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There are two reactions ch3cooc2h5 + h2o → ch3cooh + c2h5oh and 2no +cl2 → 2nocl are proceeding at same given set of experimental conditions (same temperatur
There are two reactions CH3COOC2H5 + H2O → CH3COOH + C2H5OH and 2NO +Cl2 → 2NOCl are proceeding at same given set of experimental conditions (same temperature, and pressure etc.). Which one have high rate constant? What should be best explanation for your answer?
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1. Consider the hydrolysis of acetyl chloride (CH3COCl) to produce acetic acid (CH3COOH) and hydrochloric acid (HCl). Note: water is the solvent. CH3COCl + H2O → CH3COOH + HCl Experimentally the rate law is found to be – d[CH3COCl]/dt = k [CH3COCl] [H2O] At the beginning of the reaction, the concentration of CH3COCl is 0.10 M. (i) At the beginning of the reaction, what is the concentration of H2 O? (ii) If the reaction proceeds to completion what is the final concentration of H2 O? (iii) If k = 1.16 x 10–3 M–1 s–1, how long will it take for the concentration of CH3 COCl to be reduced to 0.05 M? 2. The gas phase reaction of nitric oxide, NO, with chlorine, Cl2 , occurs according to the equation: 2 NO + Cl2 → 2 NOCl The experimental rate law is: (1/2) d[NOCl]/dt = k [NO]2 [Cl2] A possible reaction mechanism is: (i) 2 NO → N2O2 (fast, at equilibrium) (ii) N2O2 + Cl2 → 2 NOCl (slow) Identify the rate determining step (rds), show that this mechanism is consistent with the rate law, and express the experimental rate constant, kexp, in terms of the rate constants for the elementary processes.