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The 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 6.1×10^{−8} s^{−1}. What is the value of the rate constant at 845 K?

**Arrhenius Equation**

The rate of chemical reactions is a function of temperatures absolute of the system. that the chemical reaction takes place. It occurs according to the Arrhenius equation, which is described below:

k = Ae^{−}^{EA/RT}

- A is the pre-exponential factor (a constant)

- E
_{A }is the energy of activation that is the minimum amount of energy needed for the reaction to take place. - The gas constant R is the gas universal constant

To explain the reaction, we can say:

_{1 }= 6.1×10^{−8}s^{−1 }at T_{1 }= 600 K_{2}(let say) at T_{2 }= 845 K_{A }= 262 kJ/mol = 262000 J/mol.Utilizing Arrhenius equation that takes the ratio of two rate constants, we can find:

So we can have the rate constant of 845 K, which is equal to 0.25 s

^{−1}.