The chemical kinetics of the hydrolysis of t-butyl chloride was studied at different condition. The product concentration in this reaction can be determined by titration. The product concentration at different time intervals was recorded. The graph ln ([HCl]∞−[HCl]t) versus time was plotted in order to find the rate constant of the reaction. The rate constant was determined by obtaining the gradient of the graph. Aims: To determine the rate constant of a chemical reaction in different solvent mixtures. To observe and account for the change in reaction rates when different solvent system are used. Introduction: The hydrolysis reaction of a tertiary butyl chloride ((CH3)3C–Cl) is expected to proceed via an SN1 mechanism: (CH3)3C Cl (aq) (CH3)3C + …show more content…
Since 1 mol of NaOH can react with 1 mol of HCl during titration, n(NaOH)=n(HCl) and [HCl]=n(HCl)/0.01L=0.0410M X (Volume of NaOH used in L) / 0.01L For instance, the concentration of HCl produced after first time interval in data table 1: [HCl]15’20’’ = (0.0021 X 0.041) mol / (0.01) L = 0.00861 mol L-1 Assume the alkyl halide was completely hydrolysed, [HCl]∞ = 0.1M. ln ([HCl]∞−[HCl]t) versus time from two data table: The rate of reaction was related to the change of concentration of t-butyl chloride and hydrochloride. The rate of change of reactant equal to the rate of change of product [(CH3)3CCl]t= [HCl]∞−[HCl]t Equation 1 The rate of reaction was compared to find a linear rate versus t correlation. A constant was needed that was not related to the concentration, namely the rate constant k as shown as below: (-d〖[〖CH〗_3 CCl]〗_t)/dt=k〖[〖CH〗_3 CCl]〗_t Equation 2 The equation 2 was rearranged and integrated on both sides from 0 to t, then Equation 1 was substituted into this new equation: 〖d[〖CH〗_3 CCl]〗_t/〖[〖CH〗_3 CCl]〗_t =-k dt ln 〖[〖CH〗_3 CCl]〗_t/〖[〖CH〗_3 CCl]〗_0 =-kt ln (〖[HCl]〗_∞-〖[HCl]〗_t)/〖[HCl]〗_∞ =-kt ln[HCl]∞−[HCl]t = -kt +
Objective: The objective of the experiment is to determine what factors cause a change in speed of a reaction. It is also to decide if the change is correlated with the balanced equation of the reaction and, therefore, predictable. To obtain a reaction, permanganate, MnO_4^(1-), must be reduced by oxalic acid, C_2 O_4 H_2. The balanced equation for the reaction is:
For this experiment we have to use physical methods to separate the reaction mixture from the liquid. The physical methods that were used are filtration and evaporation. Filtration is the separation of a solid from a liquid by passing the liquid through a porous material, such as filter paper. Evaporation is when you place the residue and the damp filter paper into a drying oven to draw moisture from it by heating it and leaving only the dry solid portion behind (Lab Guide pg. 33.).
Input variables In this experiment there are two main factors that can affect the rate of the reaction. These key factors can change the rate of the reaction by either increasing it or decreasing it. These were considered and controlled so that they did not disrupt the success of the experiment. Temperature-
The purpose of the experiment is to study the rate of reaction through varying of concentrations of a catalyst or temperatures with a constant pH, and through the data obtained the rate law, constants, and activation energies can be experimentally determined. The rate law determines how the speed of a reaction occurs thus allowing the study of the overall mechanism formation in reactions. In the general form of the rate law it is A + B C or r=k[A]x[B]y. The rate of reaction can be affected by the concentration such as A and B in the previous equation, order of reactions, and the rate constant with each species in an overall chemical reaction. As a result, the rate law must be determined experimentally. In general, in a multi-step reac...
The Effect of Temperature of Hydrochloric Acid on the Rate of Reaction Between Hydrochloric Acid and Magnesium
Hydrochloric acid + calcium carbonate arrow calcium chloride + carbon dioxide + water. HCl(aq) + CaCO3(s) arrow CaCl2(aq) + CO2(g) + H2O(l) Things that affect the reaction rate of this experiment are: 1. The temperature of the hydrochloric acid. 2.
The aim is to find out if changing the concentration of the hydrochloric acid solution has an effect on the time taken for the reaction. The reaction that will take place is: Hydrochloric acid + Calcium Carbonate + Calcium Chloride + Water + Carbon dioxide 2HCl (aq) + CaCo3 (s) CaCL2 (aq) + H2O + CO2 (g). Collision theory - Collisions between reactant particles are needed. for the reaction to take place in order to form a product.
The Effect of Temperature on the Rate of Reaction Between Hydrochloric Acid and Calcium Carbonate
Experiment is to investigate the rate of reaction between hydrochloric acid and calcium carbonate Hydrochloric acid + Calcium Carbonate Þ Calcium Chloride + Water + Carbon Dioxide 2HCl (aq) CaCo3 (s) CaCl2(s) H2O (aq) CO2 (g) There are a number of variables in this experiment and these are listed below as input variables and outcome variables.
From looking at the results I can conclude that when the pH was 3 and
Predictions may be made about the suitability of possible catalysts by assuming that the mechanism of catalysis consists of two stages, either of which can be first:
My aim in this piece of work is to see the effect of temperature on the rate of a reaction in a solution of hydrochloric acid containing sodium thiosulphate.
[6]"The Effect of Catalysts on Rates of Reaction." Chemguide: Helping You to Understand Chemistry - Main Menu. Web. 08 Oct. 2011. .
Effect of Temperature on the Rate of Reaction between Sodium Thiosulphate and Hydrochloric Acid Investigation Chemical reactions are used in our everyday life, they literally keep us alive. They are used in food, respiration and everywhere else in the environment. A chemical reaction mainly occurs when reactants react together to produce a new product. The speed at which this reaction takes place is called the rate of reaction. The product produced has a number of particles in the solution that has formed from the reactants.
In this experiment three different equations were used and they are the Stoichiometry of Titration Reaction, Converting mL to L, and Calculating the Molarity of NaOH and HCl (Lab Guide pg. 142 and 143).