The rate constant k for a certain reaction is measured at two different temperatures temperature 376.0 °c 4.8 x 108 280.0 °C 2.3 x 10 8 Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. Round your answer to 2 significant digits. kJ x10 mol
1 answer:
Answer:
The activation energy for this reaction = 23 kJ/mol.
Explanation:
Using the expression,
Where,
is the activation energy
R is Gas constant having value = 8.314×10⁻³ kJ / K mol
The conversion of T( °C) to T(K) is shown below:
T(K) = T( °C) + 273.15
So,
T = (280 + 273.15) K = 553.15 K
The conversion of T( °C) to T(K) is shown below:
T(K) = T( °C) + 273.15
So,
T = (376 + 273.15) K = 649.15 K
So,
<u>The activation energy for this reaction = 23 kJ/mol. </u>
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