# Rates Of Reaction Between Sodium Thiosulphate And Hydrochloric Acid Coursework

If you added it to the flask using a spatula, and then quickly put the bung in, you might lose some gas before you got the bung in.Alternatively, as you pushed the bung in, you might force some air into the measuring cylinder. To start the reaction, you just need to shake the flask so that the weighing bottle falls over, and then continue shaking to make sure the catalyst mixes evenly with the solution.This is repeated for a range of concentrations of the substance you are interested in.

If you added it to the flask using a spatula, and then quickly put the bung in, you might lose some gas before you got the bung in.Alternatively, as you pushed the bung in, you might force some air into the measuring cylinder. To start the reaction, you just need to shake the flask so that the weighing bottle falls over, and then continue shaking to make sure the catalyst mixes evenly with the solution.This is repeated for a range of concentrations of the substance you are interested in.

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So you would convert all the values you had for rate into log(rate). I suspect that in the unlikely event of you needing it in an exam at this level, it would be given to you. You probably have to enter 2 and then press the log button, but on some calculators it might be the other way around.

Convert all the values for [A] into log[A], and then plot the graph. All you need to do is find the log button on your calculator and use it to convert your numbers. If you do it the wrong way around, you will just get an error message.

If you were looking at the effect of the concentration of hydrogen peroxide on the rate, then you would have to change its concentration, but keep everything else constant.

The temperature would have to be kept constant, so would the total volume of the solution and the mass of manganese(IV) oxide.

Since this is the part of the reaction you are most interested in, introducing errors here would be stupid!

You have to find a way of adding the catalyst to the hydrogen peroxide solution without changing the volume of gas collected.

This could be a reaction between a metal and an acid, for example, or the catalytic decomposition of hydrogen peroxide.

If you plotted the volume of gas given off against time, you would probably get the first graph below.

The maths of this might not be familiar to you, but you may find that you are asked to do this as a part of a practical exam or practical exercise.

If it is an exam, you would probably be given help as to how to go about it.

## Comments Rates Of Reaction Between Sodium Thiosulphate And Hydrochloric Acid Coursework

• ###### Mechanism kinetics hydrochloric acid sodium thiosulfate.

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In order to get maximum marks in this coursework it is vital that you discuss all. The hydrochloric acid - sodium thiosulphate reaction depends on the time for a.…

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Nov 17, 2014. Sodium thiosulphate decomposition for GCSE, grade a easy. the rate of reaction in the reaction of sodium thiosulphate with hydrochloric acid.…

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• ###### Safety Precautions Hydrochloric acid solution is strong acid.

The reaction of sodium thiosulphate and hydrochloric acid generates sulphur. Wear chemical splash goggles for safety of eyes, temperature-resistant gloves, and. Hypothesis The higher the concentration the faster the rate of reaction will be. I was behind on Tulane coursework and actually used UCLA's materials to.…

• ###### Order of reaction experiments - Chemguide

The simplest initial rate experiments involve measuring the time taken for some. If you add dilute hydrochloric acid to sodium thiosulphate solution, you get the. but actually doing it could only reasonably be a part of a coursework exercise.…

• ###### Rate of Reaction of Sodium Thiosulfate and Hydrochloric Acid

The purpose of this demonstration is to investigate the effect of sodium thiosulfate concentration on the rate of reaction of sodium thiosulfate with hydrochloric.…