Original post by El-Taji hi basically im doing my coursework on rate of reaction Follow 3 Follow 4 Original post by El-Taji ok i have several concetrations so does that mean i use a seperate amount of magnesioum for each and just keep the amount of excess acid constant Follow 5 The amount you use for both should reain at the same throughout all repeats, if youv done your preliminaries youll find out that solid Mg is far easier to measure the rate of reaction with than powedered Youll wanna be using an excess of Mg if your measuring the rate with respect to the H2SO Follow 6 I did the same experiment at GCSE in reverse, used Sodium Thiosulphate and Hydrochloric acid to investigate rate of reaction, timed how long it took for a point underneath the beaker of HCL to no longer be visible.
Follow 7 Follow 8 Follow 9 Original post by shengoc You need to keep the magnesium constant and vary the H2SO4, or keep the H2SO4 constant and vary the magnesium. Follow 10 Original post by El-Taji That is true but you need to do both and plot a graph for both reactions and only then you can work out the orders of reaction with respect to each of those reactants.
Follow 11 Follow 12 Original post by El-Taji so are you saying the extremites? Follow 13 Chemistry Rates of Reaction Coursework: Sodium Thiosulphate and Hydrochloric Acid An investigation to show how the rate of Gcse rates of reaction coursework - ludovicgombert. Gcse rates of reaction coursework - hogaresdemadera. Chemistry coursework - The Student Room I doing gcse triple science chemistry. I am doing my coursework on rates of reaction.
Chemistry Gcse Coursework Rates of Reaction An essential element of chemistry is finding reaction rates. Chemistry work - homework - coursework - StudyZones Chemistry coursework rate of reaction help - masscot. Rates of reaction - Coursework. In this coursework I plan to investigate the effect of varying the temperature of sodium thiosulphate Below is a table to show the effect of changing different variables.
I will make sure I handle the sodium thiosulphate solution and hydrochloric acid with care. 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. Furthermore I will be careful not to spill anything and will take extra care when doing the experiment. I can see from observing the table that the first part of my prediction was correct.
As the temperature increases the rate of reaction increases too, due to more collisions and more successful collisions, caused by the increase in temperature. The graph above is the average time taken for the solution to become cloudy. It also has a line of best fit to show the consistency and accuracy of the results.
There are no anomalous results which shows that the experiment was very accurate. Furthermore, the graph is a perfect curve. It is obvious that there is a general trend in the results.
As the temperature increases, the time taken for the sodium thiosulphate solution to become cloudy decreases. This is because as the temperature increases, the reactant particles move more quickly.
In addition to this, more particles have activation energy. This means more of the particles collide and more of the collisions result in a reaction, so the rate of reaction increases.
All of my results were accurate and fitted the pattern of results. I did not have any problem whilst carrying out my investigation apart and do not believe I could have done it any better without specialist equipment with plenty of time. The quality of my evidence is good. There were no points on my scatter graph that were not on or close to the line of best fit. 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.
From this evidence I believe my results were very reliable. This might have occurred for several different reasons, such as the fact that the temperature control might not have been exactly the same or that my judgement of when the cross may have disappeared might not have been exactly the same for each one.
In order to provide additional evidence and extend my investigation to find out more and back up my conclusion I could perhaps repeat the experiment using specialist equipment. I could also change the initial volume of either the hydrochloric acid or sodium thiosulphate solution and see if I get a similar pattern of results.
If the results were consistent and accurate I could use them to back up my original theory. 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.
Sign in or sign up and post using a HubPages Network account. Comments are not for promoting your articles or other sites. Thanks so much for this! You saved my butt! Well written and very informative! This really helped me with my chemistry coursework and I used the physics one for my physics a coursework and I got an An overall thank you so much!!!! I have done the same experiment and my results are far off from what you have done, does that mean I have done it wrong.
If you did not, then you would need to write about it in your conclusion. Lani - this experiment was done 3 years ago. It can be reproduced now, so if you are doing it now, then you can use the figures in the experiement above. What grade was this? Other product and company names shown may be trademarks of their respective owners.
Initial volume 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.
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.
- Rate of Reaction Coursework Aim: To investigate how temperature affects rate of reaction. Introduction: I am going to investigate how temperature affects the rate of reaction of hydrochloric acid with calcium carbonate. Chemistry Plan I am going to produce a piece of coursework investigating the rate of reaction, selecting a variable to see how this affects the rate. The rate of reaction is the rate of loss of a reactant or the rate of formation of a product.
This online chemistry coursework rate of reaction help catalog works best on a desktop computer with an updated web browser. chemistry coursework rate of reaction help 1. Unsacramental irresistibility grill dissertation consulting service juridique ahead of whomever reexchanged hotbed. Chemistry Rates of Reaction Coursework In: Science Submitted By karthiksree3 GCSE Chemistry Coursework: Rates of Reaction Chemistry Table of Contents The reaction rate or rate of reaction for a reactant or product in a particular reaction is intuitively defined as how fast a reaction takes place. For example, the oxidation of .