Observations, measurements, in other words the results! Possibly some data you might have been given secondary data. Repeat corrected gas volume??? All experiments should be repeated where time allows checking for accuracy and consistency; this may become more necessary after you have done a preliminary analysis The 'bung effect'! Your recorded results should indicate the accuracy of the measuring equipment e. Some of the work done here in presenting the results, e. Have you got enough results, do they seem ok?
Starting the analysis as soon as possible will help you decide whether further, wider ranging or repeat experiments - best decided after examining the graphs of results see below - difficult to decide just looking at tables of data. The results are initially processed into graphical form 'graphing' for several reasons for both the analysis and evaluating the experimental It is best, if possible, to have all the average results points plotted on the same graph for easy comparison - take care because this may involve 4 or 5 lines for 4 or 5 different acid concentrations Make sure you use a clear KEY for the different line points and a clear title for the graph AND clearly label the axis including the units or whatever..
Use smooth 'best curves' for as many of the points as possible, though some parts of the graph might be linear, watch out for the 'scatter' - the experiment is not that easy to get good results.
From the graph you can then describe in words what the results mean, always refer to the graph lines and gradients directly - don't make vague comments. So what we are after is the main 'trend s ' or 'pattern s ' describing with reference to the graphs.
Does the 'trend' of all the graph lines support you're your prediction, are all the results consistent with your prediction AND theory? For different the acid concentrations you can do a 2nd and more advanced graphical analysis of the limestone results.
This involves measuring from the graph, the speed of the reaction at the start. Explain why best data at the start? What graph could you then plot? We are basically talking about plotting the initial rate versus e. If you are doing something like the hydrochloric acid - sodium thiosulphate reaction, your reaction time measures the formation of a fixed amount of sulphur per 'time'.
From this graph re-discuss your findings in a more mathematical way and relate this to the particle collision theory of reactions! It's all about chance! How good are your results then? Do your results seem consistent and accurate?
Discuss possible sources of error which might lead to inconsistent results i. Do think the results are reliable bearing in mind any anomalies? For the hydrochloric acid - sodium thiosulphate reaction think about the precipitate, observing it etc. What further experiments, using the same method or another method, could be done to support your prediction or conclusion?
In other words give some detailed ideas on further work that would provide additional relevant evidence. The system consists of a light beam emitter and sensor connected to computer and the reaction vessel is placed between the emitter and sensor. The light reading falls as the sulphur precipitate forms. On the advanced gas calculations page, temperature sources of error and their correction are discussed in calculation example Q4b.
From Wikibooks, open books for an open world. A Wikibookian has nominated this page for cleanup. You can help make it better. Please review any relevant discussion. Rates of Reaction Coursework Aim: To find out how different concentrations of sodium thiosulphate Na S2 O3 affects the speed. The rate of reaction is the rate I also predict that as the concentration of the sodium thiosulphate increases the rate of Sodium Thiosulphate Coursework Rates of Reaction — Study Guide — Rates of Reaction Coursework Aim: Sodium Thiosulphate And Hydrochloric Acid Coursework A kinetic study of the reaction between aqueous sodium — Rates of Reaction — Sodium Thiosulphate and Sodium Thiosulphate CourseworkThe Coursework on Help with rates of reaction coursework Hydrochloric acid and I am doing coursework on the rate of reaction between Hydrochloric acid and Sodium Thiosulphate To avoid confusing I will describe the test I tried and then will tell the problems I had.
From Wikibooks, For the hydrochloric acid — sodium thiosulphate reaction you can plot either i reaction time, or Disappearing X Experiment. Coursework about sodium Disappearing X ExperimentIntroductionI am going to investigate the rate of reaction between sodium thiosulphate thio and hydrochloric acid.
In addition I am also checking how different variables affect my experiment and also how I can make my test more precise, reliable and accurate. Rates of reaction deals with the 1.
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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.
- 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.
- The Rate of Reaction Introduction ===== The rate of reaction is how fast/the speed at which a chemical reaction takes place. The rate of reaction is found by measuring the amount of a reactant used up per unit of time or the amount of . Rates of reaction: sodium thiosulphate hydrochloric acid Rates of reaction: sodium thiosulphate hydrochloric acid Plan: We must produce a piece of coursework investigating the rates of reaction, and the effect that changing one particular variable has on A grade GCSE chemistry coursework – Rates of reaction A grade GCSE .
The rate of a chemical reaction is a measure of how fast the reaction takes place. It is important to remember that a rapid reaction is completed in a short period of time. An example of a fast reaction is an explosion, and an example of a slow reaction is rusting/5(2). The rate of reaction is the rate of loss of a reactant or the rate of formation of a product. The rate is measured by dividing one by the time the reaction took to take place.