Essay about Saponifacation of Ethyl Acetate and Soldium Hydroxide

What were we trying to accomplish with this experiment? What method did we implement to accomplish the task? What techniques were used to purify and identify the product(s) of the reaction?

The slope of this graph, calculated using the average rise / run is also 1. As [S2O8-2] is held constant during these trials, the exponent n for [I-] equals one. The k constant can now be calculated.

Abstract: From the shown calculations & graphical analysis, the experimentally determined rate law is rate = K[I-].969 [H2O2].991 and the experimentally determined activation energy is 59.50 kJ/mole.

The rate of a chemical reaction often depends on reactant concentrations, temperature, and the presence of a catalyst. Additionally, the rate law is determined mathematically only from experimental data. The reaction investigated in this experiment is:

Experiment 1: The experiment one materials and methods, are contained in Wolven, 2014; Montezuma Publishing; page 121-123. The reader is advised to refer to this manual with any questions, the experiment was completed with one amendment as the first dilution was already prepared, so, only 4 test tubes were needed to complete the rest of the procedure.

I aim to find out the activation enthalpy of the reaction by finding the rate of reaction at different temperatures using the Arrhenius Equation.

In the other test tube, 0.5mL of 0.2 M 2-chloro-2-methylpropane was added. At the same time, 1mL of 1.0 M AgNO3 in absolute ethanol was added to each test tube. Observations were recorded and rates of reactions were compared.

2. Determine the activation enthalpy with and without the catalyst ammonium molybdate(VI) and with different protic acids and use this to compare the effectiveness.

That then is the final version of the simplified equation to get the values for Kp needed in the ESVL section of the experiment.

Note that log here denotes a logarithm with base 10 (ln would denote the natural base logarithm). Since the activity coefficient for the neutral species (γHA ) is 2 equal to one and γave = γH3 O+ γA− , the Eq. (12) gives:

where the logarithm on base 10 has been converted to the "natural" logarithm. Multiplying by f , Equation (2) yields:  ε 2.51 f 0.869 ln  +  3.7 D ℜ f   =0  

Sodium hydroxide solution then added to apply a protocol and the solution was heated at 140 °C for 1 h and at 180 °C for 4 h. The alkaline hydrolysis of Gdcl3 should be carried out in substoichiometric conditions, too.

Introduction : Last academic year, towards the end, in IB chemistry hl class, my class had the chance to learn about the concentration, temperature, catalysts, etc and their effects on the rate of reaction in a chemical reaction. I knew that the rate of reaction had a relationship with the factors but I wanted to know how it changes witness it for myself. I wanted to perform an experiment for myself to see what it actually is like. This IA is potentially an opportunity for me to test my understanding on the topic and

900ml THF and 0.973moles of Potassium tertiary butoxide, was charged into 5L RB under N2 atm and stirred for 5min 0.936moles of Wittig salt was charged into the above cooled reaction mixture, colour of the reaction mixture changes to yellow. 0.749moles of acetophenone was charged using a dropping funnel and stirred at 30-40○C. TLC checked, it complies, reaction was cooled. Hexane and water charged into it and stirred for 30min at 5-8°C. The reaction mass organic layer was separated followed by its washing with hexane, water and brine, it was filtered under vacuum.

carried out in a batch reactor, where ethyl benzoate was added to a mixture of water, ethanol,