Edexcel Chemistry Coursework Help Text

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Now…let's see how we'll complete your chemistry coursework: after you place an order and pay for your chemistry coursework, we'll do whatever we can to make you happy with our work. Experiment to determine the factors which affect the rate of oxidation of acidified potassium iodide solution by hydrogen peroxide. Plan as described in my preliminary introduction i intend to carry out an investigation to determine the factors which affect the rate of oxidation of acidified potassium iodide solution by hydrogen peroxide. H202 + 2ki + h2so4 k2so4 + 2h2o + i2 i intend to vary the amount of potassium iodide entered into the 100cm solution potassium iodide included in the solution. The dependant variable is time as this will vary depending on how quickly the solution turns a purple/black colour and the black cross marked on the paper below is not visible.

I intended to keep the amount of sulphuric acid constantly at 40 cm also keeping the amount of hydrogen peroxide at 15 cm and the amount of special indicator at 5 cm. In some cases where potassium iodide, sulphuric acid, hydrogen peroxide and the special indicator do not equal 100 cm. Potassium iodide is the independent variable therefore its volume must be changed in every solution. The apparatus required for this experiment consists of a stop clock, a 100 cm beaker, a 100 cm measuring cylinder, a 50 cm measuring cylinder, a 10 cm measuring cylinder and a glass rod.

Pour 40 cm of potassium iodide and 40 cm of sulphuric acid into the 100 cm measuring cylinder. Temperature will affect the experiment as the higher the temperature, the faster the particles will move therefore more movement equals more collisions. The lower the temperature the slower the particles will move therefore less movement equals fewer collisions.

At a higher temperature there will be more particles colliding with activation energy required break the initial bonds therefore the rate of the reaction will be faster. At a lower temperature there will be fewer particles colliding with activation energy required to break the initial bonds therefore the rate of the reaction will be slower. The apparatus i intend to use is suited to the experiment and will provide accurate and reliable measurements. The method i intend to follow is simple and easy to understand, allowing maximum achievement. The rate of this volume should have been much higher as the 25 cm volume had a rate of 0.029.

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