SODIUM THIOSULPHATE AND HYDROCHLORIC ACID COURSEWORK
If the reactants take a relatively short time to form the products, the reaction is known as a FAST one. The initial volume of water. Here is what the chemicals look like at the first stage of the experiment At this point of the experiment a chemical reaction has taken place. The reaction that takes place is as follows: The same person must do the timing and watch the cross through the top of the flask, because different people have different reaction times. In case of contact, immediately flush skin with plenty of water for at least 15 minutes and with eye contact get medical attention immediately. I ensured that the fair testing and safety details listed above were met.
There are certain factors that can affect the rate of reaction. The independent variables will be the initial volume and concentration of sodium thiosulphate, and the initial volume and concentration of hydrochloric acid. Changing the pressure In this particular investigation I am going to find out how heat affects the rate of reaction in the reaction of sodium thiosulphate with hydrochloric acid. 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. If we have any contact with a chemical, the part that has made contact should be washed immediately. What affects the rate.
I feel the results I obtained allowed me to draw a graph and come to valid conclusions and be confident about calculating the order and rate equation for this reaction. In a more concentrated solution there are more particles so collisions occur more frequently We already know that by mounting the concentration there will be greater amount of particles and this means that they are squashed up more, this will result with more collisions taking place because of the fact that there are more particles in a certain amount of area it will be easier for particles to collide with each other.
The graph shows that my prediction was correct, which was that as sodium thiosulphate and hydrochloric acid coursework concentration of Sodium Thiosulphate decreases the rate of reaction increases. This was a really useful bit of sodium thiosulphate and hydrochloric acid coursework data for some work i had to do.
Sodium Thiosulphate and Hydrochloric Acid Coursework Essay Example for Free
Rates of Reaction Length: Background information The collision theory briefly: This is because as the temperature increases, the reactant particles move more quickly. The rate of reaction is the rate of loss of a reactant or the rate of formation of a product during a sodium thiosulphate and hydrochloric acid coursework reaction. In order to provide additional evidence and extend my sodium thiosulphate and hydrochloric acid coursework to find out more and back up my conclusion I could perhaps repeat the experiment using specialist equipment.
Thank you so much!!!! Sign in or sign up and post using a HubPages Network account. The intercept of the graph is equal to logC, The rate of reaction is the rate of loss of a reactant or the rate of formation of a product during a chemical reaction.
Chemistry Coursework – Sodium Thiosulphate Topics: In some cases, like rising bread we have an actual chemical reaction where the yeast changes the food.
The hydrogen ions give hydrochloric acid its acidic properties, so that all solutions of hydrogen chloride and water have a sour taste; corrode active metals, forming metal chlorides and hydrogen; turn litmus red; neutralise alkalis; and react with salts of weak acids, forming sodium thiosulphate and hydrochloric acid coursework and the weak acids Furthermore I will measure out the volumes of both the sodium thiosulphate and hydrochloric acid to the greatest degree of accuracy I sodium thiosulphate and hydrochloric acid coursework manage.
Therefore, I will make sure that I only change the temperature of the reaction mixture and keep the volume and concentration of the sodium thiosulphate, the volume and concentration of hydrochloric acid and the pressure of all the mixtures the same.
I will also investigate if there will be a change in temperature after the reaction has occurred. My evidences were also supported by theories such as the collision theory and the kinetic theory.
Neutralize acid sodium thiosulphate and hydrochloric acid coursework with saturated sodium bicarbonate 3. In the experiment we use hydrochloric acid which reacts with the magnesium to form magnesium chloride.
Instead of using the sodium thiosulphate and hydrochloric acid coursework method I would use a light intensity machine that could measure the change in colour over a period of time and stop and start timing when it had reach a certain value. After drawing a graph of logRate against logConcentration and using the calculations in my plan, the gradient of the line gave me a value of 0. To calculate the rate equation and orders of the reaction I am going to use the log function:.
This again causes an error in the actual time period taken for the cross to disappear. Because if there is remains of chemicals on your hands and you touch your eyes with your hands it may cause temporary blind and irritation which may lead to a long term effect.
I am going to draw a graph analyse by results properly. If the results were consistent and accurate I could use them to back up my original theory. I can therefore deduce that the rate equation for this reaction is:.
Furthermore I will be careful not to spill anything and will take extra care when doing the experiment. The four main variables that affect rate are: Next I will place the conical flask on top of the cross, pour 5cm 3 of hydrochloric into the hot sodium thiosulphate solution and time how long sodium thiosulphate and hydrochloric acid coursework takes for the cross to disappear.
Digital stop watch to see how long a chemical reaction takes place. Apparatus Apparatus The apparatus I will use in this experiment are as follows: For a reaction to occur particles have to collide with each other. This shows how the power, and order of the reaction, can be found by drawing a graph of logRate against log[concentration] and the gradient of the line will give the order of the reaction. The independent variables sodium thiosulphate and hydrochloric acid coursework be the initial sodium thiosulphate and hydrochloric acid coursework and concentration of sodium thiosulphate, and the initial volume and concentration of hydrochloric acid.
The two equations can then put together to give an overall rate equation:. Take care with glass wear, such as pipettes as they are fragile and may break easily.
A grade GCSE chemistry coursework – Rates of reaction Decomposition of sodium thiosulphate
My evidence is extremely reliable, I state this because the experiment was repeated three times and this made the results even more accurate. Diagram steps of how I did the experiment.
To calculate the rate equation and orders of the reaction I am going to use the log function: