What is the activation energy for the reaction below if the rate constant is 3.46 × 10 -5 s -1 at 298 K and 9.2 x 10 -5 s -1 at 305 K:   2N 2O 5 → 2N 2O 4 + O 2

The rate constant k for a certain reaction is measured at two different temperatures: temperature k 248.0 °C 9.9 x 108 169.0 °C 9.8 x 107 Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. Round your answer to 2 significant digits. kJ E = x10 mol X S ?

Determine the activation energy, Ea, (in kJ/mol) of the decomposition reaction, CH3CHO →  CH4 + CO. k (M-1/2 s-1)       T (°C) 0.01028           940 0.0655             1380

The activation energy for a particular reaction is 102 kJ/mol. If the rate constant is 1.35 × 10-4 s-¹ at 310 K, what is the rate constant at 273 K? 1 4 7 +/- 2 LO 5 8 1/s 3 6 9 O X C x 100

A reaction having an activation energy of 55.1 kJ/mol has a rate constant of 4.2 x 10-8 s-1 when the temperature is 427. K. What is the rate constant (in s=1) when the temperature is 613. K?

Sketch a potential energy diagram for the decomposition of nitrous oxide. N2O(g) →→ N2(g) + O(g) The activation energy for the forward reaction is 171  kJ;  If the activation energy for the reverse reaction is 99 kJ, calculate the standard enthalpy change for this reaction.  Transfer all the information into an energy diagram.   label appropriately

Be sure to answer all parts. The second-order rate constant for the decomposition of nitrous oxide to nitrogen molecules and oxygen atoms has been determined at various temperatures: Determine the activation energy graphically.  k(M−1  ·  s−1) T( ° C) 1.87  ×  10−3 600 0.0113 650 0.0569 700 0.244 750

For a certain reaction, the activation energy is found to be (1.77x10^1) kJ/mol. If the rate constant is (3.6x10^-5) at (3.78x10^2) K, what is the rate constant at (6.290x10^2) K?   R = 8.314 J/Kmol;     T(K) = T(°C) + 273

Calculate the rate constant at 200.°C for a reaction that has a rate constant of  8.70 ×10−4 s−1 at 90. C and an activation energy of 53.1 kJ/mol.