Home/ Questions/The reaction C4H8(g)⟶2C2H4(g) has an activation energy of 262 kJ/mol.
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Asked: 2022-04-11T19:35:00+00:00 In:

The reaction C4H8(g)⟶2C2H4(g) has an activation energy of 262 kJ/mol.

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

C4H8(g) ⟶ 2C2H4(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?

♦ Relevant knowledge
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)
  • EA 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
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1 Answer

  1. Best Answer

    To explain the reaction, we can say:

    • The rate at which the reaction occurs k1 = 6.1×10−8 s−1 at T1 = 600 K
    • The rate k2 (let say) at T2 = 845 K
    • The energy for activation of the reaction is  EA = 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.

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