Accessed May 23, Secondly draw a black cross onto a piece of paper which is no bigger than the base of the conical flask, place the conical flask on top of the flask. I could have use a colorimeter to identify colour changes in the products. For every one M increase, the rate for reaction increases by 2. This is because the rate is determined by the rate of the slowest step of the mechanism, known as the rate determining step. The bars for 3M, 4m and 5M do not overlap. Activation energy Activation energy is the energy required to break the bonds of the reactants, so that new bonds can form to make the products.

Keep the size of my measuring flask is the same size; this should hopefully make my experiment much fairer and accurate. I have highlighted the 2M results on my tables because it seems as though there is a problem with that set. We will write a custom sample essay on Sodium Thiosulphate and Hydrochloric Acid Coursework specifically for you. This good because it shows that for every increase in concentration is a decrease in rate of reaction. This increases the likelihood of reactants colliding properly and so increases the rate of the chemical reaction.

sodium thiosulphate and hydrochloric acid coursework

Hi there, would you like to get such a paper? Sodium Thiosulphate in Hydrochloric Acid. As soon as thiosuphate chemicals were in, I started the timer.

Sodium Thiosulphate and Hydrochloric Acid Coursework Essay

These reactions only happen if the reacting molecules collide properly. Skip to main content. The points in the top right are quite far down so this shows a negative correlation. If you contact us after hours, we’ll get back to you in 24 hours or less. This can help me identify any faults. The easiest would be using a gas syringe to measure the amount of SO2 formed.


sodium thiosulphate and hydrochloric acid coursework

Enter the email address you signed up with and we’ll email you a reset link. Therefore the slowest step in this reaction is the breakdown of 1 Sodium Thiosulphate molecules as the reaction is 1st order.

Burning and explosions are very fast reactions: I drew 6 different graphs for this investigation. To reduce errors I will need to use my preliminary results to find a volume that will give a long enough time to measure accurately, but not too long to affect the rate which is calculated by dividing initial concentration by time. In a most reactions the mechanism is not made up of one step but a series of intermediate stages where molecules form and break down.

These graphs show how if the time taken for the reaction to reach a specific concentration is too long it will not be a true reflection on the actual initial rate of the reaction. There is a time error in the time taken when the cross disappears and the delay in stopping the time. This ciursework because the rate is determined by the rate of the slowest step of the mechanism, known as the rate determining step.

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

The state symbol for sulphur dioxide is aq not g because it is dissolved in water as its original coursewogk would be too toxic and corrosive for me to use safely. I wrote down my results and then moved on to the next concentration of sodium thiosulphate. This hydrocloric would give a more quantitative results and increase the accuracy and reliability.


How about make it original? For example, rusting is a slow reaction; it has a low rate of reaction. To calculate the rate equation and orders of the reaction I am going to use the log function:.

Hydrochloric acid is colourless, poisonous and highly acidic. I had to make sure that my classmates were safe as well as myself. I have used reliable courseork to research this information and it all confirms my conclusion.

When the temperature increases the k constant will increase, this is because the molecules have more kinetic energy and there rhiosulphate a higher probability that they will collide and react.

Hi, I am Sara from Studymoose Hi there, would you like to get such a paper? Rate of Reaction and Specific Rate Constant. To try and insure the same temperature is used I will have all reactants at room temperature and carry sdoium all the reactions in one lesson. To control the temperature I could use a large water bath which could control the temperature throughout the reaction. Reactions that happen quickly have a high rate of reaction.

Remember me on this computer. I could test hydrochloroc by asking one of my peers to follow the instructions and then asking for their feedback. I think that my method for my investigation is easy to follow.