If a reaction's rate constant at 298K is 33 M-1s-1 and 45 M-1s-1 at 675 K, what is the activation energy?

The reaction 2A--->P has a rate constant k= 3.50 x 10-4 dm6 mol-2s-1What is the order of this reaction? Why?

For the gas phase decomposition of t-butyl acetate, CH3COOC(CH,))3– 3/3 (CH,)2C=CH, + CH,COOH 3/2 the rate constant has been determined at several temperatures. When In k in s is plotted against the reciprocal of the Kelvin temperature, the resulting linear plot has a slope of -2.04×104 K and a y-intercept of 30.7. The activation energy for the gas phase decomposition of t-butyl acetate is kJ/mol.

A gas phase reaction has a rate coefficient of 1.3·104 L mol–1s–1 at 300 K and its activation energy is 8.3 kJ mol–1. Indicate the order of the reaction.

The activation energy for a given reaction equals 1.0 x 105 J/mol. If k = 2.5 x 10-3 sec-1 at 332 K, what is k at 375 K?

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

1. The following data was obtained from decomposition of nitrogen oxide (NO). 2HX H2 + X2 T(K) 703 733 759 791 811 836 865 k (L mol-¹s-¹) Find; 0.011 0.035 0.105 0.343 0.790 2.14 4.95 (a) The activation energy, Ea. (b) The Arrhenius constant, A (c) The collision frequency, ZAA (d) The following mechanism was suggested for the reaction. Is the mechanism meet with the order of reaction? X₂ = X + X X + H2 H + XH + HX2 X + H₂ Fast Slow Fast

A reaction has an activation energy of 15 kJ mol-1. The temperature of the reaction must be increased from 300 K to what temperature, in K, in order for the reaction rate to double? 394 339 278 323 350.

Be sure to answer all parts. Use the data in the following table to determine the activation energy of the reaction: T(K) k (s-1) 625 1.1 × 10-4 635 1.5 x 10-4 645 2.0 x 10-4 kJ/mol