378.5ºC, the half-life for the first order thermal decomposition of ethylene oxide is 363 min, and the energy of activation of the reaction is 2.176 x 105 J mol-1. Estimate the time required for ethylene oxide to be 75% decomposed at 450ºC. Answer is [13.6

The decomposition of sulfuryl chloride, SO2Cl2, to sulfur dioxide and chlorine gases is a first-order reaction. It is found that at a certain temperature, it takes 1.43 hours to decompose 0.0714 M  to 0.0681 M. What is the rate constant for the decomposition?

A student obtained the following data for the gas phase decomposition of hydrogen peroxide at 400 °C. H₂O₂(g) H₂O(g) + 2 O₂(g) [H₂0₂], M seconds 0.134 0 6.70x10-² 14.2 ◊ 3.35x10-2 42.7 (1) What is the half-life for the reaction starting at t=0 s? What is the half-life for the reaction starting at t=14.2 s? Does the half-life increase, decrease or remain constant as the reaction proceeds? 1.68x10-2 99.2 (2) Is the reaction zero, first, or second order? (3) Based on these data, what is the rate constant for the reaction? S M-¹S-1

Determine half-life, order, and k from concentration-time data. The following data were collected for the gas phase decomposition of dimethyl ether at 500 °C. CH3OCH3(g)-CH₂(g) + H₂(g) + CO(g) [CH3OCH 3], M 7.02x10-² time, min 0 3.51x10-2 22.20 K 1.76x10-² 44.40 8.80×10-3 66.60 (a) What is the half-life for the reaction when [CH3OCH3] = 7.02x10-² M? (b) What is the half-life for the reaction when [CH3OCH3] = 3.51x10-² M? (c) Is the reaction first order? If so, what is the rate constant for the reaction? (If not first order leave blank). min min min-1