SODIUM THIOSULPHATE AND HYDROCHLORIC ACID COURSEWORK

This is because temperature will affect the rate of the reaction as a higher temperature will cause an increase in the rate. Another limitation of the procedure at the start of the timing and I had to add the chemicals together and start the stopwatch. There are a few mild outliers. As well as environmental variations in temperature the reaction was exothermic and heat is produced. Sorry, but copying text is forbidden on this website! Burning and explosions are very fast reactions: Enter the email address you signed up with and we’ll email you a reset link.

Sodium Thiosulphate and Hydrochloric Acid Coursework. This shows that my data is quite accurate. Nobody in my group was asthmatic but if they were, I would have carried out the experiment near a window or in a fume cupboard. This energy gives the reactant particles enough energy to collide with enough force to break apart the bonds so that new products can be made from atoms. Click to learn more https:

Sodium Thiosulphate and Hydrochloric Acid Coursework Essay

I also made sure thjosulphate the measuring cylinder was on a level surface so that I could clearly see how much liquid I was putting in to it. This good because it shows that for every increase in concentration is a decrease in rate of reaction.

Similarly the cross used will need to be the same as a thicker cross would mean it will disappear at a different concentration of sulphur thioslphate the results will not be fair.

I used this to gauge when to stop the reaction — when the black x was obscured by the white sulphur precipitate, the timer was stopped.

Sodium Thiosulphate and Hydrochloric Acid Coursework Essay Example for Free – Sample words

A limitation of my procedure was the way in which the rate thisoulphate calculated using the disappearing cross method. This can help me identify any faults. These reactions only happen if the reacting molecules collide properly.

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There is one outlier in 2M concentration. These two acids react well with the right materials.

sodium thiosulphate and hydrochloric acid coursework

Variables An independent variable is one that is controlled by me, for example; the temperature, the time limit and hydrrochloric speed.

Reactions that happen quickly have a high rate of reaction.

sodium thiosulphate and hydrochloric acid coursework

Sodium Thiosulphate and Hydrochloric Acid Coursework. Also, it has a narrow top and so it is safer. This involves human judgement rather than a qualitative value that can be used to calculated the rate. Click here to sign up.

To conclude the results show that the rate of the reaction between Sodium Thiosulphate and Hydrochloric Acid is directly proportional to the concentration of Sodium Thiosulphate. We use cookies to give you the best experience possible. Ajd you need this or any other sample, we can send it to you via email. This fits in with my hypothesis and my data.

The reason why the actual rate constant, k, can be calculated is because hydrrochloric the experiments the change in concentration cannot be calculated. Aim My aim is to investigate how changing the concentration of reactants can change the rate of reaction between hydrochloric acid and sodium thiosulphate. On my ROR graph, there is a positive correlation.

Record the time taken, wash out the conical flask thoroughly and repeat from step 3 but using the next dilution until all the concentrations have been reacted and recorded. This is supportive of my conclusion.

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Sodium Thiosulphate + Hydrochloric Acid Coursework – GCSE Science – Marked by

This shows that as you increase the independent variable the concentrationhydrohloric other variable the time taken for the experimentwent down. I have used reliable resources to research this information and it all confirms my conclusion.

If broken clear up all glass immediately. The enthalpy change is the amount of heat absorbed or released when a chemical reaction occurs at a constant pressure. This causes a quicker reaction.

In this reaction although 2HCl molecules are needed for the reaction to take place; however from the kinetics that I found HCl has no effect on the rate and is zero order. I think that my method for my investigation is easy to follow. To calculate the rate equation and orders of the reaction I am going to use the log function:.

sodium thiosulphate and hydrochloric acid coursework

The points in the top right are quite far down so this shows a negative correlation. Wnd conical flask and all other equipment must be clean as any impurities may contaminate my experiment. The Rate of a reaction can be represented as: The bars of 1M and 2M overlap and this shows that there is no real difference.

This is the reaction I will be considering: