The problem gave us the values for activation energy, 2 temperatures, and 1 rate constant k. Now it asks us another k value at a certain temperature. Based on these, we can say that we would need to use the **2 point form of the Arrhenius equation. **

The following reaction has an activation energy of 262 kJ/mol.

C_{4}H_{8}(g) → 2C_{2}H_{4}(g)

At 600.0 K the rate constant is 6.1 x 10^{-8} s^{-1}. What is the value of the rate constant at 725.0 K?

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