The frequency factor for a second-order gas-phase decomposition of a species at low pressures is 2.3 × 1013 dm3 mol−1 s−1 and its activation energy is 30.0 kJ mol−1. What are (i) the entropy of activation, (ii) the enthalpy of activation, (iii) the Gibbs energy of activation at 298 K? Assume κ = 1.

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 In k is plotted against the reciprocal of the Kelvin temperature, the resulting linear plot has a slope of −2.09 × 10¹ 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.)

1) The rate constant for the gas-phase reaction H2(g) + I2(g) → 2 HI(g) has the value 4.45 x 10-5 mol-1 dm³ s-1. What is the equivalent rate constant in units of molecule-1 cm³ s- 1? 2) The kinetics of the hydrolysis of methyl methanoate, CH3COOCH3, in aqueous solution were investigated by measuring the concentration of the ester after different time intervals. The reaction was found to be first order in the concentration of the ester. Use the data below to determine the rate constant for the reaction (must provide best fit graph). 3600 time, t/s 1800 5400 7200 9000 concentration, c/ (mol dm-3) 0.300 0.191 0.135 0.081 0.055 0.035

Consider the chemical reaction described by 2A(aq) ⇌ D(aq)with rate constants k1 and k-1.  If the reaction is subject to a temperature jump, derive the equation for d[D]/dt in terms of a relaxation constant t.

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 rate constant of a chemical reaction increased from 0.100 s−1 to 3.20 s−1 upon raising the temperature from 25.0 ∘C to 55.0 ∘C . Calculate the value of (1T2−1T1) where T1 is the initial temperature and T2 is the final temperature. Express your answer numerically.

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

The rate constant for a first-order reaction is 2.66 × 10‒2 s‒1 at 298 K. What is the rate constant at 350. K if the activation energy for the reaction is 52.9 kJ/mol?