We’re being asked to **determine what happens as you increase the temperature to the ****reaction rate and activation energy.**

We need to use the ** two-point form of the Arrhenius Equation**:

$\overline{){\mathbf{}}{\mathbf{k}}{\mathbf{=}}{{\mathbf{Ae}}}^{\mathbf{-}\frac{{\mathbf{E}}_{\mathbf{a}}}{\mathbf{RT}}\mathbf{}}{\mathbf{}}}$

where:

**k** = rate constant

**E _{a}** = activation energy (in J/mol)

**R** = gas constant (8.314 J/mol • K)

**T** = temperature (in K)

**A** = Arrhenius constant or frequency factor

A certain reaction has an activation energy of 300 kJ/mol. As you increase the temperature the reaction rate will and the activation energy will .

A. increase; increase

B. increase; decrease

C. increase; stay the same

D. decrease; increase

E. decrease; decrease

F. decrease; stay the same

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What scientific concept do you need to know in order to solve this problem?

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