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In a study of the decomposition of hydrogen iodide on a gold surface at 150 °C HI(g) + H2(g) + 1/ 12(g) the following data were obtained: 0.133 (HI), M seconds 6.65x10-2 523 3.33x10-2 784 1.67x10-2 914 0 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 0.133 Mis 6.65x10-? Mis s and when the starting concentration is (2) The average rate of disappearance of HI from t=0 sto t= 523 s is Ms1 (3) The average rate of disappearance of HI from t = 523 s to t= 784 s is Ms? Based on these data, the rate constant for this order reaction is M5-1
For the gas phase isomerization of dimethyl citraconate, cis-(CH300C)(CH3)C=CHCOOCH3- -trans-(CH300C)(CH3)C=CHCOOCH3 the rate constant in s-1 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 -1.26x10+ K and a y-intercept of 11.5. The value of the rate constant for the gas phase isomerization of dimethyl citraconate at 650 K is (Enter your answer to one significant figure.)
The decomposition of hydrogen iodide on a gold surface at 150 °C HI(g) + H2(g) + 12 12(9) is zero order in HI with a rate constant of 1.20x10-4 M51 If the initial concentration of HI is 0.350 M, the concentration of HI will be Mafter 2.11103 seconds have passed.
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