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The rate of reaction increases with temperature due to increased kinetic energy, as described by the Arrhenius equation.

The rate of a chemical reaction is affected by various factors, including temperature. As the temperature increases, the kinetic energy of the reactant molecules also increases, leading to more frequent and energetic collisions between them. This results in a higher rate of reaction.

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

The activation energy is the minimum amount of energy required for a reaction to occur. As the temperature increases, the proportion of molecules with sufficient energy to overcome the activation energy barrier also increases, leading to a higher rate of reaction. The Arrhenius equation can be used to calculate the rate constant at different temperatures and to determine the activation energy of a reaction.

In summary, the rate of reaction increases with temperature due to increased kinetic energy, as described by the Arrhenius equation. This equation provides a mathematical relationship between the rate constant, activation energy, and temperature, and can be used to calculate the rate of reaction at different temperatures.

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