperature (T) in Kelvin. The equation is k = A * e^(-Ea/RT), where A is the pre-exponential factor, R is the gas constant, and e is the mathematical constant.

The Arrhenius equation explains why the rate of reaction increases with temperature. As temperature increases, the value of RT in the denominator of the equation decreases, making the exponential term larger. This means that the rate constant increases, leading to a higher rate of reaction. The activation energy also plays a role in the rate of reaction, as higher activation energies require more energy to overcome and therefore result in slower reactions.

In summary, the rate of reaction increases with temperature due to the Arrhenius equation, which describes the relationship between temperature and the rate constant of a chemical reaction. Understanding this relationship is important in fields such as chemistry and biology, where the rate of reaction can impact the efficiency of chemical processes and biological reactions.

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