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Provide an example of a rate law and activation energy.

The rate law describes the relationship between the rate of a chemical reaction and the concentrations of its reactants. Activation energy is the minimum amount of energy required for a reaction to occur.

One example of a rate law is the reaction between hydrogen peroxide and iodide ions:

2H2O2 + 2I- → 2H2O + I2

The rate law for this reaction is:

Rate = k [H2O2] [I-]

where k is the rate constant and [H2O2] and [I-] are the concentrations of hydrogen peroxide and iodide ions, respectively.

Activation energy can be determined experimentally by measuring the rate of a reaction at different temperatures and using the Arrhenius equation:

k = Ae^(-Ea/RT)

where k is the rate constant, A is the pre-exponential factor, Ea is the activation energy, R is the gas constant, and T is the temperature in Kelvin.

By plotting ln(k) against 1/T, the activation energy can be calculated from the slope of the line. A higher activation energy means that the reaction requires more energy to occur and will therefore have a slower rate.

Understanding rate laws and activation energy is important in predicting and controlling chemical reactions, as well as in the development of new drugs and materials.

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