Kinetics

Rate Equations and OrderSign up

understand the terms: (i) rate of reaction; (ii) rate equation, rate = k[A]^m[B]^n where m and n are 0, 1 or 2; (iii) order with respect to a substance in a rate equation; (iv) overall order of a reaction; (v) rate constant; (vi) half-life; (vii) rate-determining step; (viii) activation energy; (ix) heterogeneous and homogeneous catalyst · be able to calculate the half-life of a reaction, using data from a suitable graph, and identify a reaction with a constant half-life as being first order

Experimental Determination of RatesSign up

be able to select and justify a suitable experimental technique to obtain rate data for a given reaction, including: (i) titration; (ii) colorimetry; (iii) mass change; (iv) volume of gas evolved; (v) other suitable technique(s) for a given reaction · understand experiments that can be used to investigate reaction rates by: (i) an initial-rate method, carrying out separate experiments where different initial concentrations of one reagent are used (a 'clock reaction' is an acceptable approximation of this method); (ii) a continuous monitoring method to generate data to enable concentration-time or volume-time graphs to be plotted · be able to deduce the order (0, 1 or 2) with respect to a substance in a rate equation, using data from: (i) a concentration-time graph; (ii) a rate-concentration graph; (iii) an initial-rate method

Mechanisms and Activation EnergySign up

understand how to: (i) obtain data to calculate the order with respect to the reactants (and the hydrogen ion) in the acid-catalysed iodination of propanone; (ii) use these data to make predictions about species involved in the rate-determining step; (iii) deduce a possible mechanism for the reaction · be able to deduce the rate-determining step from a rate equation and vice versa · be able to deduce a reaction mechanism, using knowledge of the rate equation and the stoichiometric equation for a reaction · understand that knowledge of the rate equations for the hydrolysis of halogenoalkanes can be used to provide evidence for SN1 and SN2 mechanisms for tertiary and primary halogenoalkane hydrolysis · be able to use calculations and graphical methods to find the activation energy for a reaction from experimental data (the Arrhenius equation will be given if needed) · understand the use of a solid (heterogeneous) catalyst for industrial reactions, in the gas phase, in terms of providing a surface for the reaction · CORE PRACTICALS 9a and 9b: Following the rate of the iodine-propanone reaction by a titrimetric method and investigating a 'clock reaction' (Harcourt-Esson, iodine clock) · CORE PRACTICAL 10: Finding the activation energy of a reaction