A reaction with an activation energy of 43.3 kJ/mol has a rate constant of 0.351 s1 at 330 K. At what temperature, in K, will the rate constant for the reaction be 0.0117 s 1? Your Answer: Answer units

For the reaction, 2N₂O5(g) The following data were obtained: T = 339 K [N₂O), M 1.00 × 10 Time 0 100 300 600 900 a. 45.8 kJ/mol b. 120.6 kJ/mol 112.5 kJ/mol 95.7 kJ/mol 68.5 kJ/mol 89.7 kJ/mol 4NO2(g) + O2(g) C. d. e. f. *10² 2.33 - 10- 5.41- 10¹ 1.26 × 10¹ X T = 310 K [N₂Os]. M 1.00 × 10 9.54 × 10 X 8.63 10% 7.43 - 10 6.39 × 10 A T = 304 K [N₂O₂]. M Find the Ea using the best-fit straight line of the three rate constants at the three temperature values. 1.00 × 10 9.69 × 10² 9.15 × 10² 8.40 - 10 7.70 × 10²

The reaction C,H,(g) → 2 C,H,(g) has an activation energy of 262 kJ/mol. At 600.0 K, the rate constant, k, is 6.1 × 10-8 s-'. What is the value of the rate constant : 775.0 K? k = ?

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