Consider the following reaction equation and experimental data for the questions below. C2H4+ 3 O2→2 CO2+ 2 H2O
[C2H4] - 0.018M, 0.027M, 0.027M
[O2] - 0.036M, 0.036M, 0.072M
Rate (mol L–1s–1) - 0.0260, 0.0585, 0.0585
a)Determine the experimental rate law (rate expression) for this reaction and write it out. b)How is the rate of disappearance of O2related to the rate of production of CO2?
c)At 170 °C the rate constant is 80.2 mol–1L s–1. If you start with 0.73 mol of C2H4in a 2.0 L vessel, what will the concentration of C2H4be after 3.0 min?

Why do the strengths of london (dispersion) forces generally increase with increasing molecular size? choose one: a. heavier atoms have stronger attractions for each other than lighter atoms. b. dispersion forces are all equal in magnitude; there is no size dependence. c. dispersion forces arise from the attraction between the nuclei of atoms, and larger molecules have larger nuclei. d. dispersion forces arise from dipoles caused by the electron distribution being distorted. larger molecules have more electrons and, therefore, more distortions and a bigger force. e. dispersion forces depend on distance. larger molecules are farther apart and so the forces are smaller.