For the gas phase isomerization of methyl cis-cinnamate, cis-C6H5 CH=CHCOOCH3 → trans-C6H5 CH=CHCOOCH3 the rate constant in s¹ has been determined at several temperatures. When S In k is plotted against the reciprocal of the Kelvin temperature, the resulting linear plot has a slope of -2.09 × 104 K and a y-intercept of 24.3. The value of the rate constant for the gas phase isomerization of methyl cis-cinnamate at 667 K is s-¹. (Enter your answer to one significant figure.)

For the gas phase decomposition of t-butyl chloride, (CH3)3CC (CH3)2C=CH2 + HCI the rate constant in s has been determined at several temperatures. When In k is plotted against the reciprocal of the Kelvin temperature, the resulting linear plot has a slope of -2.08×104 K and a y-intercept of 28.6. The value of the rate constant for the gas phase decomposition of t-butyl chloride at 582 K is (Enter your answer to one significant figure.)

2 In the gas phase methyl isocyanide, H,CNC, rearranges to form ethanenitrile, H,CCN. H,C-NC H,C-CN The table below shows the experimentally determined values of the rate constant for this rearrangement at different temperatures. Temperature / °c Rate constant / s 190 2.52 x 10 199 5.25 x 10 230 6.30 х 10* 251 3.16 х 103 (a) Determine the overall order of the reaction. (b) Write the rate expression for the reaction. (c) Using a graphical method, determine the activation energy for the rearrangement of methyl isocyanide. (d) Determine the value of the rate constant for this reaction at (i) 210 °C and (ii) 283 °C.

For the gas phase isomerization of cis-cyanostyrene, cis-C6H, CH=CHCN trans-C,H,CH=CHCN the rate constant has been determined at several temperatures. When Ink in s the resulting linear plot has a slope of -2.32 x 10 K and a y-intercept of 26.7. The activation energy for the gas phase isomerization of cis-cyanostyrene is is plotted against the reciprocal of the Kelvin temperature, kj/mol.

Determine the rate law for the formation of oxygen predicted by this mechanism. (Assume the steady-state approximation is valid for any reaction intermediates.) k₁ CIO + CIO + M (CIO)₂ → CIOO + Cl (CIO)2 + sunlight k3 C100 + M k4 →→ Cl + O₂ 2x (C1 + 03 net: 2 033 0₂ → CIO + O₂) (this reaction occurs twice in the mechanism)

What are the units of the rate constant for A + B → C whose rate law is first order in A and second order in B?

The rate constant for the reaction H2(g) + I2(g) → 2HI(g) is equal to 2.40 M–1 s–1 at 355 ºC and 9.80 M–1 s–1 at 385 ºC. Using these results, estimated the value of the rate constant at 415 ºC.

I don’t know how to do this question about rate constant

In a study of the rearrangement of cyclopropane to propene at 500 °C (CH2)3 CH3CH=CH2 the concentration of (CH2)3 was followed as a function of time. It was found that a graph of In[(CH2)3] versus time in seconds gave a straight line with a slope of -9.38×104 s1 and a y-intercept of -1.57 . Based on this plot, the reaction is O order in (CH2)3 and the half life for the first reaction is seconds.

At 500 K, what is the fraction of molecular collisions with enough energy to result in a bimolecular reaction with Ea = 80 kJ mol−1?