I have come to this conclusion because of several reasons. I have chosen to investigate the effect of concentration on the rate reaction. The time taken t for the mark to totally disappear indicates how fast the reaction has occurred. Give a detailed outline of any further work that could provide additional evidence for your conclusion. Here is why: Look at this diagram The perimeter of the large chip is 12 units. Retrieved 31 January 2019, from amrita. Plan Equipment · 2 Measuring cylinders · Beaker · Stopwatch · Paper with black cross on it · Sodium Thiosulphate different concentrations · same concentration each time · Water different concentrations · Pipette Prediction I predict that the greater the concentration of Sodium Thiosulphate - Reaction of Hydrochloric Acid and Sodium Thiosulphate In this investigation I am going to investigate how fast the chemicals Hydrochloric Acid and Sodium Thiosulphate react.
Now imagine increasing the number of students in the room and replaying the same scenario. For a reaction to take place two reactants must collide and the collision must have sufficient energy. The time taken t for the mark to totally disappear indicates how fast the reaction has occurred. Chemical Kinetics The study of chemical reaction rates is known as chemical kinetics. Alternative hypothesis: there is a significant statistical difference between the heights of petioles of white clover.
Do this 3 times so it is easier for you to find out the average time taken for the cross to disappear. Firstly, is the acid-base titration method which was carried out during this experiment. Perhaps a color change has occurred and, of course, no coloring agent has been added , a gas has been produced as evidenced by the formation of bubbles, energy has been transferred exothermic or endothermic , or a solid precipitate has formed upon mixing two liquids. The rate of a reaction can be commonly explained by Collision Theory… Decomposition of sodium thiosulphate Aim: The aim or purpose of this investigation is to explain how concentration affects the rate of reaction the decomposition of sodium thiosulphate in reaction with hydrochloric. Activation energy is the minimum energy required before a reaction can occur. The sulphur formed however is insoluble and exist in the mixture as a white or pale yellow precipitate or a colloid that gives a milky appearance and makes the solution opaque.
Methods The first thing that I did was prepare myself and the area around me for the practical. The graph should be a straight slopping line. There are certain factors that can affect the rate of reaction. Also when the lower concentrations were used it was detected that the cross disappears in some areas of the flask but is still visible in a corner or in a little area. Only particles with enough energy to overcome the barrier will react after colliding. Potassium dichromate oxidizes the iodide ion in acidic medium to equivalent amount of iodine.
At each collision, energy is transferred between the particles, so the particles are continually changing their energies. So how do we increase the amount of particles in a reaction? Although there are a number of ways in which we could have made the results more reliable. Distractions — I may have been distracted by something such as a loud noise and I might have looked away at the exact moment that the X disappeared. Also when a collision occu rs, there is less chance of a reaction taking place because the movement energy in the particles is less in the animation successful collisions flash yellow, unsuccessful collisions flash blue : The effect of particle size Solids with a smaller particle size e. Then draw straight line tangents to this graph at points corresponding to a variety of concentrations. Reaction between Sodium thiosulphate and Hydrochloric Acid The effect of concentration of the reactant on the rate of a reaction can be studied easily by the reaction between sodium thiosulphate and hydrochloric acid. A great way to learn about chemical reaction rates is to perform a classic experiment called the Disappearing 'X' Experiment.
This may be because my prediction was incorrect, but it may also be due to human error in the measuring of the liquids or the timing. The result may have turned out anomalous because of basic human error, or maybe because we measured the substances wrong. It is a somewhat strong acid with pK as of 0. Therefore, in order to change the rate of a particular reaction, chemists must manipulate these particle collisions, either by increasing or decreasing their frequency depending on whether they wish to increase or decrease reaction rates respectively. There is limited data on this method with few recommendations.
We must make sure that coats and bags are all out of the way while doing the experiment. After makkins sure the chemicals are properly mixed together I will place the flask over a piece of card with an x on it and time how long it takes for the x to be no longer visible. Write down the factors you want to control or monitor P6a. Molecules exceeding the activation energy collide together to initiate the reaction. However I am restricted by time and the available facilities which means I cannot repeat it.
Evaluation Overall the investigations were a success. Many, many, many, many years ago chemists came up with the concept of the mole to simplify discussion of chemical quantities: the more moles, the more particles, and vice versa. It will also make the results more credible, removing any possibility of a coincidence and will assist in reaching a conclusion. A more concentrated substance has more molecules for a given volume than a more dilute substance. This is due to the subjective nature of the experiment. The reaction between sodium thiosulphate and hydrochloric acid: Looking at the graph the order of reaction established is 1st order. Hence, based on the above theory our aim is to prepare and standardize sodium thiosulphate using potassium dichromate and potassium iodide in presence of hydrochloric acid and starch solution as indicator.
Once the temperature has been recorded, we will get all the equipment needed ready to use. It would also be preferable to wear a scientific apron, however this is not essential. It was predicted that an increase in concentration will lead to an increase in the rate of reaction. This was important because it would help to finding out the rate of reaction Next we measured out 2cm3 of hydrochloric acid solution and sodium thiosulphate in separate measuring cylinders. By combining these results, graph one was formulated. I will also investigate if there will be a change in temperature after the reaction has occurred. If the vessel is placed on a slip of paper with a large 'X' drawn on it, the time it takes for the 'X' to disappear can be measured, indicating the relative speed of the reaction.
Before the reaction starts, the mark is clearly visible from the top of the conical flask through the solution. We had to add the Sodium Thiosulphate and the water at the same time for this to be a fair test also. This can be easily done by measuring the time taken t for forming a certain amount of sulphur. Dealing with temperatures is a difficult task especially when we have to keep constant high temperatures. .