CHEMISTRY COURSEWORK RATE OF REACTION SODIUM THIOSULPHATE AND HYDROCHLORIC ACID

If I was using solids, I could investigate surface area and for gases I could investigate pressure In concentration I looked at five different concentration of HCl The volume of HCl stayed the same; also the volume of sodium thiosulphate stayed the same, the concentration of sodium thiosulphate stayed the same. I will investigate how the rate of this reaction is affected when the experiment is carried out at different temperatures. I will be timing and watching: My data was precise because most of the points on my graphs are close to the line and are all close by each other. The size of the error bars is quite small so I think I can say that my data is quite accurate except for the 2M result which is quite a long error bar. The results for 1, 2 and 4M keep showing outliers.

I wrote down my results and then moved on to the next concentration of sodium thiosulphate. This increases the likelihood of reactants colliding properly and so increases the rate of the chemical reaction. The conical flask and all other equipment must be clean as any impurities may contaminate my experiment. For example, rusting is a slow reaction; it has a low rate of reaction. The points in the top right are quite far down so this shows a negative correlation. Building Book Love For example.

This makes sure that my experiment runs smoothly. I stood up to allow more space for others to walk by between the rooms.

On my ROR graph, there is a positive correlation. The dependent variable was the rate of reaction. The room temperature could have affected my reaction and this could be the reason that I have some outliers. I coursework on linkedin going to investigate the effect of chemistrysodium the concentration of Sodium Thiosulphate on the rate of the reaction between Hydrochloric Xhemistry and Sodium Thiosulphate.

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This fits in with my hypothesis and my data. The page you are looking for might have been removed, had its name changed, or is temporarily unavailable. The points in the top right are quite far down so this shows a negative correlation. Rates of reaction vary depending on which chemicals are being used and the activation energy required. Oops, cuemistry could not find the requested page.

Investigating the rate of reaction between sodium thiosulphate and hydrochloric acid

In a more concentrated solution there are more particles so collisions occur more frequently. The bars for 3M, 4m and 5M do not overlap. The equation to this is as follows: Research Papers words 4. This is the reaction I will be considering: Evaluation My standard deviation sheet is attached at the back of this document marked with an asterisk. There is one outlier in 2M concentration.

(DOC) GCSE CHEMISTRY RATES OF REACTION COURSEWORK | Anjelina Qureshi –

I will investigate how the rate of this reaction is affected when the experiment is carried out at xoursework temperatures. I could have use a colorimeter to identify colour changes in the products.

For example, rusting is a slow reaction; it has a low rate of reaction. This can help me identify any faults. Click here to sign up. Nobody in my group was asthmatic but if they were, I would have carried out the experiment near a window or in a fume htdrochloric.

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Reactions that happen quickly have a high rate of reaction. I would also consider using a wider range of concentrations so I can do in-depth analysis and I can compare the two acids.

chemistry coursework rate of reaction sodium thiosulphate and hydrochloric acid

Enter the email address you signed up with and we’ll email you a reset link. To do this I would make sure that: There is five factors which affect the rate of a reaction, according to the collision theory of reacting particles: I have used reliable resources to research this information and it all confirms my conclusion. The thiosulphate equation for this is: To investigate how the concentration of hydrochloric acid thisoulphate the rate of reaction.

chemistry coursework rate of reaction sodium thiosulphate and hydrochloric acid

I tied my hair back, tucked in my tie and vhemistry all stools and bags under the desk where there is no risk of anyone tripping. I have calculated the gradient of my line to support my hypothesis and found that:

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