BUT this is NOT the main reason for the increased reaction speed, so be careful in your theory explanations if investigating the effect of temperature, so read on after the pictures! When you have decided on the method, give a detailed description of how you might carry it out.
If you are confident and chosen the VARIABLE you want to investigate you should try to make a prediction and maybe justify it with some theory if you can. I will also be careful when heating up the solutions and will at all times wear safety goggles and also remain standing throughout the experiment.
The system consists of a light beam emitter and sensor connected to computer and the reaction vessel is placed between the emitter and sensor. A few health and safety ideas on risk assessment AIM for a high investigation-project mark - you have nothing to lose for your assessment!
Have you got enough results, do they seem ok? See also graphs 4. For the hydrochloric acid - sodium thiosulphate reaction think about the precipitate, observing it etc. Why does a reaction go faster at a higher temperature? Overall I think that my investigation was successful in obtaining reliable results.
Enzyme catalysed reactions e. The range of my results were also suitable to make good observations and conclusions By comparing the repeated times on each of the experiments I can see that they were similar and each one was within two seconds of each repeat.
What further experiments, using the same method or another method, could Rate of reaction coursework temperature done to support your prediction or conclusion?
As the temperature increases, the time taken for the sodium thiosulphate solution to become cloudy decreases. This means more of the particles collide and more of the collisions result in a reaction, so the rate of reaction increases. The simplest solution here, is to make sure all the chemicals have been standing in the laboratory prior to the lesson.
The light reading falls as the sulphur precipitate forms. If more experiments are conducted at another the time, the temperature must again be checked and recorded.
You can continue in a broader context by introducing some background theory and descriptions of the factors or VARIABLES which may have an effect on the rate of the reaction you are studying include briefly factors which might not apply.
The simplest solution here, is to make sure all the chemicals have been standing in the laboratory prior to the lesson. Some of the work done here in presenting the results, e. Obtaining evidence[ edit ] Observations, measurements, in other words the results! However, they will cool a little standing out in the laboratory, so not completely satisfactory solution to the problem.
Is there any other factor for the reaction you are studying? From this evidence I believe my results were very reliable. If you are varying temperature, you need to heat up the reactant solutions separately and take their temperatures, mix, start stopwatch.
If more experiments are conducted at another the time, the temperature must again be checked and recorded. To further investigate the decomposition of sodium thiosulphate I could change the concentration of hydrochloric acid and sodium thiosulphate or use a catalyst in the reaction.- Rates of Reaction Coursework.
Introduction. In this piece of science coursework I will be experimenting how the rate of reaction between Sodium thiosulphate and hydrochloric acid is affected by the concentration of Sodium thiosulphate. Enthalpy 2|Page Anjelina Qureshi Mrs Gravell Rates of Reaction Coursework Chemistry Year 11 Enthalpy, in chemistry, is the heat content in a chemical reaction.
The enthalpy change is the amount of heat absorbed or released when a chemical reaction occurs at a constant pressure. The facts. What happens?
As you increase the temperature the rate of reaction increases. As a rough approximation, for many reactions happening at around room temperature, the rate of reaction doubles for every 10°C rise in temperature. These notes on the effect of changing temperature on reaction rate, and the experimental methods and investigations involved, are designed to meet the highest standards of knowledge and understanding required for students/pupils doing GCSE chemistry, IGCSE chemistry, O Level chemistry, KS4 science courses and can be useful primer for A.
BUT you can use and extend these 'brain stormed' ideas to most rates of reaction coursework assignments e.g. The magnesium/zinc + acid reaction, you can investigate acid concentration and amount of metal and the zinc reaction is catalysed by copper and other ions in the acid).
Video created by University of Manchester for the course "Introduction to Physical Chemistry". This module explores the rate of reaction, stoichiometry and order, zero order reactions, first order reactions, second order reactions.Download